The weight of one mole of gas, also known as the molar mass, can be calculated using the ideal gas law and the definition of standard temperature and pressure (STP).

1. The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.

2. At STP, the pressure is 1 atm, the volume is 22.4 L (the volume occupied by one mole of any gas at STP), and the temperature is 273.15 K.

3. We can rearrange the ideal gas law to solve for n (the number of moles): n = PV/RT.

4. Substituting the STP conditions into this equation gives n = (1 atm * 22.4 L) / (0.0821 L atm K-1 mol-1 * 273.15 K) = 1 mole.

5. The density of a substance is its mass divided by its volume. So, the mass of one mole of the gas is its density times its volume: (1.78 g/L) * (22.4 L) = 39.872 g.

So, the weight of one mole of this gas is approximately 39.872 g.

Question

The weight of one mole of gas, also known as the molar mass, can be calculated using the ideal gas law and the definition of standard temperature and pressure (STP).

1. The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.

2. At STP, the pressure is 1 atm, the volume is 22.4 L (the volume occupied by one mole of any gas at STP), and the temperature is 273.15 K.

3. We can rearrange the ideal gas law to solve for n (the number of moles): n = PV/RT.

4. Substituting the STP conditions into this equation gives n = (1 atm * 22.4 L) / (0.0821 L atm K-1 mol-1 * 273.15 K) = 1 mole.

5. The density of a substance is its mass divided by its volume. So, the mass of one mole of the gas is its density times its volume: (1.78 g/L) * (22.4 L) = 39.872 g.

So, the weight of one mole of this gas is approximately 39.872 g.

Knowee AI · Accepted Answer

The weight of one mole of gas, also known as the molar mass, can be calculated using the ideal gas law and the definition of standard temperature and pressure (STP).

1. The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.

2. At STP, the pressure is 1 atm, the volume is 22.4 L (the volume occupied by one mole of any gas at STP), and the temperature is 273.15 K.

3. We can rearrange the ideal gas law to solve for n (the number of moles): n = PV/RT.

4. Substituting the STP conditions into this equation gives n = (1 atm * 22.4 L) / (0.0821 L atm K-1 mol-1 * 273.15 K) = 1 mole.

5. The density of a substance is its mass divided by its volume. So, the mass of one mole of the gas is its density times its volume: (1.78 g/L) * (22.4 L) = 39.872 g.

So, the weight of one mole of this gas is approximately 39.872 g.

The density of a gas is 1.78 g L-1 at STP. The weight of one mole of gas is

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