The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5¡4 NO2 + O2. The rate law is first order in N2O5. At 64 C the rate constant is 4.82 * 10-3 s-1. (a) Write the rate law for the reaction.

Video transcript

Hello everyone. Today we have the following problem. The decomposition reaction of di nitrogen PTO pent side and carbon tetrachloride is the following the rate loss. First order in our di nitrogen pint at 64 °C, the rate constant is 4.82 times 10 to the negative third seconds, rates to the power of negative one, write the rate law for the reaction. So the rate law is written in terms of the rate and it explores the relationship between the reaction rate and the concentrations of the reactants. And so they ignore the products. So if we look at this following reaction, it was stated that it was first order. So we will write the rate constant, which is K and then we will write our first reactant, we have our diane nitrogen pint to sign and we wanna make sure that we write it in brackets and then we write its order as an exponent. And since this was first order, we can leave it as is. So we can also include our rate constant for K if we substitute 4.82 times 10 to the negative third seconds raise with the power of negative one multiplied by our concentration of our di nitrogen pint oxide. We get the following or answer choice B as our final answer overall, I hope this helped. And until next time.