Nitrogen dioxide reacts with carbon monoxide according to the elementary reaction…

CHEMISTRY · Multi-part · A Level · Chemistry · Rate equations · Rate equations

Problem

Nitrogen dioxide reacts with carbon monoxide according to the elementary reaction NO2(g)+CO(g)→NO(g)+CO2(g)NO_2(g) + CO(g) \rightarrow NO(g) + CO_2(g) For the temperature under study the rate law is rate=k[NO2]2[CO]\text{rate} = k[NO_2]^2[CO]. The initial concentrations are [NO2]0=0.10 M[NO_2]_0 = 0.10\,\text{M} and [CO]0=0.050 M[CO]_0 = 0.050\,\text{M}, and the measured initial rate is 3.0×10−4 M s−13.0 \times 10^{-4}\,\text{M s}^{-1}. Answer the following questions about how the reaction rate changes when the reactant concentrations are varied. Show all reasoning and clearly state any proportionality relationships you use. (a) Calculate the reaction rate when [NO2][NO_2] is doubled while [CO][CO] remains at its initial value. (b) Calculate the reaction rate when [NO2][NO_2] is halved and [CO][CO] is tripled simultaneously. (c) Without performing additional numerical calculations, predict by what factor the rate will change if [NO2][NO_2] is increased by a factor of 5 and [CO][CO] is decreased by a factor of 2. Explain your reasoning in complete sentences.

Related theory

Browse the problem library