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1. A gas sample has a volume of 150 mL when the pressure is 175 kPa. If the temperature and amount of gas remains constant, what volume will the gas sample occupy at a pressure of 120 kPa?





2. A 650 mL sample of gas is collected at a room temperature of 300C. What volume will the sample have at 0.00C assuming the pressure of the gas remains constant?





3. An aerosol can of hair spray is filled to a pressure of 50.0 psi at a room temperature of 25.00C. Calculate the pressure inside the can if the can is placed in boiling water.





4. A balloon has a volume of 400.0 mL at a pressure of 600.0 mm Hg. Calculate the volume the balloon would have at standard atmospheric pressure if the temperature remains constant.





5. A car tire has a pressure of 30.0 psi at a temperature of 27.00C. Calculate the extremes of pressure caused by temperatures ranging from –20.00C (-4.000F) on a cold winter day to 50.00C (1220F) while being driven on a hot summer day.





6. A gas sample has a volume of 480 mL at a temperature of 370C and a pressure of 95.5 kPa. What volume would the gas occupy at STP?





7. If you collect 1.75-L of Hydrogen gas during a lab experiment, when the room temperature is 230C and the barometric pressure is 105 kPa, how many moles of hydrogen will you have?





8. What volume of gas would you expect to get from a 1.5-mole sample at 350C and 1.12 atm?

Sagot :

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From the gas laws, we can obtain that;

The final volume in the first question is 219 mL.

  • The final volume in the second question is 586 mL.
  • The final pressure in the third question is 63 Psi.
  • The final volume in the fourth question is 316 mL.
  • The pressure lies between  25.3 psi and 32.3 psi
  • The final volume in the fifth question is 398 mL.
  • The number of moles in the seventh question is 0.0035 moles.
  • The volume in the eighth question is 33.8 L.

What is gas law?

Gas laws stipulate the relationship between volume, pressure and temperature of gases based on the ideal gas approach.

1) V1 = 150 mL

P1 = 175 kPa

V2 = ?

P2 =  120 kPa

From Boyle's law;

P1V1 =P2V2

V2 = P1V1/P2

V2 = 175 kPa × 150 mL/120 kPa

V2 = 219 mL

2) V1 = 650 mL

   T1 = 30°C or 303 K

    V2 = ?

    T2 =  0.0°C or 273 K

V1/T1 = V2/T2

V1T2 = V2T1

V2 = V1T2/T1

V2 =  650 mL × 273 K/303 K

V2 = 586 mL

3) P1 =  50.0 psi

   T1 =  25.0°C or 298 K

   P2 = ?

   T2 = 100°C OR 373 K

P1/T1 = P2/T2

P1T2 = P2T1

P2 = P1T2/T1

P2 = 50.0 psi × 373 K/298 K

P2 = 63 Psi

4) V1 = 400.0 mL

  V2 = ?

  P1 =  600.0 mm Hg

  P2 = SP = 760 mmHg

P1V1 = P2V2

V2 = P1V1/P2

V2 = 600.0 mm Hg × 400.0 mL/760 mmHg

V2 = 316 mL

5) For the lower range;

P2 =  P1T2/T1

P2 = 30.0 psi × 253 K/300 K

P2 = 25.3 psi

For the higher range;

P2 =  P1T2/T1

P2 = 30.0 psi × 323 K/300 K

P2 = 32.3 psi

The pressure lies between  25.3 psi and 32.3 psi

6) P1V1/T1 = P2V2/T2

P1V1T2 = P2V2T1

V2 = P1V1T2/P2T1

  V2 = 480 mL × 95.5 kPa × 273 K / 101.325 kPa × 310 K

V2 = 398 mL

7) PV = nRT

n = PV/RT

P = 105 kPa or 0.049 atm

V =  1.75-L

R = 0.082 atm L K-1mol1-1

T = 23°C or 296 K

n = 0.049 atm ×  1.75-L/0.082 atm L K-1mol1-1 × 296 K

n = 0.0035 moles

8) PV = nRT

V = nRT/P

V = 1.5-mole × 0.082 atm L K-1mol1-1 × 308 K/ 1.12 atm

V = 33.8 L

Learn more about gas laws: https://brainly.com/question/8711877

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