Question

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4. At what temperature, in celsius, will 37.2 g of methane, CH4, exert a pressure of 905.0 torr with a volume of 2.35 L

5. determine the mass of a sample ammonia, NH3, that has a volume of 115 mL at a pressure of 0.922 atm and a temperature of 45° C

6. what is the density of 2.3 mol of ethane gas, C2H6, at a pressure of 194.3 kPa and a temperature of 25.6° C?

7. a metal canister has a volume of 859 mL. it’s pressure is 0.750 atm when 0.0445 mol of gas are pumped into the canister . what is the temperature for the gas in K?

Answer 1

4. The temperature at which 37.2 g of methane, CH4, exerts a pressure of 905.0 torr with a volume of 2.35 L is 63.7°C.

5. The mass of a sample of ammonia, NH3, that has a volume of 115 mL at a pressure of 0.922 atm and a temperature of 45°C is 1.82 g.

6. The density of 2.3 mol of ethane gas, C2H6, at a pressure of 194.3 kPa and a temperature of 25.6°C is 3.50 g/L.

7. The temperature for the gas in K when 0.0445 mol of gas is pumped into a metal canister with a volume of 859 mL and a pressure of 0.750 atm is 448 K.

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Answer 2

1. The volume of gas is 193.548 L.

2. The temperature T of CO2 is 8.867 K.

3. The moles (n) of helium gas is 0.070 mol.

4. The temperature T of methane is 694.94 K.

5. The mass of ammonia is 0.069723 g.

6. Density of 2.3 mol of ethane gas is approximately 1.199 mol/L.

7. The temperature (T) is approximately 176.45 K

1. **Volume of Gas:** Use the ideal gas law PV = nRT to find the volume (\(V\)) when given moles (n), temperature (T), and pressure P. Convert temperature to Kelvin (K).

`\[ V = (nRT)/(P) \]`

`\[ V = \frac{(4.3 \, \text{mol})(8.314 \, \text{J/mol}\cdot\text{K})(28 + 273.15 \, \text{K})}{165.2 \, \text{kPa}} \]`

Therefore, the volume of gas is 193.548 L.

2. **Temperature of CO2:** Use the ideal gas law to find the temperature (\(T\)) when given pressure (\(P\)), volume (\(V\)), and mass (\(m\)).

`\[ T = (PV)/(nR) \]\\T = \frac{(968 \, \text{mmHg})(25.12 \, \text{L})}{(44.01 \, \text{g/mol})(0.0821 \, \text{L}\cdot\text{atm/mol}\cdot\text{K})} \]`

Therefore the temperature T of CO2 is 8.867 K

3. **Moles of Helium Gas:** Use the ideal gas law to find moles (\(n\)) when given volume (\(V\)), temperature (\(T\)), and pressure (\(P\)). Convert temperature to Kelvin.

`\[ n = (PV)/(RT) \]`

`\[ n = \frac{(745 \, \text{mmHg})(1.75 \, \text{L})}{(0.0821 \, \text{L}\cdot\text{atm/mol}\cdot\text{K})(298.15 \, \text{K})} \]`

Therefore, the moles (n) of helium gas is 0.070 mol.

4. **Temperature of Methane:** Use the ideal gas law to find temperature (\(T\)) when given pressure (\(P\)), volume (\(V\)), and mass (\(m\)). Convert pressure to atm.

`\[ T = (PV)/(nR) \]`

`\[ T = \frac{(905.0 \, \text{torr})(2.35 \, \text{L})}`
`{(37.2 \, \text{g/mol})(0.0821 \, \text{L}\cdot\text{atm/mol}\cdot\text{K})} \]`

Therefore, the temperature T of methane is 694.94 K.

5. **Mass of Ammonia:** Use the ideal gas law to find mass (\(m\)) when given volume (\(V\)), temperature (\(T\)), and pressure (\(P\)). Convert temperature to Kelvin.

`\[ m = (PV)/(RT) \]`

`\[ m = \frac{(0.922 \, \text{atm})(0.115 \, \text{L})}{(0.0821 \, \text{L}\cdot\text{atm/mol}\cdot\text{K})(318.15 \, \text{K})} \]`

Therefore, the mass of ammonia is 0.069723g

6. **Density of Ethane Gas:** Calculate density (\(D\)) using the formula \
`(D = (n)/(V)\)` with moles (\(n\)) given, and convert pressure to atm.

`\[ D = (n)/(V) \]`

`\[ D = \frac{2.3 \, \text{mol}}{\frac{194.3 \, \text{kPa}}{101.325 \, \text{kPa/atm}}} \]`

Therefore, Density of 2.3 mol of ethane gas is approximately 1.199 mol/L.

7. **Temperature for Gas:** Use the ideal gas law to find temperature (\(T\)) when given volume (\(V\)), pressure (\(P\)), and moles (\(n\)). Convert pressure to atm.

`\[ T = (PV)/(nR) \]`

`\[ T = \frac{(0.750 \, \text{atm})(0.859 \, \text{L})}{(0.0445 \, \text{mol})(0.0821 \, \text{L}\cdot\text{atm/mol}\cdot\text{K})} \]`

Therefore, the temperature (T) is approximately 176.45 K

The probable question may be:

1. 4.3 moles of a gas are at a temperature of 28°C with a pressure of 165.2 kPa. What volume does the gas occupy?

2.163 g CO2 has a volume of 25.12 L at a pressure of 968 mmHg.

What is the temperature of the CO2 in "C?

3.How many moles of helium gas will it take to fill a balloon with a volume of 1.75 L when the temperature is 25°C and the atmospheric pressure is 745 mmHg?

4. At what temperature, in celsius, will 37.2 g of methane, CH4, exert a pressure of 905.0 torr with a volume of 2.35 L

5. determine the mass of a sample ammonia, NH3, that has a volume of 115 mL at a pressure of 0.922 atm and a temperature of 45° C

6. what is the density of 2.3 mol of ethane gas, C2H6, at a pressure of 194.3 kPa and a temperature of 25.6° C?

7. a metal canister has a volume of 859 mL. it’s pressure is 0.750 atm when 0.0445 mol of gas are pumped into the canister . what is the temperature for the gas in K?