CHEMISTRY NEED HELP?

1)
Pressure, P = 58.8 psi = (58.8 psi) × (0.068046 atm/psi) = 4.00 atm
Volume, V = 60.0 L
No. of moles, n = ? mol
Gas constant, R = 0.08206 L atm / (mol K)
Temperature, T = (273.2 + 27.0) K = 300.2 K

Gas law: PV = nRT
Then, n = PV/(RT)

No. of moles of C₂H₂, n = 4.00 × 6.00 / (0.08206 × 300.2) mol = 0.974 mol

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2)
Gas X : Rate₁ = 1 unit, MM₁ = 128 g/mol
Gas Y: Rate₂ = 2 units, MM₂ = ? g/mol

Rate₁/Rate₂ = √(MM₂/MM₁)
1/2 = √(MM₂/128)
[√(MM₂/128)]² = (1/2)²
MM₂/128 = 1/4
Molar mass of gas Y, MM₂ = 128 × (1/4) g/mol = 32 g/mol