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Which one of the following statements regarding post-fertilization development in flowering plants is incorrect?
The value of $E^{\circ}_{cell}$ for the following reaction is: $Cu^{2+} + Sn^{2+} \rightarrow Cu + Sn^{4+}$ (Given, equilibrium constant is $10^6$)
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?
In the silver plating of copper, $K[Ag(CN)_2]$ is used instead of $AgNO_3$. The reason is:
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 three cells with their $E^{\circ}_{cell}$ values are given below: 1. $Fe|Fe^{2+}||Fe^{3+}|Fe \ ; \ 0.404\text{ V}$ 2. $Fe|Fe^{2+}||Fe^{3+}, Fe^{2+}|Pt \ ; \ 1.211\text{ V}$ 3. $Fe|Fe^{3+}||Fe^{3+}, Fe^{2+}|Pt \ ; \ 0.807\text{ V}$ The standard Gibbs free energy change values for three cells are, respectively: (F represents the charge on $1\text{ mole}$ of electrons.)
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.
Match the redox conversions in List-I with the corresponding number of Faradays required in List-II. **List-I (Redox Conversion)** A. $1\text{ mol}$ of $\text{H}_2\text{O}$ to $\text{O}_2$ B. $1\text{ mol}$ of $\text{MnO}_4^-$ to $\text{Mn}^{2+}$ C. $1.5\text{ mol}$ of $\text{Ca}$ from molten $\text{CaCl}_2$ D. $1\text{ mol}$ of $\text{FeO}$ to $\text{Fe}_2\text{O}_3$ **List-II (Number of Faraday required)** I. $3\text{F}$ II. $2\text{F}$ III. $1\text{F}$ IV. $5\text{F}$
At $25^\circ\text{C}$, molar conductance of $0.1 \text{ molar}$ aqueous solution of ammonium hydroxide is $9.54 \text{ ohm}^{-1}\text{cm}^2\text{mol}^{-1}$ and at infinite dilution, its molar conductance is $238 \text{ ohm}^{-1}\text{cm}^2 \text{mol}^{-1}$. The degree of ionization of ammonium hydroxide at the same concentration and temperature is:
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
Based on electrode potentials in the table below: $\text{Cu}^{2+}(aq) + e^- \rightarrow \text{Cu}^+(aq) \quad E^\circ = 0.15 \text{ V}$ $\text{Cu}^+(aq) + e^- \rightarrow \text{Cu}(s) \quad E^\circ = 0.50 \text{ V}$ The value of $E^\circ_{\text{Cu}^{2+}/\text{Cu}}$ will be:
Sphincter of oddi is present at: