How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor?

Answer 1

This is the Sabatier process and is usually in need of high temperature and a metallic catalyst. So, balanced equation.

CO2 + 4H2 -> CH4 + 2H2O

As said, hydrogen is in excess, so CO2 is limiting and drives the reaction. One to one

36.6 moles CO2 (1 mole CH4/1 mole CO2)

= 36.6 moles CH4 produced in this reaction

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Answer 2

This is the Sabatier reaction or Sabatier process (the reaction of hydrogen with carbon dioxide at elevated temperatures and pressures in the presence of a nickel catalyst to produce methane and water) CO2 + 4H2 → CH4 + 2H2O

The hydrogen is required both to react with the carbon and the oxygen and all of this must be accounted for to produce the 76.6 moles of water. From the equation 4 moles of hydrogen reacts with 1 mole of carbon dioxide ot produce 2 moles of water. The production of 76.6 moles of water requires 153.2 moles of hydrogen.

Answer 3

48,1 moles Methane is equivalent to 48,1 moles carbon dioxide. If the reaction actually happen is a different story. It will be highly endothermic, that's for sure.

Answer 4

CO2+4H2 = CH4 + 2H20 (Balanced)

82.6 Moles.

The Ratio is 1 Mol CH4 over 1 Mol CO2.

So...

82.6 Mol CO2 * 1 Mol CH4/1 Mol CO2= 82.6 Moles of CH4

Answer 5

Use dimensional analysis:

(85.1 mol CO2)(1 mol CH4 / 1 mol CO2) = 85.1 mol CH4

Answer 6

Equation.

CO2 + H2 - CO + H2O

all one to one, so you need 53.6 moles of hydrogen gas

Answer 7

Q: How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor?

Answer 8

59.6 moles of methane are produced.

Answer 9

84,2 moles hydrogen are needed.