How many grams of co(g) are there in 74.5 ml of the gas at 0.933 atm and 30o c?

As per the given statement: Using ideal gas law equation: where P represents the Pressure of a gas V represents the Volume it occupies R represents the Universal constant , usually given as: R = 0.082 atm L/ mol k First convert Celsius into Kelvin. T = 273 + 30 = 303 K Use conversion: 1 L = 1000 mL V = 74.5 mL = L Now substitute the given values we have; Simplify: n = 0.00279757305 or n ≈0.0028 moles. Since carbon monoxide, CO has molar mass of 28.01 g/mol then; g Therefore, 0.078 g of CO(g) are there in 74.5 mL of the gas at 0.933 atm and 30 degree C

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