Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a flask with of ammonia gas and of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be . Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to significant digits.

The pressure equilibrium constant for the combustion of ammonia is 0.132

Explanation:

the balanced chemical reaction of the combustion of ammonia is as follows:

                                4NH3 + 3O2     =    2N2 +   6H2O

initially we have        4.8        1.9               0         0

in equilibrium            3.54      0.955        0.63    1.89

therefore the value of the equilibrium constant in terms of pressures is equal to:

Keq = ((PN2)^2 * (PH2O)^6)/((PNH3)^4 * (PO2)^3) = ((0.63^2)*(1.89^6))/((3.54^4) * (0.955^3)) = 0.132

c, liquids evaporate, creating a gas

can you list the answers so i can answer