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by BlastRoom
Practice applying PV = nRT with matching units and Kelvin temperatures.
#chemistry
24 questions
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How many moles of gas are in a 10.0 L container at 2.00 atm and 300 K? Use R = 0.0821 L·atm/(mol·K).
A 0.500 mol gas sample is at 298 K and 1.20 atm. What volume does it occupy? Use R = 0.0821 L·atm/(mol·K).
A 0.250 mol gas sample is in a 5.00 L flask at 350 K. What is its pressure? Use R = 0.0821 L·atm/(mol·K).
A gas occupies 18.5 L at 0.950 atm, and the sample contains 0.750 mol. What is the temperature? Use R = 0.0821 L·atm/(mol·K).
A 3.00 L flask contains 0.120 mol of gas at 27.0°C. What pressure does it exert? Use R = 0.0821 L·atm/(mol·K).
What amount of gas is in a 2.50 L container at 101.3 kPa and 298 K? Use R = 8.314 L·kPa/(mol·K).
A gas in a 1.50 L container has a pressure of 740 mmHg at 290 K. How many moles are present? Use R = 62.4 L·mmHg/(mol·K).
What volume is occupied by 0.0400 mol of gas at 800 mmHg and 310 K? Use R = 62.4 L·mmHg/(mol·K).
A sealed 12.0 L cylinder contains 1.50 mol of gas at 2.40 atm. What is the gas temperature? Use R = 0.0821 L·atm/(mol·K).
A 0.800 mol gas sample occupies 6.00 L at 310 K. What pressure does it exert in kPa? Use R = 8.314 L·kPa/(mol·K).
What volume does 1.25 mol of gas occupy at 2.00 atm and 25.0°C? Use R = 0.0821 L·atm/(mol·K).
A 500 mL bulb holds gas at 0.980 atm and 295 K. How many moles are inside? Use R = 0.0821 L·atm/(mol·K).
A gas-law problem gives pressure in atm, volume in liters, and temperature in kelvins. Which R value fits PV = nRT?
A sample has 98.0 kPa, 3.00 L, 0.150 mol, and 25.0°C. Which substitution is ready for PV = nRT?
Pressure is measured in mmHg, volume in liters, and temperature in kelvins. Which R value keeps the pressure unit unchanged?
A problem uses R = 0.0821 L·atm/(mol·K), but the pressure is 755 mmHg. Which pressure should go into PV = nRT?
You want to use R = 0.0821 L·atm/(mol·K) for a gas at 150 kPa. What pressure value matches that R?
Which temperature value should be used in PV = nRT for a gas at 18.0°C?
A 4.00 g sample of He is in a 22.4 L container at 273 K. The molar mass of He is 4.00 g/mol. What pressure does it exert? Use R = 0.0821 L·atm/(mol·K).
An 8.80 g sample of CO2 is in a 5.00 L container at 300 K. The molar mass of CO2 is 44.0 g/mol. What is the pressure? Use R = 0.0821 L·atm/(mol·K).
What volume will 14.0 g of N2 occupy at 1.00 atm and 27.0°C? The molar mass of N2 is 28.0 g/mol. Use R = 0.0821 L·atm/(mol·K).
A 1.60 g sample of CH4 is at 101.3 kPa and 298 K. The molar mass of CH4 is 16.0 g/mol. What volume does it occupy? Use R = 8.314 L·kPa/(mol·K).
A 3.20 g sample of O2 is sealed in a 2.00 L container at 25.0°C. The molar mass of O2 is 32.0 g/mol. What is the pressure? Use R = 0.0821 L·atm/(mol·K).
What mass of Ne is needed to fill a 10.0 L container to 1.50 atm at 300 K? The molar mass of Ne is 20.2 g/mol. Use R = 0.0821 L·atm/(mol·K).
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Solute, Solvent and the Dissolving Process
24 questions
