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1. How many moles of oxygen will occupy a volume of 2.50 liters at 121.6 kPa and 331 K?
2. An unknown volume of chlorine gas (Cl2) is resting at 127 °C at a of pressure 152.4 kPa. If the gas weighs 191.4 g, what is the volume?
3. A 2.917 mole sample of an ideal gas at 285 K occupies a volume of 4.3 L. What is the pressure of the gas?
4. At what temperature would 2.10 moles of Kr gas have a pressure of 111.1 kPa and in a 25.0 L tank?
5. What is the volume of 146.2 grams of nitrogen gas (N2) molecules at STP?
6. What mass (NOT moles) of CO2 is needed to fill an 80.0 L tank to a pressure of 150.0 kPa at 27.0°C?
1. PV = nRT
2. PV = nRT and n = grams/molar mass
3. PV = nRT
4. {V = nRT
5. mols = grams/molar mass, then mols x 22.4L/mol at STP
6. PV = nRT, then n = grams/molar mass.
Remember in these problems that if you you atmospheres for pressure then R is 0.08206. If you use P in kPa, then R is 8.314.
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Sure! I'll go through each question and show you the steps to find the answers.
1. To find the number of moles of oxygen, we can use the ideal gas equation, which is PV = nRT. We are given the volume (2.50 L), pressure (121.6 kPa), and temperature (331 K). The gas constant (R) is 8.314 J/(mol·K). Plugging in these values into the equation, we can solve for n (moles of oxygen):
n = PV / RT
= (121.6 kPa) * (2.50 L) / (8.314 J/(mol·K) * (331 K)
Note: It's important to convert the pressure from kPa to Pa and the volume from liters to cubic meters if using these specific units of gas constant (R).
2. To find the volume of chlorine gas, we can use the ideal gas equation again. This time, we are given the temperature (127 °C), pressure (152.4 kPa), and mass (191.4 g). First, we need to convert the temperature from Celsius to Kelvin (K). Then, we can rearrange the ideal gas equation to solve for volume (V):
V = (nRT) / P
We need to find moles (n), which can be obtained using the given mass and molar mass of chlorine gas (Cl2) from the periodic table. Then, we can substitute the values into the equation to find V.
3. To find the pressure of the gas, we can rearrange the ideal gas equation again. This time, we are given the moles (2.917 mol), temperature (285 K), and volume (4.3 L). Plugging in these values, we can rearrange the equation to solve for pressure (P):
P = (nRT) / V
4. To find the temperature, we once again rearrange the ideal gas equation. This time, we are given the moles (2.10 mol), pressure (111.1 kPa), and volume (25.0 L). Plugging in these values, we can solve for temperature (T):
T = (PV) / (nR)
5. To find the volume of nitrogen gas at STP (standard temperature and pressure), we can use the equation PV = nRT. At STP, the pressure is 1 atm (or 101.3 kPa) and the temperature is 273 K. We are given the molar mass of nitrogen gas (N2) from the periodic table and the mass of the gas (146.2 g). First, find the moles (n) using the given mass and molar mass, and then substitute the values into the equation to solve for volume (V).
6. To find the mass of CO2 needed, we first need to convert the temperature from Celsius to Kelvin (K). Then, we can rearrange the ideal gas equation to solve for the mass (m):
m = (PV) / (RT)
We are given the volume (80.0 L), pressure (150.0 kPa), and temperature (27.0 °C). Plugging in these values and using the molar mass of CO2 from the periodic table, we can solve for the mass.