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17. ⁠Chemical kinetics question bank (Chemistry)

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Q1.

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

(A)
\(1 \times 10^{-4} \, \text{mol L}^{-1}\text{s}^{-1}\)
(B)
\(3 \times 10^{-4} \, \text{mol L}^{-1}\text{s}^{-1}\)
(C)
\(4 \times 10^{-4} \, \text{mol L}^{-1}\text{s}^{-1}\)
(D)
\(6 \times 10^{-4} \, \text{mol L}^{-1}\text{s}^{-1}\)
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Q2.

In the reaction  
\(\text{BrO}_3^-(aq) + 5\text{Br}^-(aq) + 6\text{H}^+ \rightarrow 3\text{Br}_2(\ell) + 3\text{H}_2\text{O}(\ell)\)  
The rate of appearance of bromine (\(\text{Br}_2\)) is related to the rate of disappearance of bromide ions as follows:  

(A)
\(\frac{d[\text{Br}_2]}{dt} = \frac{3}{5} \frac{d[\text{Br}^-]}{dt}\)
(B)
\(\frac{d[\text{Br}_2]}{dt} = -\frac{3}{5} \frac{d[\text{Br}^-]}{dt}\)
(C)
\(\frac{d[\text{Br}_2]}{dt} = -\frac{5}{3} \frac{d[\text{Br}^-]}{dt}\)
(D)
\(\frac{d[\text{Br}_2]}{dt} = \frac{5}{3} \frac{d[\text{Br}^-]}{dt}\)
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