1
answer
0
watching
517
views
18 Nov 2019
Given the following data, determine the rate law for the reaction a. k [NO][Cl_2] b. k[NO][Cl_2]^2 c. k[NO]^2[Cl_2] d. k[NO]^2[Cl_2]^2 e. k[NO][Cl_2]^1/2 The reaction C_2H_5CI (g) rightarrow C_2H_4(g) + HCI(g) has a rate constant of approximately 4.20 times 10^-5 s^-1 at 700 K. What is the reaction rate if 123.8 g C_2H_5CI is placed in an 8.00 L container at 700 K? a. 1.75 times 10^-4 M/s b. 3.36 times 10^-4 M/s c. 6.50 times 10^-4 M/s d. 1.01 times 10^-5M/s e. 8.01 times 10^-5 M/s Suppose 2.00 g azomethane (58.1 g/mol) are placed in a 2.50 L container at 425 degree C and allowed to decompose according to the first order reaction. CH_3NNCH_3(g) rightarrow C_2H_6(g) + N_2(g). Initially, 0.0234 moles of C_2H_6 are produced per second. What is the rate constant?
Given the following data, determine the rate law for the reaction a. k [NO][Cl_2] b. k[NO][Cl_2]^2 c. k[NO]^2[Cl_2] d. k[NO]^2[Cl_2]^2 e. k[NO][Cl_2]^1/2 The reaction C_2H_5CI (g) rightarrow C_2H_4(g) + HCI(g) has a rate constant of approximately 4.20 times 10^-5 s^-1 at 700 K. What is the reaction rate if 123.8 g C_2H_5CI is placed in an 8.00 L container at 700 K? a. 1.75 times 10^-4 M/s b. 3.36 times 10^-4 M/s c. 6.50 times 10^-4 M/s d. 1.01 times 10^-5M/s e. 8.01 times 10^-5 M/s Suppose 2.00 g azomethane (58.1 g/mol) are placed in a 2.50 L container at 425 degree C and allowed to decompose according to the first order reaction. CH_3NNCH_3(g) rightarrow C_2H_6(g) + N_2(g). Initially, 0.0234 moles of C_2H_6 are produced per second. What is the rate constant?
Nestor RutherfordLv2
17 Jan 2019