Question

At elevated temperature, carbon tetrachloride decomposes to its elements: CCl4(g) C(s) 2Cl2(g). At 700 K, if the initial pressure of CCl4 is 1. 00 atm and at equilibrium the total pressure is 1. 35 atm, then calculate K

Answer 1

`K=0.0131M`

Step-by-step explanation:

Hello,

In this case, the undergoing chemical reaction turns out:

`CCl_4(g) \rightleftharpoons C(s)+ 2Cl_2(g)`

In such a way, by means of the mass of law action for such reaction, which is given below:

`Kp=(p_(Cl_2)^2)/(p_(CCl_4))`

And in terms of the change
`x` due to reaction extent:

`p_(CCl_4)=p_(CCl_4)^0-x\\p_(Cl_2)=2x\\p_T=p_(CCl_4)+p_(Cl_2)=1.00-x+2x\\p_T=1.00+x`

`x` results:

`x=1.35 atm -1.00atm=0.35atm`

In such a way, Kp:

`Kp=((2x)^2)/(1.00-x) =((2*0.35atm)^2)/(1.00atm-0.35atm)=0.754atm`

Nonetheless, K is asked instead of Kp, thus:

`K=\frac{Kp}{(RT)^{\Delta \\u _(gas)}}`

Whereas:

`\Delta \\u _(gas)=2-1=1`

Which is the change in the moles of gaseous species chlorine and carbon tetrachloride. Hence, we finally obtain:

`K=(0.754atm)/((0.082(atm*L)/(mol*K)*700K)^(1))\\\\K=0.0131mol/L=0.0131M`

Best regards.