U6 Gas Laws

Boyles Law

100

What is the formula for Boyle's Law

P1V1=P2V2

200

What is the relationship between pressure and volume?

inverse

300

NO MATH

The pressure on 400 mL of gas is at standard pressure. Will the volume be bigger or smaller if the pressure changes to 5 atm?

smaller volume

400

The pressure on 5 L of carbon dioxide gas changes from 680 mmHg to standard pressure. What will the new volume be? 

4.47 L

500

The volume of a gas at 10 atm is doubled. What will be the final pressure?

5 atm

Charles Law

100

what is the formula for charles's law?

v1/T1 = v2/T2

200

What is the relationship between volume and temperature?

direct

300

Give a specific example for the relationship between volume and temperature?

answers vary (balloon station / tire example)

400

If the volume of a gas changes from 10 L to 100 L, what will the new temperature be if the gas was originally 273 K?

2730 K

500

What will be the new volume of 75 mL of hydrogen gas if the temperature changes from 10^oC to 60^oC?

88.3 mL

Gay-Lussacs

100

what is the formula for gay-lussac's law?

P1/T1 = P2/T2

200

what is the relationship between pressure and temperature?

direct

300

When using this formula, temperature needs to be in what unit?

Kelvin

400

A gas has a pressure of 50 mmHg at 540 K. What will be the pressure at 200 K?

18.5 mmHg

500

The pressure in a car tire is 2 atm at 30^oC. During the day, the temperature rises and the pressure of the tire increases to 2.5 atm. What is the temperature of the gas? 

378.75 K

Combined

100

What is the formula for the combined gas law?

(P1V1)/T1 = (P2V2)/T2

200

How do you convert ^oC to K? 

K= ^oC + 273

300

What is the standard pressure you would use in this problem: 

Calculate the volume of a gas at STP if the gas occupies 500 mL at 750 mmHg at 27 ^oC?

760 mmHg

400

A container with an initial volume of 1 L is occupied by a gas at a pressure of 1.5 atm at 298 K. The pressure increases to 6 atm as the temperature rises to 373 K. What is the new volume?

0.31 L

500

If a gas occupies a volume of 100 mL at a pressure of 760 mmHg at 27^oC, what volume will the gas occupy at 800 mmHg at 50^oC? 

102.3 mL

Ideal

100

What is the formula for the Ideal gas law?

PV=nRT

200

What units must the variable be in to use the formula?

P=atm

V= L

n=mol

R= .082 atmL/molK

T = K

300

What is wrong with the way this problem is written?

What volume will 2 moles of chlorine gas occupy at 770 mmHg and 295K? 

Pressure needs to be in atm

400

How many moles are in a 4 L balloon at 1 atm and 273K. R= 0.082

0.179 mol

500

What volume will 3 moles of chlorine gas occupy at 1 atm and 295 K? R = 0.082

72.57 L