Write a balanced chemical equation for carbon dioxide reacting with hydrogen gas (H2) to produce methane and water. Then write the equation for the combustion of methane. If you start with 100 g of hydrogen that reacts in this entire process in an excess of carbon dioxide and oxygen how much water is theoretically produced?
I have a homework question:
“The industrial process for producing hydrogen gas involves reacting methane and steam at a high temperature. Predict the direction of equilibrium shift for each of the following stresses…”
My problem is I don’t know what the equation for this process is! Can? anyone tell me
When carbon monoxide reacts with hydrogen gas, methane and water vapor are formed according to the following reaction
CO(g) + 3H2(g) = CH4(g) + H2O(g)
Analysis at equilibrium shows that Keq = 0.555, the [CO] = 0.921 M, the [H2] = 1.21 M, and the [CH4] = 0.0391 M. Calculate the equilibrium concentration for the water vapor.
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