Question

5. The ideal gas law is as follows: PV = nRT, where P = pressure of the gas V = volume that the gas occupies n = moles of gas in the sample T = temperature of the gas R = ideal gas law constant (0.08206 L?atm/mole?K) a. What are the units of P, V and T in the ideal gas law? (2 points) b. An important relationship between the amount of gas present in a sample and the volume that it occupies is called the standard molar volume. It is calculated under conditions known as standard temperature and pressure or "STP" (1 atm pressure, 0 °C). Calculate the standard molar volume for a gas (i.e. the volume that one mole of gas occupies at STP). (5 points) c. At room temperature (25 °C) and 1 atm pressure, would you expect the volume that one mole of gas occupies to be larger, smaller or equal to the standard molar volume? Explain. (5 points) d. Considering your answer to part b, try the following stoichiometry problem: C2H4 reacts with O2 according to the following equation: C2H4(g) + O2(g) ? CO2(g) + H2O(g) What volume of oxygen at STP is needed to react with 1.50 moles of C2H4? (5 points) e. What is your answer to part d if the temperature is changed to 25 °C at 1 atm pressure (room temperature and pressure)? (5 points) 6. Given access to water, how might you be able to determine the volume of an empty container? (1 points)

          5. The ideal gas law is as follows: PV = nRT, where

P = pressure of the gas
V = volume that the gas occupies
n = moles of gas in the sample
T = temperature of the gas
R = ideal gas law constant (0.08206 L?atm/mole?K)

a. What are the units of P, V and T in the ideal gas law? (2 points)

b. An important relationship between the amount of gas present in a sample and the volume that it occupies is called the standard molar volume. It is calculated under conditions known as standard temperature and pressure or "STP" (1 atm pressure, 0 °C). Calculate the standard molar volume for a gas (i.e. the volume that one mole of gas occupies at STP). (5 points)

c. At room temperature (25 °C) and 1 atm pressure, would you expect the volume that one mole of gas occupies to be larger, smaller or equal to the standard molar volume? Explain. (5 points)

d. Considering your answer to part b, try the following stoichiometry problem:

C2H4 reacts with O2 according to the following equation: C2H4(g) + O2(g) ? CO2(g) + H2O(g)

What volume of oxygen at STP is needed to react with 1.50 moles of C2H4? (5 points)

e. What is your answer to part d if the temperature is changed to 25 °C at 1 atm pressure (room temperature and pressure)? (5 points)

6. Given access to water, how might you be able to determine the volume of an empty container? (1 points)

5. The ideal gas law is as follows: PV = nRT, where

P = pressure of the gas
V = volume that the gas occupies
n = moles of gas in the sample
T = temperature of the gas
R = ideal gas law constant (0.08206 L?atm/mole?K)

a. What are the units of P, V and T in the ideal gas law? (2 points)

b. An important relationship between the amount of gas present in a sample and the volume that it occupies is called the standard molar volume. It is calculated under conditions known as standard temperature and pressure or "STP" (1 atm pressure, 0 °C). Calculate the standard molar volume for a gas (i.e. the volume that one mole of gas occupies at STP). (5 points)

c. At room temperature (25 °C) and 1 atm pressure, would you expect the volume that one mole of gas occupies to be larger, smaller or equal to the standard molar volume? Explain. (5 points)

d. Considering your answer to part b, try the following stoichiometry problem:

C2H4 reacts with O2 according to the following equation: C2H4(g) + O2(g) ? CO2(g) + H2O(g)

What volume of oxygen at STP is needed to react with 1.50 moles of C2H4? (5 points)

e. What is your answer to part d if the temperature is changed to 25 °C at 1 atm pressure (room temperature and pressure)? (5 points)

6. Given access to water, how might you be able to determine the volume of an empty container? (1 points)

Added by Ashley S.

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