The water-gas reaction is a source of hydrogen. Passing steam over hot carbon produces a mixture of carbon monoxide and hydrogen. $$H2O(g)+C(s)CO(g)+H2(g) The value of Kc for the reaction at 1000.0°C is 3.00 × 10–2. kp=3.1354. Calculate the equilibrium partial pressure of H2O given that PH2O = 0.442 atm and PCO = 5.000 atm at the start of the reaction. Assume that the carbon is in excess. =.2747 the partial pressure of CO is 5.1676 the equilibrium partial pressure of H2 is .1676 Determine the equilibrium partial pressure of H2O after CO and H2 at 0.0800 atm are added to the equilibrium mixture described above. Determine the equilibrium partial pressure of CO after the addition described above Determine the equilibrium partial pressure of H2 after the addition described above.
The water-gas reaction is a source of hydrogen. Passing steam over hot carbon produces a mixture of carbon monoxide and hydrogen.
$$H2O(g)+C(s)CO(g)+H2(g)
The value of Kc for the reaction at 1000.0°C is 3.00 × 10–2.
kp=3.1354.
Calculate the equilibrium partial pressure of H2O given that PH2O = 0.442 atm and PCO = 5.000 atm at the start of the reaction. Assume that the carbon is in excess. =.2747
the partial pressure of CO is 5.1676
the equilibrium partial pressure of H2 is .1676
Determine the equilibrium partial pressure of H2O after CO and H2 at 0.0800 atm are added to the equilibrium mixture described above.
Determine the equilibrium partial pressure of CO after the addition described above
Determine the equilibrium partial pressure of H2 after the addition described above.
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