{"id":170,"date":"2020-09-15T14:53:35","date_gmt":"2020-09-15T09:53:35","guid":{"rendered":"https:\/\/talib.pk\/test-preparation\/?p=170"},"modified":"2020-09-15T14:53:35","modified_gmt":"2020-09-15T09:53:35","slug":"1st-year-chemistry-reaction-kinetics-mcqs","status":"publish","type":"post","link":"https:\/\/talib.pk\/test-preparation\/1st-year-chemistry-reaction-kinetics-mcqs\/","title":{"rendered":"1st Year Chemistry Reaction Kinetics MCQs"},"content":{"rendered":"<div class=\"28d95f43054b69d67289d6316e9506d8\" data-index=\"1\" style=\"float: none; margin:12px 0 12px 0; text-align:center;\">\n<script async src=\"\/\/pagead2.googlesyndication.com\/pagead\/js\/adsbygoogle.js\"><\/script>\r\n<!-- talib-new -->\r\n<ins class=\"adsbygoogle\"\r\n     style=\"display:block\"\r\n     data-ad-client=\"ca-pub-3438155045791616\"\r\n     data-ad-slot=\"6774242552\"\r\n     data-ad-format=\"auto\"><\/ins>\r\n<script>\r\n(adsbygoogle = window.adsbygoogle || []).push({});\r\n<\/script>\n<\/div>\n<p>On this page, we are going to share 1st Year Chemistry Reaction Kinetics MCQs with the students. You can prepare for the entry test accordingly. In Reaction Kinetics, the characteristics of Chemical reactions and the factors affecting them are studied. Every reaction has its rate, which defines its progress speed concerning time. In chemical reactions, the Half-Period took great importance. The rate of Chemical reaction is determined by a unique formula. Some physical and chemical methods are also used for this purpose. Activation energy plays an important part in reactions. Many factors affect the rate of reactions. Catalysts play a unique role in chemical reactions. They make the reaction quite efficient. So, this is a brief introduction to this chapter. Check the important MCQs with their answers given below.<\/p>\n<h2 style=\"text-align: center;\">1st Year Chemistry Reaction Kinetics MCQs<\/h2>\n<p><img decoding=\"async\" loading=\"lazy\" class=\"size-full wp-image-351 aligncenter\" src=\"https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2020\/09\/Chemistry.jpg\" alt=\"1st Year Chemistry Reaction Kinetics MCQs\" width=\"300\" height=\"300\" srcset=\"https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2020\/09\/Chemistry.jpg 300w, https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2020\/09\/Chemistry-150x150.jpg 150w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p><strong>KEY POINTS<\/strong><\/p>\n<div class=\"box info  alignleft\" style=\"width:100%\"><div class=\"box-inner-block\"><i class=\"fa tie-shortcode-boxicon\"><\/i>\n\t\t\t\n<div class=\"lightbulb tie-list-shortcode\">\n<ul>\n<li>Rate of Reactions<\/li>\n<li>Orders of reaction<\/li>\n<li>Half-Life period<\/li>\n<li>Determination of Rate of Chemical Reaction<\/li>\n<li>Physical and Chemical methods<\/li>\n<li>Energy of Activation<\/li>\n<li>Finding order of reaction<\/li>\n<li>Factors affecting the rate of reactions<\/li>\n<li>Catalysis<\/li>\n<\/ul>\n<\/div>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#1<\/span>. The activation energy of reaction:<\/strong><\/p>\n<ul>\n<li>Includes the average kinetic energy of the reactants<\/li>\n<li>Is in addition to the average kinetic energy of the reactants<\/li>\n<li>Is in addition to the average kinetic energy of the products<\/li>\n<li>Required for effective collisions<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Required for effective collisions<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#2<\/span>. E<sub>a<\/sub> appears as a potential energy hill between _________ for carrying out the reaction:<\/strong><\/p>\n<ul>\n<li>Among the reactants<\/li>\n<li>Reactants and the products<\/li>\n<li>Among the products<\/li>\n<li>None of the above<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Reactants and the products<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#3<\/span>. The slope of the curve between 1\/T and log k gives:<\/strong><\/p>\n<ul>\n<li>Reaction rate<\/li>\n<li>Both of the above<\/li>\n<li>Specific rate constant<\/li>\n<li>Activation energy<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Activation energy<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#4<\/span>. The unit of the rate constant is the same as that of the rate of reaction in:<\/strong><\/p>\n<ul>\n<li>1<sup>st<\/sup> order reaction<\/li>\n<li>Zero-order reaction<\/li>\n<li>2<sup>nd<\/sup> order reaction<\/li>\n<li>3<sup>rd<\/sup> order reaction<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Zero-order reaction<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#5<\/span>. Arrhenius equation can be used for evaluating:<\/strong><\/p>\n<ul>\n<li>Specific rate constant<\/li>\n<li>Both of the above<\/li>\n<li>Activation energy<\/li>\n<li>Half-life period<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Activation energy<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#6<\/span>. A catalyst can:<\/strong><\/p>\n<ul>\n<li>Accelerate the reaction rate<\/li>\n<li>Retard the reaction rate<\/li>\n<li>Chemically un-consumed at the end of the reaction<\/li>\n<li>All of the above<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>All of the above<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#7<\/span>. The 2<sup>nd<\/sup> order reaction becomes 1<sup>st<\/sup> when:<\/strong><\/p>\n<ul>\n<li>One of the reactants is limiting<\/li>\n<li>One of the reactants is in large excess<\/li>\n<li>None of the reactants is in large excess<\/li>\n<li>One of the reactants is acidic<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>One of the reactants is in large excess<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#8<\/span>. Oxidation of SO<sub>2(g)<\/sub> in the presence of NO<sub>(g)<\/sub> catalyst is an example of:<\/strong><\/p>\n<ul>\n<li>Homogeneous catalysis<\/li>\n<li>Autocatalysis<\/li>\n<li>Heterogeneous catalysis<\/li>\n<li>Negative catalysis<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Homogeneous catalysis<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#9<\/span>. Oxidation of SO<sub>2(g)<\/sub> in the presence of V<sub>2<\/sub>O<sub>5(s)<\/sub> is an example of:<\/strong><\/p>\n<ul>\n<li>Homogeneous catalysis<\/li>\n<li>Autocatalysis<\/li>\n<li>Heterogeneous catalysis<\/li>\n<li>Negative catalysis<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Heterogeneous catalysis<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#10<\/span>. Which one of the following is not a characteristic of a catalyst:<\/strong><\/p>\n<ul>\n<li>It is specific in its action<\/li>\n<li>Provides the reactants a low activation energy barrier<\/li>\n<li>Becomes chemically changed at the end of a reaction<\/li>\n<li>It can be poisoned by an impurity which deactivates its catalytic capability<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Becomes chemically changed at the end of a reaction<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#11<\/span>. The specific rate constant of a chemical reaction is the rate of the reaction when the concentration of the reactant is:<\/strong><\/p>\n<ul>\n<li>Less than unity<\/li>\n<li>Greater than unity<\/li>\n<li>Equal to unity<\/li>\n<li>Equal to the concentration of 2<sup>nd<\/sup> order reaction<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Equal to unity<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#12<\/span>. The half life for a 1<sup>st<\/sup> order decomposition of a substance dissolved in CCl<sub>4<\/sub> is 2.5 hours at 30\u00b0C. The amount of substance left after 10 hours if the initial weight of the substance is 160g:<\/strong><\/p>\n<ul>\n<li>5g<\/li>\n<li>15g<\/li>\n<li>10<strong><br \/>\n<\/strong><\/li>\n<li>20g<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>10<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#13<\/span>. An endothermic reaction A \u2192 B has an activation energy 15kcal \/mol and the heat of reaction 5kcal\/mol. The activation energy for the reaction B \u2192 A will be:<\/strong><\/p>\n<ul>\n<li>20kcal\/mol<\/li>\n<li>10kcal\/mol<\/li>\n<li>15kcal\/mol<\/li>\n<li>None of the above<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>10kcal\/mol<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#14<\/span>. The rate of reaction is doubled for every 10\u00b0C rise in temperature. The increase in reaction rate as a result of temperature rise from 10\u00b0C to 100\u00b0C is:<\/strong><\/p>\n<ul>\n<li>112<\/li>\n<li>400<\/li>\n<li>512<strong><br \/>\n<\/strong><\/li>\n<li>614<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>512<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#15<\/span>. For the 1<sup>st<\/sup> order decomposition reaction 2N<sub>2<\/sub>O<sub>5<\/sub> (g) \u2192 4NO<sub>2(g)<\/sub> + O<sub>2(g)<\/sub> the half-life is given as:<\/strong><\/p>\n<ul>\n<li>0.693\/k<\/li>\n<li>log2\/k<\/li>\n<li>0.693\/2k<\/li>\n<li>ln2\/k<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>0.693\/k<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#16<\/span>. Which one of the following is correct about the following reaction if the iron is not 100% pure?<\/strong><br \/>\n<strong>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 2Fe + 3H<sub>2<\/sub>O + O<sub>2<\/sub> \u2192 Fe<sub>2<\/sub>O<sub>3<\/sub>.3H<sub>2<\/sub>O<\/strong><\/p>\n<ul>\n<li>Very fast reaction<\/li>\n<li>Moderately reaction<\/li>\n<li>Very slow reaction<\/li>\n<li>Not predicted<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Very slow reaction<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#17<\/span>. For a chemical reaction to occur:<\/strong><\/p>\n<ul>\n<li>The vessel shall be open<\/li>\n<li>Reacting molecules should have less energy than Ea at the time of the collision<\/li>\n<li>Reacting molecules must be properly oriented and energy more than or equal to Ea<\/li>\n<li>The reacting molecules must not collide with each other<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Reacting molecules must be properly oriented and energy more than or equal to Ea<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#18<\/span>. The reaction that involves gases, its rate does not depend upon?<\/strong><\/p>\n<ul>\n<li>Catalyst<\/li>\n<li>Partial pressure<\/li>\n<li>Temperature<\/li>\n<li>Moles dm<sup>-3<\/sup><\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Moles dm<sup>-3<\/sup><\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#19<\/span>. The mathematical relation between the rate of reaction and the concentrations of the reactants is known as the:<\/strong><\/p>\n<ul>\n<li>Rate equation<\/li>\n<li>Arrhenius equation<\/li>\n<li>Rate low<\/li>\n<li>Both a and c<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Rate low<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#20<\/span>. Which one affects the specific rate constant?<\/strong><\/p>\n<ul>\n<li>Temperature<\/li>\n<li>Concentration of reactants<\/li>\n<li>Catalyst<\/li>\n<li>All of these<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Temperature<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#21<\/span>. Which one is a chemical method for the determination of the rate of reaction?<\/strong><\/p>\n<ul>\n<li>Spectrometry<\/li>\n<li>Refractrometric method<\/li>\n<li>Dilatometric method<\/li>\n<li>Titration<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Titration<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#22<\/span>. When the concentration of a reactant in the reaction is increased by 8 times, the rate increased only by 2 times. The order of the reaction is:<\/strong><\/p>\n<ul>\n<li>1<\/li>\n<li>\u00bd<\/li>\n<li>1\/3<\/li>\n<li>2<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>1\/3<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#23<\/span>. The rate expression for a reaction A+B \u2192 products is rate = k [A]<sup>2\/3<\/sup> [B]<sup>-1\/2<\/sup> the order of reaction is:<\/strong><\/p>\n<ul>\n<li>0<\/li>\n<li>5\/2<\/li>\n<li>3\/2<\/li>\n<li>1<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>1<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#24<\/span>. If 75% of any given amount of radioactive element disintegrates in 60 min. The half life of a radioactive element is.<\/strong><\/p>\n<ul>\n<li>20 min<\/li>\n<li>30 min<\/li>\n<li>45 min<\/li>\n<li>25 min<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>30 min<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#25<\/span>. The unit of rate constant depends on?<\/strong><\/p>\n<ul>\n<li>Number of reactants<\/li>\n<li>Order of reaction<\/li>\n<li>Concentration terms<\/li>\n<li>Molecularity of reaction<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Order of reaction<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#26<\/span>. The unit of the rate constant of a second-order reaction is:<\/strong><\/p>\n<ul>\n<li>mol dm<sup>-3<\/sup> sec<sup>-1<\/sup><\/li>\n<li>mol<sup>-2<\/sup> dm<sup>+6<\/sup><\/li>\n<li>sec<sup>-1<\/sup><\/li>\n<li>mol<sup>-1<\/sup> dm<sup>+3<\/sup> sec<sup>-1<\/sup><\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>mol<sup>-1<\/sup> dm<sup>+3<\/sup> sec<sup>-1<\/sup><\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#27<\/span>. The half-life period of the zero-order reaction is equal to:<\/strong><\/p>\n<ul>\n<li>0.693\/K<\/li>\n<li>1\/Ka<\/li>\n<li>a\/2<\/li>\n<li>1.5\/Ka<sup>2<\/sup><\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>a\/2<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#28<\/span>. The influence of temperature on the reaction rate is predicted by:<\/strong><\/p>\n<ul>\n<li>Free energy change of reaction<\/li>\n<li>Arrhenius equation<\/li>\n<li>Van der Waal\u2019 equation<\/li>\n<li>Kinetic equation<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Arrhenius equation<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#29<\/span>. If the energy of the activated complex lies close to the energy of reactants, it means that reaction is:<\/strong><\/p>\n<ul>\n<li>Slow<\/li>\n<li>Endothermic<\/li>\n<li>Exothermic<\/li>\n<li>Exothermic and fast<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>Exothermic and fast<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#30<\/span>. Which of the following statements regarding a catalyst is not true?<\/strong><\/p>\n<ul>\n<li>A catalyst does not alter the equilibrium in a reversible reaction<\/li>\n<li>A catalyst can initiate the reaction which is not thermodynamically favorable<\/li>\n<li>Catalytic reactions are very specific<\/li>\n<li>A catalyst remains unchanged in composition and quantity<\/li>\n<\/ul>\n<div class=\"clear\"><\/div><div class=\"toggle close\"><h3 class=\"toggle-head-open\">Answer<i class=\"fa fa-angle-up\"><\/i><\/h3><h3 class=\"toggle-head-close\">Answer<i class=\"fa fa-angle-down\"><\/i><\/h3><div class=\"toggle-content\">\n\t\t\t<strong>A catalyst can initiate the reaction which is not thermodynamically favourable<\/strong>\n\t\t\t<\/div><\/div>\n\n<div style=\"font-size: 0px; height: 0px; line-height: 0px; margin: 0; padding: 0; clear: both;\"><\/div>","protected":false},"excerpt":{"rendered":"<p>On this page, we are going to share 1st Year Chemistry Reaction Kinetics MCQs with the students. You can prepare for the entry test accordingly. In Reaction Kinetics, the characteristics of Chemical reactions and the factors affecting them are studied. Every reaction has its rate, which defines its progress speed concerning time. In chemical reactions, &hellip;<\/p>\n","protected":false},"author":2,"featured_media":351,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":[],"categories":[4],"tags":[],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/posts\/170"}],"collection":[{"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/users\/2"}],"replies":[{"embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/comments?post=170"}],"version-history":[{"count":0,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/posts\/170\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/media\/351"}],"wp:attachment":[{"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/media?parent=170"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/categories?post=170"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/tags?post=170"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}