This reaction is first order in N₂O₅: N₂O₅(g) → NO₃(g) + NO₂(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N₂O₅] = 0.055 M

Video transcript

Hello. In this problem, we are told the given reaction is second order with respect to the concentration of X. And at two R 98 Kelvin, the rate constant for the reaction is 0.683 per minority per second. Were asked to calculate the initial rate. When given the concentration of X is 1.135 Mueller will begin by writing our reaction rate law. So the rate is equal to our reaction rate constant times the concentration of X squared. Since its second order with regard to concentration of X, We have to find the initial rate. So we have our reaction rate constant which is 0.683 per minority per second times the concentration of X which is 1.135 Mueller. We're gonna square that. This works out to 0.880 hilarity squared. For morality second will simplify our units. One of the clarity units cancels were left within 0.880 similarity per second as our initial rate. Thanks for watching. Hope this help.