Final answer:
The rate of disappearance of NO during a reaction cannot be calculated without the proper rate law and reaction order. Given data alone, such as concentrations of NO and O2, are insufficient without this additional information.
Step-by-step explanation:
The rate of disappearance of NO (which is likely to mean nitric oxide in this context, not to be confused with N2O or dinitrogen monoxide) can't be determined precisely with the given data alone. To calculate the rate of disappearance of NO during a reaction, you would typically use the rate law for the reaction and the concentrations of the reactants involved. If the question refers to the decomposition of N2O5 into NO and O2, the rate of decomposition can be found using the given rate constant k for the reaction, which depends on temperature, and the concentration of N2O5.
However, to provide a specific answer, one would need to know the exact balanced chemical equation and the order of reaction for each reactant (i.e., whether it is first order or second order with respect to NO and O2). Without this additional information or a specific rate law, we cannot identify which of the given answers (a, b, c, or d) is the rate of disappearance of NO for the concentrations provided.