nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in this reaction 2NO(g) +
ID: 883047 • Letter: N
Question
nitric oxide, NO(g) reacts with chlorine gas, Cl2(g), in this reaction 2NO(g) + Cl2(g) -> 2NOCl(g)Initial rates of reaction are determine for various combinations of initial concentration of reactants and recorded below ( picture below) A) what is the rate law equation for the reaction? B) what is the rate determining step? C) calculate a value for the rate law constant, including units D) calculate the expected rate of reaction if the initial concentration of NO and Cl2 gases were 0.30 and 0.40mol/L, respectively. *** Please show all the word I am really confused about these questions **** thank you SCH4U -Chemistry Lesson 12 3. Nitric oxide, NO(g) reacts with chiorine gas, Clazug, in tie re a), in the reaction Initial rates of reaction are determined for various combinations o concentrations of reactants and recorded below; binations of initial Trial Initial [NO] Rate of production nitial [Cll (mol/L) 0.10 0.20 0.20 mol/L) of NOCI (mol/Ls) 2 3 0.10 0.10 0.20 1.8 x 10 3.6 x 10 1.43 x 10 a) What is the rate law equation for the reaction? (1 mark) b) What is the rate-determining step? (1 mark) c) Calculate a value for the rate constant, including units. (3 marks) d) Calculate the expected rate of reaction if the initial concentrations of NO and Cla gases were 0.30 and U.40 mo/L, respectively. (3 marks)
Explanation / Answer
A) to determine the rate law of the reaction we will find the order of reaction with respect to each reactant
Trial 1 and Trial 2 the concentration of [NO] is same
However the concentration of Cl2 is doubled, and the rate of reaction also becomes double.
So order of reaction with respect ot Cl2 will be 1
Similarly in Trial 2 and Trial 3 the concentration of Cl2 is kept constant and that of [NO] is doubled, and the rate of reaction also becomes four times ( 14.3 / 3.6 = 3.97 ).
So order of reaction with respect ot NO will be 2
So rate law will be
Rate = K [Cl2][NO]2
B) Rate determining step is
NOCl2(g) + NO (g) -->2 NOCl (g)
C) Rate law is
Rate = K [Cl2][NO]2
1.8 X 10^-2 = K [NO]2[Cl2]
1.8 X 10^-2 / [0.1][0.1]2 = K
K = 18 mol-2 L 2 sec -1
D) Rate of reaction = K [NO]2[Cl2]
Rate of reaction = 18 X [0.3]2[0.4] = 0.648
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