A 7.50 × 10^-³-m³ bottle contains 0.0200 kg of oxygen gas, O₂, at 77.0 °C. What is the pressure exerted on the inner walls of the flask by the oxygen gas? Note: the atomic mass of O is 15.9994 u.

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of oxygen gas in the bottle using the formula:

n = m/M

where n is the number of moles, m is the mass of the gas, and M is the molar mass of the gas.

n = 0.0200 kg / (15.9994 g/mol) = 1.250 x 10^-3 mol

Next, we can use the ideal gas law to calculate the pressure of the gas:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

We need to convert the volume of the bottle from mL to m^3:

V = 7.50 x 10^-6 m^3

We also need to convert the temperature from °C to K:

T = 77.0 + 273.15 = 350.15 K

We can now substitute these values into the ideal gas law:

P = nRT/V = (1.250 x 10^-3 mol)(8.314 J/mol K)(350.15 K)/(7.50 x 10^-6 m^3) = 2.43 x 10^5 Pa

Therefore, the best answer choice is (C), 2.43 x 10^15 Pa.

A 750 × 10-3-M3 Bottle Contains 0

A 750 × 10^-³-M³ Bottle Contains 0