Equilibrium concentrations
(a)(mol/L)// (b)(mol/L)// (c)(mol/L)
0.040 // 0.066 // 1.72x10^-2
0.080 // 0.017 // 8.8x10^-3
0.030 // 0.024 // 4.7x10^-3
My data was collected at 25○C for the reaction A(g) + B(g) = C(g)
What i have to do now is involving three different initial sets of concentrations, use the data to show that K does not vary with initial concentrations at the same time.
I am very stuck on this question i just wish i could understand it more.
A + B ==> C
K = (C)/(A)(B)
Substitute for C and A and B and solve for K in each instance.
I have 6.515 for trial 1, 6.47 for trial 2, and 6.52 for trial 3 which is very close to the same value for K at each of the three trials. You need to do it yourself with more accuracy and don't forget to round to the correct number of significant figures.
okay i have the vaule of K being 6.527.
I'm just confused as to how to start the teials. do i just do (b)/(a)(c), (a)/(b)(c) and (c)/(a)(b) ?
i got all the answers now Doctor Bob. thank you so much for your help! its muchly appreciated!
To show that the equilibrium constant, K, does not vary with initial concentrations, you need to calculate the value of K for each set of initial concentrations and compare the results. Here's how you can approach this problem:
1. Write the balanced chemical equation for the reaction:
A(g) + B(g) ⇌ C(g)
2. Use the given data to construct an ICE (Initial, Change, Equilibrium) table for each set of initial concentrations.
For the first set of initial concentrations:
Initial: A = 0.040 mol/L, B = 0.066 mol/L, C = 1.72x10^(-2) mol/L
Let x be the change in concentration at equilibrium.
Change: A = -x, B = -x, C = +x
Equilibrium: A = (0.040 - x) mol/L, B = (0.066 - x) mol/L, C = (1.72x10^(-2) + x) mol/L
3. Use the equilibrium concentrations from the ICE table to calculate the equilibrium constant, K, for each set of initial concentrations.
K = [C] / ([A] * [B])
For the first set of initial concentrations:
K1 = (1.72x10^(-2) + x) / ((0.040 - x) * (0.066 - x))
Similarly, calculate K2 and K3 for the other two sets of initial concentrations.
4. Simplify the expressions for K1, K2, and K3 by assuming that x is small compared to the initial concentrations.
5. Compare the values of K1, K2, and K3. If K remains constant regardless of the initial concentrations, then the values of K should be approximately equal.
Calculate the numerical values of K1, K2, and K3 using the given initial concentrations and compare them. If the values are close to each other, it will show that K does not vary significantly with the initial concentrations.
By performing these calculations, you can demonstrate whether K varies or remains constant with different initial concentrations.