Calculate the approximate volume of a 1.50 mol sample of gas at 300k and a pressure of 3.75 atm.
4. pressure co2 = 760 mm hg volume co2 = 2.965 l temperature co2= 25.5 °c
how many moles of co2 were produced?
5. what instrument do you measure pressure with?
6. the volume of a gas is 500 ml at 20.0 k. what will be the new temperature if the gas is compressed to 100 ml?
. the volume of a sample of oxygen is 200.0 ml when the pressure is 4.0 atm and the temperature is 37.0 °c. what is the new temperature if the volume increases to 400.0 ml and the pressure decreases to 2.000 atm?
8. the pressure on a 2.00l sample of co2(g) is increased from 50 kpa to 100 kpa. what is the new volume of the gas?
9. the temperature of a 2.0 liter sample of helium gas at stp is increased to 37°c, and the pressure is decreased to 80 kpa. what is the new volume of the helium sample?

3. 9.84 L.

4. 0.1211 mol.

5. Barometer, Bourdon tube, and Aneroid barometers.

6. 4.0 K.

7. 310 K.

8. 1.0 L.

9. 2.637 L.

Explanation:

3. Calculate the approximate volume of a 1.50 mol sample of gas at 300K and a pressure of 3.75 atm.

where, P is the pressure of the gas in atm (P = 3.75 atm).

V is the volume of the gas in L.

n is the no. of moles of the gas in mol (n = 1.5 mol).

R is the general gas constant (R = 0.082 L.atm/mol.K),

T is the temperature of the gas in K (T = 300 K).

∴ V = nRT/P = (1.5 mol)( 0.082 L.atm/mol.K)( 300 K)/(3.75 atm) = 9.84 L.

4. Pressure CO2 = 760 mm Hg Volume CO2 = 2.965 L Temperature CO2= 25.5 °C . How many moles of CO2 were produced?

∵ P = 760 mmHg = 1.0 atm, V = 2.965 L, T = 25.5°C + 273 = 298.5 K, R = 0.082 L.atm/mol.K.

∴ n = PV/RT = (1.0 atm)(2.965 L)/(0.082 L.atm/mol.K)(298.5 K) = 0.1211 mol.

5. What instrument do you measure pressure with?

Barometer, Bourdon tube, and Aneroid barometers.

6. The volume of a gas is 500 mL at 20.0 K. What will be the new temperature if the gas is compressed to 100 mL?

If n and P are constant, and have two different values of V and T:

V₁T₂ = V₂T₁

V₁ = 500 mL, T₁ = 20 K.

V₂ = 100 mL, T₂ =??? K.

∴ T₂ = V₂T₁/V₁ = (100 mL)(20 K)/(500 mL) = 4.0 K.

7. The volume of a sample of oxygen is 200.0 mL when the pressure is 4.0 atm and the temperature is 37.0 °C. What is the new temperature if the volume increases to 400.0 mL and the pressure decreases to 2.000 atm?

P₁V₁T₂ = P₂V₂T₁

P₁ = 4.0 atm, V₁ = 200 mL, T₁ = 37°C + 273 = 310 K.

P₂ = 2.0 atm, V₂ = 400 mL, T₂ =??? K.

∴ T₂ = P₂V₂T₁/P₁V₁ = (2.0 atm)(400 mL)(310 K)/(4.0 atm)(200 mL) = 310 K.

8. The pressure on a 2.00L sample of CO2(g) is increased from 50 kPa to 100 kPa. What is the new volume of the gas?

P₁V₁ = P₂V₂

P1 = 50 kPa, V1 = 2.0 L.

P₂ = 100 kPa, V₂ = ??? L.

∴ V₂ = P₁V₁/P₂ = (50 kPa)(2.0 L)/(100 kPa) = 1.0 L.

9. The temperature of a 2.0 liter sample of helium gas at STP is increased to 37°C, and the pressure is decreased to 80 kPa. What is the new volume of the helium sample?

P₁V₁T₂ = P₂V₂T₁

P₁ = 1.0 atm (standard P), V₁ = 2.0 L, T₁ = 25°C + 273 = 298 K (standard T).

P₂ = 80 kPa = 0.789 atm, V₂ = ??? L, T₂ = 37°C + 273 = 310 K.

V₂ = P₁V₁T₂/P₂T₁ = (1.0 atm)(2.0 L)(310 K)/(0.789 atm)(298 K) = 2.637 L.

aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.