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Pressure exerted by a mixture of $4 g$ of $O_{2}$ and $2 g$ of $H_{2}$ confined in a bulb of 1 litre at $0 ° C$ is

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31.205 atm

$25.215 a t m$

45.215 atm

15.210 atm

answer is A.

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Detailed Solution

The pressure can be calculated using the ideal gas equation:

P = (nRT) / V

Step 1: Calculate the moles of O₂ and H₂

Moles of O₂:

Molar mass of O₂ = 32 g/mol

Moles of O₂ = Mass / Molar mass = 4 / 32 = 0.125 mol

Moles of H₂:

Molar mass of H₂ = 2 g/mol

Moles of H₂ = Mass / Molar mass = 2 / 2 = 1 mol

Step 2: Total moles of gas in the mixture

n_total = n_O2 + n_H2 = 0.125 + 1 = 1.125 mol

Step 3: Calculate the pressure using the ideal gas equation

P = (nRT) / V

Substituting the values:

P = (1.125 × 0.0821 × 273) / 1

P = 25.215 atm

Final Answer: 25.215 atm (Option a)

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