For a reaction : \(N_2 + 3H_2 \rightarrow 2NH_3\), the rate of reaction with respect to \(NH_3\) is
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- \(+\dfrac{1}{3}\dfrac{\Delta[NH_3]}{\Delta t}\)
- \(-\dfrac{1}{2}\dfrac{\Delta[NH_3]}{\Delta t}\)
- \(+\dfrac{1}{4}\dfrac{\Delta[NH_3]}{\Delta t}\)
- \(+\dfrac{1}{2}\dfrac{\Delta[NH_3]}{\Delta t}\)
The Correct Option is D
Solution and Explanation
For a reaction, the rate is expressed by dividing the change in concentration of each species by its stoichiometric coefficient. For a product, the sign is positive (it is being formed).
Step 1:
In \(N_2 + 3H_2 \rightarrow 2NH_3\), the coefficient of \(NH_3\) is 2, and \(NH_3\) is a product, so its term is positive.
Step 2:
Rate with respect to \(NH_3\) = \(+\dfrac{1}{2}\dfrac{\Delta[NH_3]}{\Delta t}\).
Answer: Option (D) \(+\dfrac{1}{2}\dfrac{\Delta[NH_3]}{\Delta t}\).
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