Steam reforming of methane ( ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a flask with of methane gas and of water vapor at . She then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be . Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to significant digits.

Explanation:

The missing data on the question are:

1. Equilibrium equation:

2. ICE (initial, change, equilibrium) table:

Partial pressures in atm

I           4.7            2.5           0            0

C          -x             -x          +x          +3x

E        4.7 - x     2.5  - x       x           3x

3. Partial pressures:

The partial pressure of hdyrogen gas at equilibrium is 2.3 atm

Then:

4. Pressure equilibrium constant equation:

Round to two significant figures: 1.4 atm²

answer: i have one answer

acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (h+) ions

explanation:

hope this and sorry i could only come up with one answer!