For the reaction CH₄(g)+ 4 NO(g)$\to$ 2 N₂(g)+ CO₂(g)+ 2 H₂O(g),the rate of the reaction in terms of the change in nitrogen monoxide concentration would be written as __________

Question

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The rate of the reaction is proportional to the change in the concentration of nitrogen monoxide, so the correct rate expression would include [NO] in the numerator. Looking at the balanced chemical equation, for every 4 molecules of NO consumed, 10 molecules of nitrogen sulfide are produced. Therefore, the rate of the reaction is directly proportional to -d[NO]/dt, which is represented as [NO] with a negative sign in the rate expression. The coefficient in front of [NO] would come from the stoichiometry of the reaction, which is 4. Thus, the rate expression would be -1/4 d[NO]/dt = k[CH3CONH2][NO]^4. Converting this to a rate law by multiplying both sides by -4 gives  d[NO]/dt = -4k[CH3CONH2][NO]^4. Since the question is asking for the expression in terms of the change in NO concentration, the answer would be -4k[CH3CONH2][NO]^4.

For the Reaction CH4(g)+ 4 NO(g) →\to→ 2 N2(g)+ CO2(g)+ 2 H2O(g),the Rate of the Reaction in 2

For the Reaction CH₄(g)+ 4 NO(g) $\to$ 2 N₂(g)+ CO₂(g)+ 2 H₂O(g),the Rate of the Reaction in 2