What is the initial rate when the initial concentrations of both reactants are 0.16M? The initial rates listed in the following table were determined for the reaction 2NO (g) + Cl2 (g) →2NOCl (g) Experiment Initial [NO] Initial [Cl2] Cl2 consumption rate (initial) 1 0.13 0.20 1.010^-2 2 0.26 0.20 4.010^-2 3 0.13 0.10 5.0x10^-3 rate=k[NO]^2[Cl_2] value of rate constant is k=3.0 / M^2 x s

Question

Zechariah Galloway

Chemistry

30 November, 07:11

What is the initial rate when the initial concentrations of both reactants are 0.16M? The initial rates listed in the following table were determined for the reaction 2NO (g) + Cl2 (g) →2NOCl (g) Experiment Initial [NO] Initial [Cl2] Cl2 consumption rate (initial) 1 0.13 0.20 1.010^-2 2 0.26 0.20 4.010^-2 3 0.13 0.10 5.0x10^-3 rate=k[NO]^2[Cl_2] value of rate constant is k=3.0 / M^2 x s

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Dashawn Herring · Answer 1

We are given with the initial concentrations of both reactants, nitrous oxide and chlorine of 0.16 M and the value of the rate constant equal to M. The initial rate constant is required in this problem. The rate is expressed in k NO^2 * Cl2. Substituting 0.16 to both components, the initial rate is 0.12288.