Given info:
A] (mol/L) [B] (mol/L) Rate of appearance of C (mol/L-hr)
1.0 ×10^-2 1.0 0.30×10^−6
1.0 ×10^−2 3.0 8.10×10^−6
2.0 ×10^−2 3.0 3.24×10^−5
2.0 ×10^−2 1.0 1.20×10^−6
3.0 ×10^−2 3.0 7.30×10^−5
Reaction: 3A+2B--->2C+D
Calculate the specific rate constant?
To calculate the specific rate constant (k) for the reaction 3A + 2B -> 2C + D, we can use the rate equation:
Rate = k[A]^m [B]^n
where [A] and [B] are the concentrations of reactants A and B, and m and n are the stoichiometric coefficients of A and B in the balanced chemical equation. In this case, m = 3 and n = 2.
Let's take the first set of data:
[A] = 1.0 × 10^-2 mol/L
[B] = 1.0 mol/L
Rate of appearance of C = 0.30 × 10^−6 mol/(L·hr)
Plugging these values into the rate equation, we get:
0.30 × 10^−6 mol/(L·hr) = k(1.0 × 10^-2 mol/L)^3 (1.0 mol/L)^2
Simplifying, we have:
0.30 × 10^−6 = k(1.0 × 10^-2)^3 (1.0)^2
0.30 × 10^−6 = k(1.0 × 10^-2)^3
Solving for k, we have:
k = (0.30 × 10^−6) / (1.0 × 10^-2)^3
Substituting the values, we get:
k = (0.30 × 10^−6) / (1.0 × 10^-2)^3
k = (0.30 × 10^−6) / (1.0 × 10^-6)
k ≈ 0.30
Similarly, you can repeat this calculation for the other sets of data and take the average to obtain a more accurate value for the specific rate constant.