Question

Initial   Pressure   Initial   Temperature   Final   Temperature   Final   Pressure   (a) 276 torr 324 K 240 K ×...

Initial
  Pressure  
Initial
  Temperature  
Final
  Temperature  
Final
  Pressure  
(a) 276 torr 324 K 240 K

×

10 torr
(b) 916 torr 23

°

C
227 K

×

10 torr
(c) 2.74 atm 164

°

C
25

°

C
atm

Homework Answers

Answer #1

a)

Given:

Pi = 276 torr

Ti = 324.0 K

Tf = 240.0 K

use:

Pi/Ti = Pf/Tf

276 torr / 324.0 K = Pf / 240.0 K

Pf = 204 torr

Answer: 204 torr

b)

Given:

Pi = 916 torr

Ti = 23.0 oC

= (23.0+273) K

= 296 K

Tf = 227.0 K

use:

Pi/Ti = Pf/Tf

916 torr / 296.0 K = Pf / 227.0 K

Pf = 702 torr

Answer: 702 torr

c)

Given:

Pi = 2.74 atm

Ti = 164.0 oC

= (164.0+273) K

= 437 K

Tf = 25.0 oC

= (25.0+273) K

= 298 K

use:

Pi/Ti = Pf/Tf

2.74 atm / 437.0 K = Pf / 298.0 K

Pf = 1.87 atm

Answer: 1.87 atm

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
One mole of ideal gas initially at 300 K is expanded from an initial pressure of...
One mole of ideal gas initially at 300 K is expanded from an initial pressure of 10 atm to a final pressure of 1 atm. Calculate ΔU, q, w, ΔH, and the final temperature T2 for this expansion carried out according to each of the following paths. The heat capacity of an ideal gas is cV=3R/2. 1. A reversible adiabatic expansion.
A sample of gas inside a 150 mL piston has an initial temperature of 550 K...
A sample of gas inside a 150 mL piston has an initial temperature of 550 K and pressure of 9.9 atm. As the piston expands to 650 mL, the pressure decreases to 1.5 atm. What is the final temperature (in K) of the gas? Remember that the ideal gas constant (R) has the same value for all gases, so P1V1/n1T1 = P2V2/n2T2. Also remember that the amount of gas remains constant in this problem (n1 = n2). Select one: a....
At temperature of 273 K and pressure of 1.00 × 10−2 atm, the density of a...
At temperature of 273 K and pressure of 1.00 × 10−2 atm, the density of a monatomic gas is 1.24 × 10−5g/cm3. Also, we know 1 atm = 1.01 × 105 Pa, R = 8.31 J/mol.K and ? = 1.38 × 10−23 J/K. (a) Find ???? for the gas particles. (b) Find the molar mass of the gas.
5.00 moles of a gas sample has a pressure of 600 torr at 400 K. What...
5.00 moles of a gas sample has a pressure of 600 torr at 400 K. What is the pressure (in torr) if the amount of gas is changed to 9.00 moles and temperature to 600 K (volume of gas is constant?). a) 540 b) 1,620 c) 1,260 d) 420
The initial temperature of three moles of oxygen gas is 40.0°C, and its pressure is 6.30...
The initial temperature of three moles of oxygen gas is 40.0°C, and its pressure is 6.30 atm. (a) What will its final temperature be when heated at constant volume so the pressure is five times its initial value? 1292 Correct: Your answer is correct. °C (b) Now the volume of the gas is also allowed to change. Determine the final temperature if the gas is heated until the pressure and the volume are doubled.
150 grams of C2H6 an ideal gas has an initial pressure of 9120 mmHg and a...
150 grams of C2H6 an ideal gas has an initial pressure of 9120 mmHg and a temperature of 300 K. At a constant temperature and moles, the gas changes to a final pressure is 2280 mmHg. a) Calculate the initial and final volumes (L) b) Calculate the work done (in kJ) for the gas volume change if it is carried out against a constant external pressure of 6 atm. (1 L atm = 101.325 J) c) Using answer 5b, is...
A vessel with a movable piston contains 1.90 mol of an ideal gas with initial pressure...
A vessel with a movable piston contains 1.90 mol of an ideal gas with initial pressure Pi = 2.03 ✕ 105 Pa, initial volume Vi = 1.00 ✕ 10−2 m3, and initial temperature Ti = 128 K. (a) What is the work done on the gas during a constant-pressure compression, after which the final volume of the gas is 2.50 L? J (b) What is the work done on the gas during an isothermal compression, after which the final pressure...
The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure...
The solubility of CO2 in a salt water lake at 298 K and 750 torr pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous solution. The Henry’s Law constant in this case is 3.0 x 10-2 mol/L.atm. Please find the partial pressure of CO2 (g) (PCO2, in atm) in the air above the lake (2) Please use your answer to determine the percentage of CO2 in the atmosphere (2) Given the percentage of CO2 in the atmosphere...
Calculate the final temperature, in degrees Celsius, for each of the following, if n and V...
Calculate the final temperature, in degrees Celsius, for each of the following, if n and V are constant. A. A sample of xenon gas at 31 ∘C and 800. mmHg is cooled to give a pressure of 560. mmHg . B. A tank of argon gas with a pressure of 0.940 atm at -14 ∘C is heated to give a pressure of 1450 torr .
A typical barometric pressure in Denver, Colorado, is 615 mm Hg. What is this pressure in...
A typical barometric pressure in Denver, Colorado, is 615 mm Hg. What is this pressure in atmospheres and kilopascals? Supposewehaveasampleofammoniagaswithavolumeof3.5Latapressureof 1.68 atm. The gas is compressed to a volume of 1.35 L at a constant temperature. Calculate the final pressure. A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT