Question

if the rate constant for this reaction at 1000 k is 6.0 x 10⁴ m⁻² s⁻¹, what is the re- action rate when 3NO₄ = 0.035 m and 3H₂₄ = 0.015 m?

Answer 1

The reaction rate can be calculated by multiplying the rate constant with the concentrations of the reactants. In this case, it will be 3.15 x 10⁻⁵ m/s.

Step-by-step explanation:

The reaction rate can be determined using the rate constant and the concentrations of the reactants. In this case, the reaction involves the compounds 3NO₄ and 3H₂₄. To calculate the reaction rate, we can use the formula:

Reaction rate = k × [3NO₄] × [3H₂₄]

Substituting the values, where k = 6.0 x 10⁴ m⁻² s⁻¹, [3NO₄] = 0.035 m, and [3H₂₄] = 0.015 m, we get:

Reaction rate = (6.0 x 10⁴) × (0.035) × (0.015) = 3.15 x 10⁻⁵ m/s

The question asks to calculate the reaction rate given the rate constant k and the concentrations of the reactants for the decomposition of N2O5 into NO and O2 at a temperature of 1000 K.

To find the rate of the reaction, we need to use the rate law, which for this reaction is expected to be in the form of rate = k[NO4]^3[H2]^3 based on the stoichiometry provided in the question. Given that k = 6.0 x 10⁴ m⁻² s⁻¹, [NO4] = 0.035 m, and [H2] = 0.015 m, the rate would be calculated by plugging these values into the rate law equation.