The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of carbon monoxide? C(s) + H2O(g)

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Elin HesselLv2

25 May 2019

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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 500.mL flask at 18.Â°C with 4.9atm of carbon monoxide gas and 0.83atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 4.62atm of carbon monoxide gas, 0.55atm of water vapor and 0.28atm of carbon dioxide. The engineer then adds another 2.5atm 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.

The reaction of coal with water at high temperatures produces synthesis gas, which is a mixture of carbon monoxide and hydrogen. Use the bond energies in the table below to estimate the enthalpy of the reaction C(g) + H2O(g) ? CO(g) + H2(g) Energy(kj/mol) c-o = 358 c=o = 770 c-triple bond-o = 1070 o-h = 465 h-h = 435

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The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of carbon monoxide? C(s) + H2O(g)

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