For the reaction 2A(g) + B(aq) + 3C(l)<------> D(s) + 3E(g), the concentrations at equilibrium are found to be:
A: 2.3x10^3 Pa
B: 1.8x10^-2 M
C: 15.8M
D: 12.5M
E: 5.6x10^4 Torr
i got an answer of 1.83x10^-13 is this correct??
Did you get my answer to your problem yesterday?
I don't think you have this one right. Remember D(solids) and C(liquids) don't count.They aren't included in keq.
I obtained 4.3E10
To determine if your answer of 1.83x10^-13 is correct, we need to calculate the equilibrium constant (K) for the given reaction.
The equilibrium constant (K) can be calculated using the concentrations of the products and reactants at equilibrium. For a reaction in the gas phase, such as the one provided, the equilibrium constant can be determined using the partial pressures.
The equation for the equilibrium constant (Kp) in terms of partial pressures is:
Kp = (PD * PE^3) / (PA^2 * PB)
Where PD, PE, PA, and PB represent the partial pressures of D, E, A, and B, respectively.
Now, let's substitute the given values into the formula and calculate the equilibrium constant (Kp).
PD = partial pressure of D = 12.5 M (since we're given the concentration, we can assume it's the same as the partial pressure in this case)
PE = partial pressure of E = 5.6x10^4 Torr (convert Torr to Pa by multiplying by 133.32, so PE = 5.6x10^4 Torr * 133.32 Pa/Torr)
PA = partial pressure of A = 2.3x10^3 Pa
PB = concentration of B = 1.8x10^-2 M
Substituting these values into the equation:
Kp = (12.5 M * (5.6x10^4 Torr * 133.32 Pa/Torr)^3) / ((2.3x10^3 Pa)^2 * 1.8x10^-2 M)
To avoid confusion with units, convert all units to the same system. In this case, convert Torr to Pascal, which is the SI unit for pressure.
Now, calculate the value of Kp using a calculator.
After performing the calculation, we find that the equilibrium constant (Kp) is approximately 2.2x10^21.
Therefore, your answer of 1.83x10^-13 does not match the calculated equilibrium constant (Kp). Please recheck your calculations to find the correct value.