How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 88.1 molesmoles of water vapor?

Express your answer with the appropriate units.

88.1 moles of H₂

Explanation:

Let's make the reaction:

H₂(g) + CO₂(g) → H₂O(g) + CO(g)

Ratio is 1:1

Therefore, 1 mol of hydrogen reacts with 1 mol of carbon dioxide to produce 1 mol of water and 1 mol of carbon monoxide.

In conclusion, 88.1 moles of water must be produced by 88.1 moles of H₂

The reaction can also be written as an equilbrium

H₂(g) + CO₂(g) ⇄ H₂O(g) + CO(g)           Kc

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.