Question

hydrogen gas and oxygen gas react in the clouds to produce water vapor. if the temperature in the atmosphere is 16oc and the pressure is 0.855 atm, what volume of hydrogen gas would be needed to produce 155 g of water?

Answer 1

The balanced chemical equation for the reaction is:

2 H2 (g) + O2 (g) → 2 H2O (g)

From the equation, we can see that 2 moles of hydrogen gas react to form 2 moles of water vapor.

We can use the ideal gas law to calculate the volume of hydrogen gas needed. The ideal gas law is:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, we need to calculate the number of moles of water vapor produced from 155 g of water:

moles of H2O = mass/molar mass = 155 g/18.015 g/mol = 8.610 mol

Since 2 moles of hydrogen gas react to form 2 moles of water vapor, we need 4.320 moles of hydrogen gas:

moles of H2 = 2 × moles of H2O = 2 × 8.610 mol = 17.220 mol

Now we can use the ideal gas law to calculate the volume of hydrogen gas needed:

V = nRT/P = (17.220 mol)(0.0821 L·atm/mol·K)(289 K)/(0.855 atm) ≈ 536 L

Therefore, approximately 536 liters of hydrogen gas would be needed to produce 155 g of water vapor at 16°C and 0.855 atm pressure.

Step-by-step explanation:

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