Question

Use the References to access importal STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. Current international standards define STP as 0°C and 1 bar, which yield a molar volume of 22.7 L/mol. It is calculated that an experiment will yield 8.36 L of methane gas at STP. If the actual temperature is 42° C and the actual pressure is 622 mmHg, what volume of methane would result? (1 bar = 0.987 atm and 1 atm = 760 mmHg)____L

Answer 1

To convert the given volume of 8.36 L of methane gas at 42°C and 622 mmHg to the volume at STP, we can use the molar volume of a gas at STP, which is 22.4 L/mol. By setting up a proportion, we can calculate that the volume of methane gas at STP would be 8.35 L.

Step-by-step explanation:

To calculate the volume of methane gas at a given temperature and pressure, we can use the ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

However, in this case, we are given the volume at STP (Standard Temperature and Pressure), so we need to use the molar volume at STP as a conversion factor. At STP, one mole of any gas occupies a volume of 22.4 L.

We can use this information to convert the given volume of 8.36 L at 42°C and 622 mmHg to the volume at STP.

Conversion:

Given volume at 42°C and 622 mmHg: 8.36 L

Conversion factor: 22.4 L/mol

Since we are given the volume, we can set up a proportion:

8.36 L / X = 22.4 L / 1 mol

By cross-multiplying, we get:

X = (8.36 L × 1 mol) / 22.4 L

X = 0.373 mol

So, the volume of methane gas at STP would be 0.373 mol × 22.4 L/mol = 8.35 L (rounded to two decimal places).