Question

If the rate constant for this reaction at 1000 K is 6.0×10⁴ m⁻² s⁻¹, what is the reaction rate when [NO] = 0.022 M and [H₂] = 0.020 M?

Answer 1

The reaction rate at 1000 K for a given rate constant of 6.0×10⁴ m⁻² s⁻¹ when [NO] = 0.022 M and [H₂] = 0.020 M is 0.58248 m⁻² s⁻¹, considering the reaction is second order with respect to NO.

Step-by-step explanation:

To calculate the reaction rate of the given chemical reaction at 1000 K with the rate constant 6.0×10⁴ m⁻² s⁻¹, when the concentration of NO is 0.022 M and the concentration of H₂ is 0.020 M, we must first understand the order of the reaction with respect to each reactant.

From the given information, since the initial rate of the reaction quadruples when the concentration of NO is doubled while keeping the concentration of H₂ constant, we infer that the reaction is second order with respect to NO. This means that the rate equation for the reaction is rate = k[NO]²[H₂].

Substituting the given values into the rate equation:

• rate = (6.0×10⁴ m⁻² s⁻¹) × (0.022 M)² × (0.020 M)

Now we calculate the rate:

• rate = 6.0×10⁴ × 0.000484 × 0.020 = 0.58248 m⁻² s⁻¹

The reaction rate at 1000 K when [NO] = 0.022 M and [H₂] = 0.020 M is 0.58248 m⁻² s⁻¹.