Question

 1. A sample of air at 0.750 atm is expanded from 250.0 mL to 650.o mL. If the temperature remains constant, what is the final pressure in atm:

 2. What is the final volume of argon gas if 2.50 L at 705 torr is compressed to a pressure of 1550 torr? Assuming the temperature remains constant:

 Charles Law; Convert OC to Kelvin

 3. Calculate the final Celsius temperature of hydrogen chloride gas if o.500 L at 35°C is heated until the volume reaches 1.26 L. Assuming the pressure remains constant:

 4. A 335 mL sample of oxygen at 25°C is heated to 50°C. If the pressure remains constant, what is the final volume in milliliters:

Answer 1

1)

Given:

Pi = 0.750 atm

Vi = 250 mL

Vf = 650 mL

use:

Pi*Vi = Pf*Vf

0.750 atm * 250.0 mL = Pf * 650.0 mL

Pf = 0.2885 atm

Answer: 0.289 atm

2)

Given:

Vi = 2.50 L

Pi = 705 torr

Pf = 1550 torr

use:

Pi*Vi = Pf*Vf

705 torr * 2.50 L = 1550 torr * Vf

Vf = 1.1371 L

Answer: 1.14 L

3)

Given:

Ti = 35.0 oC

= (35.0+273) K

= 308 K

Vi = 0.500 L

Vf = 1.26 L

use:

Vi/Ti = Vf/Tf

0.5 L / 308.0 K = 1.26 L / Tf

Tf = 776.16 K

Tf = 503 oC

Answer: 503 oC

4)

Given:

Vi = 335 mL

Ti = 25.0 oC

= (25.0+273) K

= 298 K

Tf = 50.0 oC

= (50.0+273) K

= 323 K

use:

Vi/Ti = Vf/Tf

335 mL / 298.0 K = Vf / 323.0 K

Vf = 363 mL

Answer: 363 mL

Only 4 parts at a time