What is the pressure in atm of 0.47mol of a gas in a 1.7L container at 276K?

1 answer:

5 0

The answer is 1. A sample of 0.50 moles of gas is placed in a container of volume of 2.5 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.89 atm = 3719 torr

2. A sample of gas is placed in a container at 25oC and 2 atm of pressure. If the temperature is raised to 50oC, what is the new pressure? P = 2.17 atm

3. At 1 atm of pressure water boils at 100oC, if the sample was placed under 2 atm of pressure, what would be the temperature? (This would be like a pressure cooker).
T = 746 K = 473oC = 883oF

4. At what temperature would water boil if the pressure is 600 torr? (Use information from problem 3: this shows why food doesn't cook well at higher elevations)
T = 294 K = 21.5oC = 70.7oF

5. Calculate the volume of 40.6 g of F2 at STP. V = 23.9 L

6. A sample of 2.0 moles of hydrogen gas is placed in a container with a volume of 10.4 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.70 atm = 3576

7. The tire pressure is 32 psi. What is the pressure in torr if 1 atm = 14.7 psi?
P = 1654 torr

8. A gas is placed in a balloon with a volume of 3.0 L at 28oC and 900 torr. What would be the new volume for the gas if placed under STP? V = 3.2 L

9. How many moles of gas would occupy a volume of 14 L at a pressure of 700 torr and a temperature of 30oC? n = 0.52 mol

10. Calculate the volume of 24.0 g of HCl at STP. V = 14.8 L

11. What is the volume of one mole of acetylene gas at STP? V =22.414 L

12. What is the volume of 0.75 mol of gas at 72oC and 2 atm? V = 10.6 L

13. After eating beans, a student collects a sample of gas at 0.97 atm and 26oC which occupies a volume of 3.5 L, calculate its volume at STP. V = 3.1 L

14. Ammonia (NH3) is placed in 1.5 L flask at 25oC. If the pressure of the gas is 0.899 atm, what is the density? d = 0.626 g/L

15. A mixture of Ar and CO gases is collected over water at 28oC and an atmospheric pressure of 1.05 atm. If the partial pressure of Ar is 600 torr, what is the partial pressure of CO? (vapor pressure of water at 28oC is 28.3 mmHg) PCO = 0.223 atm

16. Determine the partial pressures of each of the gases in the following mixture: 17.04 g NH3, 40.36 g Ne and 19.00 g F2. The gases are at 1.5 atm of pressure.
PNH3 = 0.428 atm; PNe = 0.857 atm; PF2 = 0.2124 atm

17. Potassium chlorate decomposes under heat as follows:

2 KClO3 (s) -------> 2 KCl (s) + 3 O2 (g)

The oxygen gas is collected over water at 25oC. The volume of gas is 560 mL measured at 1 atm. Calculate the number of grams of KClO3 used in the reaction. (vapor pressure of water = 0.0313 atm) nO2 = 0.022 mol; 1.81 g KClO3

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1, When temperature is increased the volume will also increase. this is because the particles will gain kinetic energy and bombard the walls of the container of the gas at a higher frequency, therefore, for the pressure to remain constant as per Charles' law, the volume will have to increase so that the rate of bombardment remains constant. This is explained by the Charles law which states that the volume of a gas is directly proportional to the absolute temperature provided pressure remains constant.

2. When temperature is Decreased the volume will also Decrease. this is because the particles will loose kinetic energy and bombard the walls of the container of the gas less frequently, therefore, for the pressure to remain constant as per Charles' law, the volume will have to reduce so that the rate of bombardment remains constant. This is explained by the Charles law which states that the volume of a gas is directly proportional to the absolute temperature provided pressure remains constant.

3. When temperature is increased the pressure will increase. This is because the gas particles gain kinetic energy and bombard the walls of the container more frequently. this is according to Pressure law which states that for a constant volume of a gas the pressure is directly proportional to absolute temperature

4. When temperature is decreased, pressure will decrease, This is because the gas particles lose kinetic energy and bombard the walls of the container less frequently. this is according to Pressure law which states that for a constant volume of a gas the pressure is directly proportional to absolute temperature

5. When particles are added, pressure will increase. This is because the bombardment per unit area also increases. Boyles law explains this, that at fixed temperature the volume of a gas is inversely proportional to the pressure.

6. When particles are removed, the pressure will decrease. This is because the bombardment per unit area also decreases. Boyle's law explains this, that at fixed temperature the volume of a gas is inversely proportional to the pressure.

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