Consider the equilibrium N₂O4(g) = 2NO₂(g). At 500 °C, a sealed vessel contained 39.1 M nitrogen dioxide gas and 64.1 M dinitrogen tetroxide gas. Calculate the value of Kc at this temperature. Provide your answer to one decimal. Do not enter units. Type your answer...

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"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 125 L tank with 20. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.0 mol of carbon monoxide gas, 11. mol of water vapor and 13. mol of carbon dioxide. The engineer then adds another 7.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. mol

Initially 10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas at equilibrium would be? 2NH3(g) + 94 kJ <=====> N2(g) + 3H2(g)