1.

a sample of s8 (8) is placed in an otherwise empty rigid container at 1325 k at an initial pressure of 1.00 atm, where it

decomposes to s2 by the reaction: s8() 4 s2(2). |

at equilibrium, the partial pressure of s, is 0.25 atm. calculate k, for this reaction at 1325 k

The value of is 324

Explanation:

We are given:

Initial pressure of = 1.00 atm

The chemical equation for the conversion of to follows:

Initial:          1

At eqllm:    1-x       4x

We are given:

Equilibrium partial pressure of

Evaluating the value of 'x', we get:

The expression of for the above reaction follows:

Putting values in above expression, we get:

Hence, the value of is 324

the answer is a and have a great day