The Gas Laws Unit Test Review And Test 96%

The gas in the piston is at constant temperature. A student increases the pressure on the piston from 2 atm to 3 atm. The observation will be summarized in a row of the incomplete table below. Which row of the table and which observation would the student fill?

Which best defines partial pressure in a mixture of gases?

If a gas is moved from a large container to a small container but its temperature and number of moles remain the same, what would happen to the pressure of the gas?

Which statement can best be concluded from the ideal gas law?

If 6.00 g of carbon is burned completely, what volume of carbon dioxide gas is released at STP?

The pressure of 1 mol of gas is decreased to 0.5 atm at 273 K. What happens to the molar volume of the gas under these conditions?

If the pressure, volume, and temperature of a gas are known, which can most likely be found by using the ideal gas law?

The table below shows a comparison of the different gas laws. Some cells have been left blank. Which are assumed to be constant while using the combined gas law?

Consider this reaction. mc030-1.jpg What volume (in milliliters) of oxygen gas is required to react with 4.03 g of Mg at STP?

The volume of a gas is 450 mL when its pressure is 1.00 atm. If the temperature of the gas does not change, what is the pressure when its volume is changed to 2.00 L?

How many moles of oxygen (O2) are present in 33.6 L of the gas at 1 atm and 0°C?

Which describes the volume of 1 mol of gas at standard temperature and pressure?

According to the equation 2Na + 2H2O mc012-1.jpg 2NaOH+H2, what mass of Na is required to yield 22.4 L of H2 at STP? (The atomic mass of Na is 22.99 u.)

Which correctly defines molar volume of an ideal gas?

Consider the equation. mc016-1.jpg Which represents the correct mass-volume relationship at STP?

Which law is based on the graph that is shown below?

Which law relates temperature, pressure, volume, and the number of moles of a gas under perfect conditions?

Which law states that the pressure and absolute temperature of a fixed quantity of gas are directly proportional under constant volume conditions?

What volume would 3.01•1023 molecules of oxygen gas occupy at STP?

The gas in the piston is being heated, and the piston has moved upward. The observation will be summarized in a row of the incomplete table below. mc023-1.jpg What are the variables for this piston?

A balloon that had a volume of 3.50 L at 25.0°C is placed in a hot room at 40.0°C. If the pressure remains constant at 1.00 atm, what is the new volume of the balloon in the hot room?

A student uses 0.0821 L• atm/mol • K as the value of the gas constant. What is most likely true about the variables in the ideal gas law?

The absolute temperature of a gas is increased four times while maintaining a constant volume. What happens to the pressure of the gas?

Consider the proportionality below. mc009-1.jpg What does this best represent?

Which law states that the volume of a gas is proportional to the moles of the gas when pressure and temperature are kept constant?

Which quantity is held constant when working with Boyle's, Charles's, and Gay-Lussac's laws?

The gases listed are at standard temperature and pressure: · 1 mol of CO2 gas · 1 mol of N2 gas · 2 mol of O2 gas Which statement is correct?

The ideal gas constant, R has several different values that could be used. Which quantity causes these differences?

Consider the reaction. C(s) + O2(g) -> CO2(g) How many grams of carbon should be burned in an excess of oxygen at STP to obtain 2.21 L of carbon dioxide?

A scientist is examining a mixture of nitrogen, hydrogen, and ammonia. The individual pressures that are exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively. If the total pressure is 0.90 atm, what is the partial pressure of ammonia?

Which law is described by saying that when the pressure of a gas in a sealed container is cut in half, the gas will double in volume at a steady temperature?

What is the volume of 0.200 mol of an ideal gas at 200. kPa and 400. K?

A tire at 21°C has a pressure of 0.82 atm. Its temperature decreases to -3.5°C. If there is no volume change in the tire, what is the pressure after the temperature change?

Shana solves stoichiometry problems using the equation for the synthesis of water. 2H2(g) + O2(G) -> 2H2O(g) Which interpretation of the balanced equation would cause Shana to make a mistake?

Consider the reaction. 3Mg(s) + 2H3PO4(aq) -> Mg3(PO4)2(s) + 3H2(g) Which statement is true at STP? (The atomic mass of Mg is 24.31 u.)

The volume of a gas decreases to half of its original volume, but the gas maintains the same number of moles and temperature. According to the ideal gas law, what will most likely happen to the pressure?

Which proportionality shows the result of combining Avogadro's law with Boyle's law?