# A vessel of volume 11.2 L contains 2.0 mol of H2(g) and 1.0 mol of N2(g) at 273.15K. Calculate the total pressure and partial pressures of these gases.

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A vessel of volume 11.2 L contains 2.0 mol of H2(g) and 1.0 mol of N2(g) at 273.15K. Calculate the total pressure and partial pressures of these gases.

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Step 1

A vessel of volume 11.2 L contains 2.0 mol of H2(g) and 1.0 mol of N2(g) at 273.15K. The total pressure and partial pressures of these gases is to be calculated.

Step 2

Dalton’s Law of partial pressures-

According to this law, the total pressure exerted by a mixture of non- reacting gases is equal to the sum of the partial pressure of each gas in the mixture.

Step 3

Now, calculate the partial pressure of H2 (g) and N2 (g) in the vessel-

V = 11.2 L

T = 273.15 K

R = 0.082 L.atm.mol-1.K-1

n (H2) = 2.0 moles

n (N2) = 1.0 moles&nbs...

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