Question

The reaction below has a Kp value of 3.3 × 10-5. What is the value of Kc for this reaction at 700 K? Note: Type the correct answer with 1 decimal place and in scientific notation. Example: 6.5 x 10-15 should be input as 6.5E-15. Example 2: 5.4 x 10-6 should be input at 5.4E-06.

Answer 1

This is an incomplete question, here is a complete question.

The reaction below has a Kp value of 3.3 × 10⁻⁵. What is the value of Kc for this reaction at 700 K?

$2SO_3(g)\rightleftharpoons 2SO_2(g)+O_2(g)$

Answer : The value of $K_p$ is, $5.79E^{-7}$

Explanation :

The relation between $K_c$ and $K_p$ is:

$K_p=K_c\times (RT)^{\Delta n}$

where,

$K_p$ = equilibrium constant at constant pressure  = $3.3\times 10^{-5}$

R = gas constant = 0.0821 L.atm/mol.K

T = temperature = 700 K

$\Delta n$ = change in number of gaseous moles = Product moles - Reactant moles = (2+1) - (2) = 3 - 1 = 1 mol

$K_c$ = equilibrium constant

Now put all the given values in the above expression, we get:

$K_p=K_c\times (RT)^{\Delta n}$

$3.3\times 10^{-5}=K_c(0.0821\times 700)^{1}$

$K_c=5.7\times 10^{-7}=5.7E^{-7}$

Therefore, the value of $K_p$ is, $5.7E^{-7}$

Answer 2

The value of the equilibrium constant of the reaction (Kc) is $5.74 \times 10^{-7}$

The given parameters;

• equilibrium constant at constant pressure, $K_p$ = 3.3 x 10⁻⁵.
• gas constant, R = 0.0821 L.atm/mol.K
• temperature, T = 700 K

The change in the number of gaseous moles is calculated as follows;

$\Delta n = product \ - reactant\\\\\Delta n = (2+1) - 2 = 1 \ mole$

The value of the equilibrium constant (Kc) is calculated as follows;

$K_p = K_c \times (RT)^{\Delta n}\\\\3.3 \times 10^{-5} = K_c \times (0.0821 \times 700)^1\\\\3.3 \times 10^{-5} = 57.47K_c\\\\K_c = \frac{3.3 \times 10^{-5} }{57.47} \\\\K_c = 5.74 \times 10^{-7}$

Thus, the value of the equilibrium constant of the reaction (Kc) is $5.74 \times 10^{-7}$

"Your question is not complete, it seems to be missing the following information;"

The reaction below has a Kp value of 3.3 × 10⁻⁵. What is the value of Kc for this reaction at 700 K?

$2SO_3(g) \ ---> \ 2SO_2(g) \ + \ O_2$

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