Question 1 :
An article made of an ordinary metal is desired to be coated with gold by electroplating, then gold has to be:
Question 3 :
What happens when an electrolysis experiment is stopped and the battery terminals are reversed?
Question 5 :
In a dry cell _______ containing a moist paste of plaster of Paris, $NH_4Cl$ and $ZnCl$ acts as
Question 6 :
If $m$ is the mass of silver deposited at the cathode by $2 A$ current flowing for $25 min$ through a silver voltameter, then the mass deposited by $1.5 A$ current flowing for $600 s$ is _________.
Question 7 :
The reaction: $PCl_3 + 3H_2C_2O_4 \rightarrow H_3PO_3 + 3CO + 3CO_2 + 3HCl$ is a disproportionation reaction.<br>If true enter 1, else enter 0.<br>
Question 8 :
All combustion reactions are oxidation-reduction reactions.<br>If true enter 1, else enter 0.<br>
Question 9 :
Assertion: $KMn{ O }_{ 4 }$ is a stronger oxidising agent than ${ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }$.
Reason: This is due to the increasing stability of the lower species to which they are reduced.
Question 10 :
The oxidant which cannot act as a reducing agent is :
Question 12 :
Assertion: The reaction, $P_{4}+3NaOH+3H_{2}O\rightarrow 3NaH_{2}PO_{2}+PH_{3}$, is a disproportionation reaction.
Reason: In a disproportionation reaction, neither oxidation nor reduction takes place.
Question 13 :
The number of mole of ferrous oxalate oxidized by one mole of $KMnO_4$ is
Question 14 :
$Cu^+$ undergoes disproportionation to $Cu$ and $Cu^{2+}$.<br>If true enter 1, else enter 0.<br>
Question 15 :
To an acidic solution of an anion, a few drops of $KMn{ O }_{ 4 }$ solution are added. Which of the following, if present, will not decolourise the $KMn{ O }_{ 4 }$ solution?
Question 16 :
Which of the following reactions does not involve either oxidation or reduction?
Question 17 :
Identify the correct statement regarding the following chemical reaction.<br/>$2HI\left( aq \right) +C{l }_{ 2 }\left( aq \right) \longrightarrow { I }_{ 2 }\left( s \right) +2HCl\left( aq \right)$
Question 19 :
The reaction is balanced if<span> :</span> <div>$5H_2O_2 + XClO_2 + 2OH^- \rightarrow XCl^- + YO_2 + 6H_2O$</div>
Question 20 :
How many moles of electrons are involved in the reduction of one mole of $ {MnO}^{-}_4$ ion in an alkaline medium to $ {MnO}^{-}_3$?
Question 21 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">Number of moles of $K_{2}Cr_{2}O_{7}$</span></span><i> </i><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">reduced by one </span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">mole of $Sn^{2+}$</span></span><span class="wysiwyg-font-size-xx-small"><span class="wysiwyg-font-size-xx-small"> </span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">ions is :</span></span>
Question 22 :
Which gas is evolved when $Pb{O}_{2}$ is treated with conc $HN{O}_{3}$?
Question 23 :
$2H_2O_2 \rightarrow 2H_2O + O_2$ is an example of disproportionation reaction.<br>If true enter 1, else enter 0.<br>
Question 25 :
The cell potential of dry cell when it is discharged will be zero.
Question 26 :
Equivalent weight of $H_3PO_2$ when it disproportionates into $PH_3$ and $H3PO_3$ (mol. wt. = $M$) is :
Question 27 :
Assertion: ${ O }_{ 3 }$ can act as an oxidising agent as well as a reducing agent but $S{ O }_{ 2 }$ can act only as an oxidant.
Reason: The oxidation number of $O$ in ${ O }_{ 3 }$ is zero and the oxidation number of $S$ in $S{ O }_{ 2 }$ is +4.
Question 30 :
In the chemical reaction, $K_{2}Cr_{2}O_{7}+XH_{2}SO_{4}+YSO_{2}\rightarrow K_{2}SO_{4}+Cr(SO_{4})_{3}+zH_{2}O$, $X,\: Y$ and $Z$ are respectively,<br>
Question 31 :
Which of the following reactant is oxidised in the following (unbalanced) reaction?<br>${ C }_{ 6 }{ H }_{ 5 }OH+{ O }_{ 3 }\longrightarrow { CO }_{ 2 }+{ H }_{ 2 }O+{ O }_{ 2 }$
Question 33 :
Reduction of the metal centre in aqueous permanganate ion involves :<br>
Question 35 :
Number of moles of $K_2Cr_2O_7$ reduced by $1$ mol of $Sn^{2+}$ is:
Question 36 :
Which of the following is not a disproportionation reaction?<br/>I. $N{ H }_{ 4 }N{ O }_{ 3 }\xrightarrow { \quad \Delta \quad } { N }_{ 2 }O+{ H }_{ 2 }O$<br/>II. ${ P }_{ 4 }\xrightarrow { \quad \Delta \quad } P{ H }_{ 3 }+HP{ O }_{ 2 }^{ \ominus }$<br/>III. $P{ Cl }_{ 5 }\xrightarrow { \quad \Delta \quad } P{ Cl }_{ 3 }+{ Cl }_{ 2 }$<br/>IV. $I{ O }_{ 3 }^{ \ominus }+{ I }^{ \ominus }\longrightarrow { I }_{ 2 }$
Question 37 :
The following equations are balanced atomwise and chargewise.<br/>(i) $Cr_2O_7^2+8H^++3H_2O_2\rightarrow2Cr^{3+}+7H_2O+3O_2$<br/>(ii) $Cr_2O_7^2+8H^++5H_2O_2\rightarrow2Cr^{3+}+9H_2O+4O_2$<br/>(iii) $Cr_2O_7^2+8H^++7H_2O_2\rightarrow2Cr^{3+}+11H_2O+5O_2$<br/>The precise equation/equations representing the oxidation of $H_2O_2$ is/are :
Question 38 :
Assertion: ${ H }_{ 2 }{ O }_{ 2 }$ acts only as an oxidising agent. <br>${ H }_{ 2 }{ O }_{ 2 }\longrightarrow { H }_{ 2 }O+O$
Reason: All peroxides behaves as oxidising agents only.
Question 39 :
Consider the following reaction:<br/>$M^{x+}+MnO^{\circleddash}_4\rightarrow MO^{\circleddash}_3+Mn^{2+}$<br/>If $1$ mol of $MnO^{\circleddash}_4$ oxidises $1.67$ mol of $M^{x+}$ to $MO^{\circleddash}_3$, then the value of $x$ in the reaction is :
Question 40 :
The oxidation state of oxygen of $H_2O_2$ in the final products when it reacts with $As_2O_3$ is :
Question 41 :
Which of the following in each pair acts as oxidant or reductant or both?
Question 42 :
How many electrons are involved in the following redox reaction?<br>$Cr_2O_{7}^{2-}+Fe^{2+}+C_2O_{4}^{2-}\rightarrow Cr^{3+}+Fe^{3+}+CO_2$ (Unbalanced)
Question 43 :
Calculate the volume of $Cl_{2}(g)$ (in mL) liberated at $1$ atm, $273$ K when $1.74$ gm $MnO_{2}$ reacts with $2.19$ gm $HCl$ according to the following reaction with $40\%$ yield.<br>$MnO_{2}+HCl\rightarrow MnCl_{2}+Cl_{2}+H_{2}O$<br>(Atomic mass of $Mn=55,\:Cl=35.5$)
Question 44 :
$As_2S_3 + NO^{\circleddash}_3 + H_2O \rightarrow AsO^{3-}_4 + SO^{2-}_4 + NO +H^{\bigoplus}$<br/>The number of electrons involved in the oxidation reaction is:
Question 45 :
<div><span>Write half-reactions using electrons.</span><br/></div><div><span><br/></span></div>$2Mn{ O }_{ 4 }^{ - }+5{ C }_{ 2 }{ O }_{ 4 }^{ 2- }+16{ H }^{ + }\longrightarrow 10{ CO }_{ 2 }+2{ Mn }^{ 2+ }+8{ H }_{ 2 }O$