Question

A sample of oxygen gas collected at a pressure of 1.43 atm and a temperature of 304 K is found to occupy a volume of 711 milliliters. How many moles of O₂ gas are in the sample?

= mol

Answer 1

By applying the Ideal Gas Law, the number of moles of O₂ gas in the sample is calculated to be 0.039 moles.

Step-by-step explanation:

The student's question involves calculating the number of moles of O₂ gas present in a sample with known pressure, volume, and temperature. By using the Ideal Gas Law, PV = nRT, where P is the pressure in atmospheres, V is the volume in liters, n is the number of moles of gas, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin, we can solve for n.

• In order to use the Ideal Gas Law, we need to convert the volume from milliliters to liters by dividing by 1000 (711 mL / 1000 = 0.711 L).
• Plugging these values into the Ideal Gas Law equation we get:

1.43 atm × 0.711 L = n × 0.0821 L·atm/mol·K × 304 K

Solving for n we find:

n = (1.43 atm × 0.711 L) / (0.0821 L·atm/mol·K × 304 K)

n = 0.039 moles of O₂