Find the starting pressure of CCl4 at this temperature that produces a total pressure of 1.1 atm at equilibrium. Express the pressure in atmospheres to three significant figures.

The complete question is as follows: At 700 K, decomposes to carbon and chlorine. The Kp for the decomposition is 0.76.

Find the starting pressure of at this temperature that will produce a total pressure of 1.1 atm at equilibrium.

The starting pressure of is 0.79 atm.

Explanation:

The equation for decomposition of is as follows.

Let us assume that initial concentration of is 'a'. Hence, the initial and equilibrium concentrations will be as follows.

Initial:            a                0          0

Equilibrium:  (a - x)          0          2x

Total pressure = (a - x) + 2x = a + x

As it is given that the total pressure is 1.1 atm.

So, a + x = 1.1

a = 1.1 - x

Now, expression for equilibrium constant for this equation is as follows.

Hence, the value of 'a' is calculated as follows.

a + x = 1.1 atm

a = 1.1 atm - x

  = 1.1 atm - 0.31 atm

  = 0.79 atm

Thus, we can conclude that starting pressure of is 0.79 atm.

work: w = fd (given)

work done by chet   =50*1 = 50 j

work done by mika =40*2 = 80 j

work done by sara =30*1.5 = 45 j

work done by bill =60*0.5 = 30 j

students in order from the greatest amount of work done to the least is mika> chet> sara> bill

hence option (b) is correct.

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