1 mole of an ideal gas is allowed to expand isothermally and reversibly from $\mathrm{1L}$ to 5 L at 300 K . The change in enthalpy (in kJ ) is $\left(R=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
Consider the following equilibrium reaction in gaseous state at $T(\mathrm{~K})$.
$$ A+2 B \rightleftharpoons 2 C+D $$
The initial concentration of $B$ is 1.5 times that of $A$. At equilibrium, the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is
At $T(\mathrm{~K}) K_{\mathrm{sp}}$ of two ionic salts $M X_2$ and $M X$ is $5 \times 10^{-13}$ and $1.6 \times 10^{-11}$ respectively. The ratio of molar solubility of $M X_2$ and $M X$ is
Consider the following.
Statement $\mathrm{IH}_2 \mathrm{O}_2$ acts as an oxidising as well as reducing agent in both acidic and basic mediim.
Statement $\mathrm{II} 10 \mathrm{~V} \mathrm{H}_2 \mathrm{O}_2$ sample means it contains $6 \% \left(\frac{w}{v}\right) \mathrm{H}_2 \mathrm{O}_2$.
The correct answer is
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