1.00 mol of oxygen gas (O₂) is heated at constant pressure of 1.00 atm from 10.0°C to 25.0°C. What is the change of volume of the gas in this process? A) 1.23 L B) 0.86 L C) 1.88 L D) 2.09 L

Question

Quizplus · Accepted Answer

The change in volume can be calculated using the ideal gas law and the concept of molar volume at standard temperature and pressure (STP). At STP, 1 mole of any gas occupies 22.4 L. The change in temperature is from 10.0°C to 25.0°C, which is a 15.0°C increase. Using the formula for the change in volume ΔV = nRΔT/P (where n is the number of moles, R is the ideal gas constant in L·atm/(mol·K), ΔT is the change in temperature in Kelvin, and P is the pressure in atm), and converting the temperature change to Kelvin, we can calculate the change in volume. Given that R = 0.0821 L·atm/(mol·K), n = 1.00 mol, ΔT = 15.0 K (since a change in degrees Celsius is equivalent to a change in Kelvin), and P = 1.00 atm, the calculation yields a change in volume close to 1.23 L, making option A correct.

100 Mol of Oxygen Gas (O2) Is Heated at Constant

100 Mol of Oxygen Gas (O₂) Is Heated at Constant