164222 For the reaction,
\( \mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \)
\( \text { if } \frac{\mathrm{d}\left(\mathrm{NH}_3\right)}{\mathrm{dt}}=2.0 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
the value of \(-\frac{\mathrm{d}\left(\mathrm{H}_2\right)}{\mathrm{dt}}\) would be :

164237 \(3 A \rightarrow 2 B\), rate of reaction \(\frac{d[B]}{d t}\) is equal to :

164223 The \(t_{1 / 2}\) for a zero order reaction at the initial concentration of \(6 \times 10^{-3} \mathrm{M}\) is one minute at \(27^{\circ} \mathrm{C}\). The rate constant at \(27^{\circ} \mathrm{C}\) in \(\mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}\) is :

164224 In respect of the equation \(\mathrm{K}=\mathrm{Ae}^{-\mathrm{Ea} / \mathrm{RT}^2}\) in chemical kinetics, which one of the following statements is correct :

164222 For the reaction,
\( \mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \)
\( \text { if } \frac{\mathrm{d}\left(\mathrm{NH}_3\right)}{\mathrm{dt}}=2.0 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
the value of \(-\frac{\mathrm{d}\left(\mathrm{H}_2\right)}{\mathrm{dt}}\) would be :

164237 \(3 A \rightarrow 2 B\), rate of reaction \(\frac{d[B]}{d t}\) is equal to :

164223 The \(t_{1 / 2}\) for a zero order reaction at the initial concentration of \(6 \times 10^{-3} \mathrm{M}\) is one minute at \(27^{\circ} \mathrm{C}\). The rate constant at \(27^{\circ} \mathrm{C}\) in \(\mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}\) is :

164224 In respect of the equation \(\mathrm{K}=\mathrm{Ae}^{-\mathrm{Ea} / \mathrm{RT}^2}\) in chemical kinetics, which one of the following statements is correct :

164222 For the reaction,
\( \mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \)
\( \text { if } \frac{\mathrm{d}\left(\mathrm{NH}_3\right)}{\mathrm{dt}}=2.0 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
the value of \(-\frac{\mathrm{d}\left(\mathrm{H}_2\right)}{\mathrm{dt}}\) would be :

164237 \(3 A \rightarrow 2 B\), rate of reaction \(\frac{d[B]}{d t}\) is equal to :

164223 The \(t_{1 / 2}\) for a zero order reaction at the initial concentration of \(6 \times 10^{-3} \mathrm{M}\) is one minute at \(27^{\circ} \mathrm{C}\). The rate constant at \(27^{\circ} \mathrm{C}\) in \(\mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}\) is :

164224 In respect of the equation \(\mathrm{K}=\mathrm{Ae}^{-\mathrm{Ea} / \mathrm{RT}^2}\) in chemical kinetics, which one of the following statements is correct :

164222 For the reaction,
\( \mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \)
\( \text { if } \frac{\mathrm{d}\left(\mathrm{NH}_3\right)}{\mathrm{dt}}=2.0 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
the value of \(-\frac{\mathrm{d}\left(\mathrm{H}_2\right)}{\mathrm{dt}}\) would be :

164237 \(3 A \rightarrow 2 B\), rate of reaction \(\frac{d[B]}{d t}\) is equal to :

164223 The \(t_{1 / 2}\) for a zero order reaction at the initial concentration of \(6 \times 10^{-3} \mathrm{M}\) is one minute at \(27^{\circ} \mathrm{C}\). The rate constant at \(27^{\circ} \mathrm{C}\) in \(\mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}\) is :

164224 In respect of the equation \(\mathrm{K}=\mathrm{Ae}^{-\mathrm{Ea} / \mathrm{RT}^2}\) in chemical kinetics, which one of the following statements is correct :