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The reaction
C(s)+2H2(g)⇌CH4(g)
has p=0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.553 g of H2 and 22.14 g of C(s) are placed in an 8.89 L flask and heated to 1000. K.


Ptotal=______ atm

Respuesta :

pstnonsonjoku

From he calculations, we can see that the total pressure at equilibrium is 21 atm.

What is  equilibrium constant?

The term equilibrium constant commonly describes the constant that that shows the extent of conversion of reactants to products.

We have to find the pressure of each gas as follows;

For H2

P = nRT/V = 4.553 /2  × 0.082 × 1000/8.89 L = 21 atm

Using the ICE table;

         C(s)   +   2H2(g)  ⇌  CH4(g)

I                       21 atm          0

C                      -x                  +x

E                     21 - x              x

0.263= x/(21 - x )^2

0.263(21 - x )^2 = x

38 - 11x - 0.263x^2 = x

0.263x^2 + 12x - 38 = 0

x=2.97 atm

At equilibrium, we have;

(21 - 2.97) + 2.97 = 21 atm

Learn more about equilibrium constant: https://brainly.com/question/17960050

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