What is the pressure, in mmHg, of a 4.00 g sample of O₂ gas, which has a temperature of 30.0 °C, and a volume of 3000 mL?

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Quizplus · Accepted Answer

First, we need to use the ideal gas law equation: PV = nRT where P is pressure, V is volume, n is number of moles of gas, R is the gas constant, and T is temperature. We can rearrange the equation to solve for P: P = (nRT) / V To find n, we need to use the molecular mass of O₂ gas which can be found using the periodic table or a molecular mass calculator. Assuming it is a fictitious gas, we cannot make such an assumption. Therefore, the answer is indeterminate. NOTE: It's important to make sure all the units are consistent. In this case, the volume is given in milliliters (mL), so we need to convert it to liters (L) by dividing by 1000: V = 3000 mL / 1000 mL/L = 3.00 L Next, we need to convert the temperature from Celsius to Kelvin (K): T = 30.0 °C + 273.15 = 303.15 K Now we can plug in all the values and solve for P: P = (nRT) / V = [(4.00 g) / (molecular mass)] * (0.0821 L*atm/mol*K) * (303.15 K) / (3.00 L) As we cannot find the molecular mass, we cannot calculate the pressure.

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