Carbon monoxide and chlorine gas react to form phosgene (COCl_2) according to th
ID: 1013069 • Letter: C
Question
Carbon monoxide and chlorine gas react to form phosgene (COCl_2) according to the equation CO(g) + Cl_2(g) rightarrow COCl_2(g) The rate law tor the reaction is rate = k[Cl_2][CO]^1.5 Which mixture of chlorine gas and carbon monoxide gas has the fastest initial rate? Consider this two step mechanism for a reaction: NO_2(g) + Cl_2(g) rightarrow ClNO_2(g) + Cl(g) Slow NO_2(g) + Cl(g) rightarrow ClNO_2(g) Fast What is the overall reaction? What is the predicated rate law? 2NO_2(g) + Cl_2(g) rightarrow 2ClNO_2(g): rate = k [NO_2][Cl_2] 2NO_2(g) + Cl_2(g) rightarrow ClNO_2(g): rate = k [NO_2][Cl] NO_2(g) + Cl_2(g) rightarrow ClNO_2(g): rate = k [NO_2][Cl_2]Explanation / Answer
Answer : C
Because the CO and Cl2 are in the ratio 1.5 : 1 so the initial rate will be fast
NO2 (g) + Cl2(g) -------> ClNO2(g) + Cl(g) (Slow step)
NO2(g) + Cl(g) --------> ClNO2(g) (fast step)
2 NO2 (g) + Cl2(g) -------> 2 ClNO2(g)
Rate law = K [NO2]^1 [Cl2]^1
Rate of reaction involved slow step of the reaction. so the rate law is expressed as above.