{"id":168,"date":"2020-09-15T15:35:18","date_gmt":"2020-09-15T10:35:18","guid":{"rendered":"https:\/\/talib.pk\/test-preparation\/?p=168"},"modified":"2020-09-15T15:35:18","modified_gmt":"2020-09-15T10:35:18","slug":"1st-year-chemistry-electrochemistry-mcqs","status":"publish","type":"post","link":"https:\/\/talib.pk\/test-preparation\/1st-year-chemistry-electrochemistry-mcqs\/","title":{"rendered":"1st Year Chemistry Electrochemistry 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>You can get 1st Year Chemistry Electrochemistry MCQs here if you are searching for the MCQs of Entry Test. This chapter is very important for Entry Test. When we talk about Electrochemistry, we first study oxidation and reduction. Then the most important term which comes is Ionization. There are many electrolytic cells e.g. Down&#8217;s cell etc. Electrolysis is a specific phenomenon used in the cells. The electrodes have their own Electrode Potential. There is a complete Electrochemical series for elements. They have numerous applications. When we say about batteries, there are two types of batteries. One is Rechargeable and the other is Non-Rechargeable. Both have their own importance and products. So, this is the brief introduction of this chapter. Check the important MCQs below.<\/p>\n<h2 style=\"text-align: center;\">1st Year Chemistry Electrochemistry MCQs<\/h2>\n<p><img decoding=\"async\" loading=\"lazy\" class=\"size-full wp-image-371 aligncenter\" src=\"https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2019\/09\/Chemistry.jpg\" alt=\"1st Year Chemistry Electrochemistry MCQs\" width=\"300\" height=\"300\" srcset=\"https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2019\/09\/Chemistry.jpg 300w, https:\/\/talib.pk\/test-preparation\/wp-content\/uploads\/2019\/09\/Chemistry-150x150.jpg 150w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<h3><strong>KEY POINTS<\/strong><\/h3>\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>Oxidation State and Balancing of Redox Equations<\/li>\n<li>Electrolytic Conduction<\/li>\n<li>Electrolytic Cells<\/li>\n<li>Voltaic and Galvanic Cells<\/li>\n<li>Electrode Potential<\/li>\n<li>Electrochemical Series<\/li>\n<li>Rechargeable Batteries<\/li>\n<li>Non-Rechargeable Batteries<\/li>\n<\/ul>\n<\/div>\n\t\t\t<\/div><\/div>\n<p>&nbsp;<\/p>\n<p><strong><span style=\"color: #ff6600;\">Question#1<\/span>. Magnesium metal is extracted by the electrolysis of its:<\/strong><\/p>\n<p>A concentrated aqueous solution of its chloride<br \/>\nDilute aqueous solution on of its chloride<br \/>\nIts fused chloride<br \/>\nAny solution<\/p>\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>Its fused chloride<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#2<\/span>. Iron can be prevented from rusting by:<\/strong><\/p>\n<p>Connecting iron to more electropositive metal, a case of cathodic protection<br \/>\nConnecting iron to more electropositive metal, a case of anodic protection<br \/>\nConnecting iron to less electropositive metal, a case of anodic protection<br \/>\nConnecting iron to less electropositive metal, a case of cathodic protection<\/p>\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>Connecting iron to more electropositive metal, a case of anodic protection<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#3<\/span>. Standard hydrogen electrode has an arbitrarily fixed potential of:<\/strong><\/p>\n<p>0 V<br \/>\n0.1 V<br \/>\n1.0 V<br \/>\n0.001 V<\/p>\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 V<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#4<\/span>. The correct order of equivalent conductance at infinite dilution among LiCl, NaCl, and KCl is:<\/strong><\/p>\n<p>LiCl &gt; NaCl &gt; KCl<br \/>\nNaCl &gt; KCl &gt; LiCl<br \/>\nKCl &gt; NaCl &gt; LiCl<br \/>\nLiCl &gt; KCl &gt; NaCl<\/p>\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>KCl &gt; NaCl &gt; LiCl<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#5<\/span>. Electrochemical series is useful in:<\/strong><\/p>\n<p>Prediction of the feasibility of a chemical reaction<br \/>\nCalculation of voltage<br \/>\nComparison of the relative tendencies of the metals and non-metals to get oxidized or reduced<br \/>\nAll of the above<\/p>\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#6<\/span>. A normal aluminum electrode coupled with a normal hydrogen electrode gives an emf of 1.66 volts and deflection of the needle towards Hydrogen. The standard electrode potential of aluminum is:<\/strong><\/p>\n<p>-1.66 V<br \/>\n-0.83 V<br \/>\n+1.66 V<br \/>\n+0.83 V<\/p>\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>-1.66 V<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#7<\/span>. If the sum of E<sup>o <\/sup>values of the two half cells is negative, then:<\/strong><\/p>\n<p>The reaction will be feasible<br \/>\nThe reaction may or may not be feasible<br \/>\nThe reaction will not be feasible<br \/>\nNo prediction can be made<\/p>\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>The reaction will not be feasible<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#8<\/span>. Which of the following cell can convert chemical energy directly into electrical energy:<\/strong><\/p>\n<p>Mercury cell<br \/>\nLead storage battery<br \/>\nDaniel cell<br \/>\nFuel cell<\/p>\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>Fuel cell<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#9<\/span>. In a galvanic cell, the electrode occupying a lower position in the electrochemical series:<\/strong><\/p>\n<p>Will act as a cathode<br \/>\nThe reduction will take place on it<br \/>\nOxidation will take place on it<br \/>\nBoth a and b<\/p>\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>Both a and b<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#10<\/span>. Which of the following statement is true about galvanic cell:<\/strong><\/p>\n<p>The anode is positively charged<br \/>\nThe cathode is positively charged<br \/>\nReduction occurs at the anode<br \/>\nReduction occurs at the cathode<\/p>\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>Reduction occurs at cathode<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#11<\/span>. Greater the value of the standard reduction potential of the given species:<\/strong><\/p>\n<p>Greater is its tendency to accept electrons to undergo reduction<br \/>\nGreater is its tendency to accept electrons to undergo oxidation<br \/>\nGreater is its tendency to lose electrons to undergo reduction<br \/>\nGreater is its tendency to lose electrons to undergo oxidation<\/p>\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>Greater is its tendency to accept electrons to undergo reduction<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#12<\/span>. Coinage metals have the least reactivity because they have:<\/strong><\/p>\n<p>Positive oxidation potentials<br \/>\nZero oxidation potentials<br \/>\nPositive reduction potentials<br \/>\nZero reduction potentials<\/p>\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>Positive reduction potentials<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#13<\/span>. Which of the following is a secondary cell:<\/strong><\/p>\n<p>Dry cell<br \/>\nNi-Cd cell<br \/>\nMercury cell<br \/>\nAlkali cell<\/p>\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>Ni \u2013 Cd cell<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#14<\/span>. Four metals A, B, C, and D are having standard electrode potential as -3.05, -1.66, -0.4, and 0.8V respectively. Which one will be the best reducing agent:<\/strong><\/p>\n<p>A<strong><br \/>\n<\/strong>B<br \/>\nC<br \/>\nD<\/p>\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<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#15<\/span>. The oxidation potential of Mg and Al are +2.37 and 1.66V, respectively. The Mg is a chemical reaction:<\/strong><\/p>\n<p>Will be replaced by Al<br \/>\nWon&#8217;t be able to replace Al<br \/>\nWill replace Al<br \/>\nNone of the above<\/p>\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>Will replace Al<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#16<\/span>. Which can replace hydrogen from dilute acids?<\/strong><\/p>\n<p>Au<br \/>\nZn<strong><br \/>\n<\/strong>Pt<br \/>\nNone of these<\/p>\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>Zn<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#17<\/span>. The oxidation state of carbon-atom in glucose is:<\/strong><\/p>\n<p>+4<br \/>\n+6<br \/>\n-4<br \/>\nNone of these<\/p>\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>None of these<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#18<\/span>. The cell in which electrical energy is converted into chemical energy is:<\/strong><\/p>\n<p>Galvanic cell<br \/>\nElectrolytic cell<br \/>\nVoltaic cell<br \/>\nAll of these<\/p>\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>Electrolytic cell<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#19<\/span>. The ability of elements to act as reducing agent _________ down to electrochemical series.<\/strong><\/p>\n<p>Increases<br \/>\nRemain constant<br \/>\nDecreases<strong><br \/>\n<\/strong>Depends upon the reaction conditions<\/p>\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>Decreases<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#20<\/span>. If a strip of Cu-metals is placed in a solution of FeSO<sub>4<\/sub> then:<\/strong><\/p>\n<p>Cu will be deposited<br \/>\nCu and Fe both dissolve<br \/>\nFe is precipitated<br \/>\nNo reaction occur<\/p>\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>No reaction occur<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#21<\/span>. \u201cAl\u201d metal is extracted from its ________ during electrolysis.<\/strong><\/p>\n<p>Chlorides<br \/>\nCryolite<br \/>\nOxides<br \/>\nAll of these<\/p>\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>Oxides<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#22<\/span>. Halogens are placed at the lower level of electrochemical series, this indicates that:<\/strong><\/p>\n<p>Halogens are good reducing agents<br \/>\nHalogens are an oxidizing agent but bad reducing agents<br \/>\nHalogens are good oxidizing agent as well as good reducing agents<br \/>\nAll the above statements are correct<\/p>\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>Halogens are oxidizing agent but bad reducing agents<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#23<\/span>. The electrolysis product of molten NaCl at electrodes:<\/strong><\/p>\n<p>Na and Cl<sub>2<\/sub><br \/>\nNa and NaOH<br \/>\nH<sub>2<\/sub> and Cl<sub>2<\/sub><br \/>\nH<sub>2<\/sub>, Cl<sub>2<\/sub>, and NaOH<\/p>\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>Na and Cl<sub>2<\/sub><\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#24<\/span>. SHE acts as an anode when connected with Cu electrode but cathode with Zn electrode because:<\/strong><\/p>\n<p>Zn has less reduction potential than hydrogen and Cu more<br \/>\nZn has less oxidizing potential than hydrogen and Cu more<br \/>\nZn is above in electrochemical series than hydrogen and Cu below<br \/>\nAll the above are possible reasons<\/p>\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>Zn has less reduction potential than hydrogen and Cu more<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#25<\/span>. When an element is in contact with 1M aqueous solution of its own ions, at 298K then the potential is called?<\/strong><\/p>\n<p>Standard reduction potential<br \/>\nReduction potential<br \/>\nStandard electrode potential<br \/>\nBoth a and c<\/p>\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>Both a and c<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#26<\/span>. Gold and silver are the least reactive due to:<\/strong><\/p>\n<p>Positive oxidation potential<br \/>\nZero oxidation potential<br \/>\nPositive reduction potential<br \/>\nHaving a large negative electrode potential<\/p>\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>Positive reduction potential<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#27<\/span>. During the electrolysis of aqueous KNO<sub>3<\/sub>, H<sub>2<\/sub> is produced at cathode instead of potassium due to:<\/strong><\/p>\n<p>The reduction potential of K is greater than hydrogen<br \/>\nHydrogen is more reactive than potassium<br \/>\nThe reduction potential of potassium is less than hydrogen<br \/>\nAll of the above are possible reasons<\/p>\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>Reduction potential of potassium is less than hydrogen<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#28<\/span>. Which of the following statement is correct?<\/strong><\/p>\n<p>Zn can replace Cu<sup>2+<\/sup> in CuSO<sub>4<\/sub><br \/>\nCu can replace H<sup>+ <\/sup>in H<sub>2<\/sub>SO<sub>4<\/sub><br \/>\nCu can replace Zn<sup>2+<\/sup> in ZnSO<sub>4<\/sub><br \/>\nNone of these<\/p>\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>Zn can replace Cu<sup>2+<\/sup> in CuSO<sub>4<\/sub><\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#29<\/span>. In a reaction Zn + HNO<sub>3<\/sub> \u2192 Zn(NO<sub>3<\/sub>)<sub>2<\/sub> + NO + H<sub>2<\/sub>O:<\/strong><\/p>\n<p>Zn is reduced<br \/>\nN is oxidized<br \/>\nN is reduced<br \/>\nHydrogen is reduced<\/p>\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>N is reduced<\/strong>\n\t\t\t<\/div><\/div>\n<p><strong><span style=\"color: #ff6600;\">Question#30<\/span>. Which one metal shows the maximum oxidation state?<\/strong><\/p>\n<p>Mn<strong><br \/>\n<\/strong>Ag<br \/>\nCr<br \/>\nHg<\/p>\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>Mn<\/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>You can get 1st Year Chemistry Electrochemistry MCQs here if you are searching for the MCQs of Entry Test. This chapter is very important for Entry Test. When we talk about Electrochemistry, we first study oxidation and reduction. Then the most important term which comes is Ionization. There are many electrolytic cells e.g. Down&#8217;s cell &hellip;<\/p>\n","protected":false},"author":2,"featured_media":371,"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\/168"}],"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=168"}],"version-history":[{"count":0,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/posts\/168\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/media\/371"}],"wp:attachment":[{"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/media?parent=168"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/categories?post=168"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/talib.pk\/test-preparation\/wp-json\/wp\/v2\/tags?post=168"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}