"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact, this reaction is one of the ways hydrogen is made industrially.
A chemical engineer studying this reaction fills a 200.0 mL flask at 12.0 °C with 1.3 atm of carbon monoxide gas and 3.6 atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 0.82 atm of carbon monoxide gas, 3.12 atm of water vapor and 0.48 atm of carbon dioxide.
The engineer then adds another 0.43 atm of carbon monoxide and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits.