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Question

A gaseous reaction, $$A_2(g)\rightarrow B(g)+\frac {1}{2}C(g)$$, shows increase in pressure of C from 100 mm to 120 mm in 5 minutes. The rate of disappearance of $$A_2$$ is:


A
4 mm min1
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B
8 mm min1
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C
16 mm min1
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D
2 mm min1
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Solution

The correct option is C 8 mm min$$^{-1}$$
$$A_2\rightarrow B+\dfrac {1}{2}C$$

$$\dfrac {-d[A_2]}{dt}=\dfrac {2d[C]}{dt}$$

Thus $$\dfrac {d[C]}{dt}=\dfrac {120-100}{5}=4 mm\ min^{-1}$$

$$\therefore \dfrac {-d[A_2]}{dt}=2\times 4=8 mm\ min^{-1}$$

Hence, option B is correct.

Chemistry
NCERT
Standard XII

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