What is the overall order of the following reaction, given the rate law? 2 NO(g)

Question

What is the overall order of the following reaction, given the rate law? 2 NO(g) + H_2(g) rightarrow N_2(g) + 2 H_2O (g) Rate = k[NO]^2[H_2] A. zeroth order B. first order C. second order D. third order E. fourth order Given the following rate law, how does the rate of reaction concentration of X is doubled? Rate = k[X]^2[Y]^3 A. The rate of the reaction will not change. B. The rate of the reaction will increase by a factor of 2. C. The rate of the reaction will increase by a factor of 4. D. The rate of the reaction will increase by a factor of 8. E. The rate of the reaction will increase by a factor of 9. Write the equilibrium constant expression (K_c = ...) for the following reaction. 2 P(g) + 3Cl_2(g) 2PCl_3(g) A. [PCl_3]^2/[P]^2[Cl_2]^3 B. [PCl_3]^1/2/[P]^1/2[Cl_2]^1/3 C. [PCl_3]/[P][Cl_2] D. [P]^2[Cl_2]^3/[PCl_3]^2 E. [P][Cl_2]/[PCl_3] Determine the value of [N_2] for the following reaction if K_c = 2 and the equilibrium concentrations are as follows: [H_2] = 2.0 M and [NH_3] = 0.5 M. N_2(g) + 3 H_2(g) 2NH_3(g) A. 0.016 M B. 0.031 M C. 0.062 M D. 0.40 M E. 62.5 M

Explanation / Answer

9) D) third order

10)C) the rate of the reaction will increase by a factor 4

11)A) [ PCl3]^2/[P]^2[Cl2]^3

12) A) 0.016M

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