2NO(g) + 2H2(g) → N2(g) + 2H2O(g) 6.0×10^4 M^-2 s^-1

다음 반응을 생각해 보자.

2NO(g) + 2H2(g) → N2(g) + 2H2O(g)

(a) 이 반응의 속도 법칙은 H2에 대하여 일차이고

NO에 대하여 이차이다. 속도 법칙을 쓰시오.

(b) 반응의 속도 상수가 1000 K에서

6.0×10^4 M^-2 s^-1이라고 하면,

[NO] = 0.035 M이고 [H2] = 0.015 M일 때의

반응 속도는 얼마인가?

H2의 농도가 0.010 M일 때의 반응 속도는 얼마인가?

(d) 1000 K에서 [NO]가 0.010 M로 감소하고

[H2]가 0.030 M로 증가할 때의 반응 속도는 얼마인가?

Consider the following reaction:

2NO(g) + 2H2(g) → N2(g) + 2H2O(g)

(a) The rate law for this reaction is first order in H2

and second order in NO. Write the rate law.

(b) If the rate constant for this reaction

at 1000 K is 6.0×10^4 M^-2 s^-1,

what is the reaction rate

when [NO] = 0.035 M and [H2] = 0.015 M?

when the concentration of NO is increased to 0.10 M,

while the concentration of H2 is 0.010 M?

(d) What is the reaction rate at 1000 K

if [NO] is decreased to 0.010 M

and [H2] is increased to 0.030 M?

(a) The rate law for this reaction is first order in H2 and second order in NO. Write the rate law.

rate = k [NO]^2 [H2]

(b) If the rate constant for this reaction at 1000 K is 6.0×10^4 M^-2 s^-1, what is the reaction rate when [NO] = 0.035 M and [H2] = 0.015 M?

rate = k [NO]^2 [H2]

= (6.0×10^4) (0.035)^2 (0.015)

= 1.1025 M/s

≒ 1.1 M/s

(c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H2 is 0.010 M?

rate = k [NO]^2 [H2]

= (6.0×10^4) (0.10)^2 (0.010)

= 6.0 M/s

(d) What is the reaction rate at 1000 K

if [NO] is decreased to 0.010 M

and [H2] is increased to 0.030 M?

rate = k [NO]^2 [H2]

= (6.0×10^4) (0.010)^2 (0.030)

= 0.18 M/s

[ 관련 글 https://ywpop.tistory.com/22591 ]

NO와 H2의 농도가 모두 2.0×10^(-6) mol L-1일 때,

반응 속도가 7.86×10^(-3) mol L-1 s-1이라면,

이 반응의 속도 상수 값과 단위는?

[키워드] 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) 기준, 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) rate law

2NO(g) + 2H2(g) → N2(g) + 2H2O(g) 6.0×10^4 M^-2 s^-1