Standards D v. I It’s the law! Calculate It! Dalton 100 100 100 100 100 200 200 200 200 200 300 300 300 300 300 400 400 400 400 400 500 500 500 500 500

Standard temperature is: A. 273°C B. 273 K C. 101.3 °C D. 0 K $100 Standard temperature is: A. 273°C B. 273 K C. 101.3 °C D. 0 K B

Standard Pressure is: A. 101.3 atm B. 101.3 kPa C. 273 atm D. 273 kPa $200 Standard Pressure is: A. 101.3 atm B. 101.3 kPa C. 273 atm D. 273 kPa B

$300 To convert Celsius to Kelvin you: A. add 273 B. subtract 273 C. multiply 273 D. add 101.3 A

$400 To convert atm to kPa you: A. add 273 B. add 101.3 C. multiply by 273 D. multiply by 101.3 D

$500 mmHg stands for: A. millimeters of hydrogen gas B. millimeters of mercury C. millimeters of helium gas D. millimeters of chlorine B

$100 When both variables increase or decrease at the same rate, the equation is said to be: Direct Inverse A

A direct equation = A. x/y B. x*y $200 A direct equation = A. x/y B. x*y A

An inverse equation produces a: Line graph Curved graph No change $300 An inverse equation produces a: Line graph Curved graph No change B

$400 Which of the following is an inverse relationship? A. Boyle’s Law B. Charles’ Law C. Gay-Lussac’s Law A

$500 Assuming temperature and pressure are constant, which of the following statements is correct? A. Equal volumes of different gases have the same mass. B. Equal volumes of different gases contain the same number of moles. C. Equal masses of different gases have the same volume. D. Equal masses of different gases contain the same number of moles. B

$100 Boyle’s Law relates what two variables? A. Volume & pressure B. Volume & temperature C. Temperature & pressure D. Pressure & moles of gas A

The gas particles move closer together causing the can to collapse $200 When a steaming hot soda can is placed in ice cold water the can collapses. Which of the following explains this phenomenon? The gas particles move closer together causing the can to collapse The gas particles shrink The number of gas particles striking the inside wall of the can decreases A

$300 Which of the following equations correctly relates the two variables? A. P1/V1 = P2/V2 B. V1/T1 = V2/T2 C. P1T1 = P2T2 D. P1N1 = P2N2 B

$400 If the volume is held constant, increasing the temperature of a gas will increase the pressure of a gas. How does the kinetic-molecular theory of gases explain this? At higher temperatures, the gas molecules have … A. Greater mass, and collisions with the walls of the container occur with greater force. B. Higher velocity and therefore there are more collisions with the walls of the container. C. Dissociate into smaller molecules, and since there are more molecules there are more collisions with the walls of the container. D. Some of the gas molecules condense to a liquid B

$500 Which of the following statements is true about ideal gases? A. They have a volume B. They are not attracted to each other C. A real gas is an ideal gas at all temperature and pressures D. An ideal gas conforms to the ideal gas law only at STP B

$100 When the volume of a gas is tripled, what happens to the pressure? A. It is tripled B. It is divided by 3 C. It is cubed D. No change B

$200 If the volume is 2 L and then changes to 4 L, the temperature will change from… A. 200 K to 100 K B. 200 K to 800 K C. 200 K to 400 K D. 400 K to 200 K C

$300 You are given P1, V1, and V2. P2 = A. (P1*V1)/V2 B. (V1*V2)/P1 C. (P1*V2)/V1 A

$400 A sample of gas occupies a volume of 2.00 liters at a temperature of 10.0°C. What volume will the gas occupy at 100.°C assuming the pressure remains constant? A. 1.52 liters B. 2.64 liters C. 20.0 liters D. 52800 liters B

$500 What volume would be occupied by 0.50 moles of gas at STP? A. 1.5 L B. 1.3 L C. 11 L D. 45 L C

$100 There are three gases. Gas A exerts 1 mmHg pressure, Gas B exerts 3 mmHg, Gas C exerts 2 mmHg. What is the total pressure? A. 3 mmHg B. 4 mmHg C. 5 mmHg D. 6 mmHg D

$200 There are 3 gases in a system. Gas A has 5 particles, Gas B has 7 particles, Gas C has 2 particles. Which gas exerts the most pressure? A. Gas A B. Gas B C. Gas C B

$300 When we blow up a balloon, we add more gas particles to the balloon. This increases the pressure because: A. the force of each gas particle is increased B. the number of particles hitting the wall of the balloon is increased C. the force of each gas particle is decreased B

$400 A container with two gases, helium and argon, is 30% by volume helium. Calculate the partial pressure of argon if the total pressure inside the container is 5.00 atm. A. 1.50 atm B. 2.00 atm C. 3.50 atm D. 5.00 atm C He: 1.5 = .3 * 5 Ar: 3.5 = .7 * 5

$500 There is a mixture of gases in a container. Gas A has 10 particles. Gases B and C each have 5 particles. The total pressure is 6 atm. What is the partial pressure of Gas A? A. 3 atm B. 4 atm C. 6 atm D. 10 atm A

Dalton’s Law The contribution each gas in a mixture makes to the total pressure is called the partial pressure exerted by that gas. In a mixture of gases, the total pressure is the sum of the partial pressures of the gases. Ptotal = P1 + P2 + P3 + … A- 10 / 20 = 0.50 * 6.0 atm = 3.0 atm B- 5 / 20 = 0.25 * 6.0 atm = 1.5 atm C- 5 / 20 = 0.25 * 6.0 atm = 1.5 atm