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A button cell used in watches functions as following: $\text{Zn}(s) + \text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) \rightleftharpoons 2\text{Ag}(s) + \text{Zn}^{2+}(aq) + 2\text{OH}^-(aq)$ If half cell potentials are: $\text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s); E^\circ = -0.76 \text{ V}$ $\text{Ag}_2\text{O}(s) + \text{H}_2\text{O}(l) + 2e^- \rightarrow 2\text{Ag}(s) + 2\text{OH}^-(aq); E^\circ = 0.34 \text{ V}$ The cell potential will be:
Which one of the following statements regarding post-fertilization development in flowering plants is incorrect?
Kohlrausch's law states that at
The standard Emf of a galvanic cell involving cell reaction with $n = 2$ is found to be $0.295\text{ V}$ at $25^{\circ}\text{C}$. The equilibrium constant of the reaction would be: (Given $F = 96500\text{ C mol}^{-1}$; $R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}$)
Given the reaction: $\text{Cu}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Cu}^{2+}(aq) + 2\text{Ag}(s)$ with $E^\circ = 0.46 \text{ V}$ at $298 \text{ K}$, what is the equilibrium constant for the reaction?
On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:
Which one of the following molecular hydrides acts as a Lewis acid?
The molar conductivity of $0.007\text{ M}$ acetic acid is $20\text{ S cm}^2\text{ mol}^{-1}$. The dissociation constant of acetic acid is: ($\Lambda^o_{H^+} = 350\text{ S cm}^2\text{ mol}^{-1}$ and $\Lambda^o_{CH_3COO^-} = 50\text{ S cm}^2\text{ mol}^{-1}$)
The molar conductivity of a $0.5 \text{ mol/dm}^3$ solution of $\text{AgNO}_3$ with electrolytic conductivity of $5.76 \times 10^{-3} \text{ S cm}^{-1}$ at $298 \text{ K}$ is:
Standard electrode potential for the cell with cell reaction $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$ is $1.1\text{ V}$. Calculate the standard Gibbs energy change for the cell reaction. (Given $F = 96487\text{ C mol}^{–1}$)
Given below are two statements: Assertion (A): In the equation, $\Delta_rG = -nFE_{cell}$, value of $\Delta_rG$ depends on $n$. Reason (R): $E_{cell}$ is an intensive property and $\Delta_rG$ is an extensive property.
Mass in grams of copper deposited by passing $9.6487\text{ A}$ current through a voltmeter containing copper sulphate for $100\text{ seconds}$ is (Given: Molar mass of Cu: $63\text{ g mol}^{-1}$, $1\text{ F} = 96487\text{ C mol}^{-1}$)
Vernalisation stimulates flowering in:
Among the following, the one that is not a green house gas is
Spraying sugarcane crop with which of the following plant growth regulators, increases the length of the stem, thus, increasing the yield?
Given that the ionic product of $\text{Ni(OH)}_2$ is $2 \times 10^{-15}$. The solubility of $\text{Ni(OH)}_2$ in $0.1\text{ M}$ NaOH is:
The concentration of the $Ag^+$ ions in a saturated solution of $Ag_2C_2O_4$ is $2.2 \times 10^{-4}\text{ M}$. The solubility product of $Ag_2C_2O_4$ is:
The percentage of pyridine ($C_5H_5N$) that forms pyridinium ion ($C_5H_5NH^+$) in a 0.10 M aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is:
The $K_{sp}$ of $Ag_2CrO_4$, $AgCl$, $AgBr$ and $AgI$ are, respectively, $1.1 \times 10^{-12}$, $1.8 \times 10^{-10}$, $5.0 \times 10^{-13}$, and $8.3 \times 10^{-17}$. The salt that precipitates last if $AgNO_3$ solution is added to the solution containing equal moles of $NaCl$, $NaBr$, $NaI$ and $Na_2CrO_4$ is:
The molecule that is least likely to behave as Lewis base is: