If 4.71 moles of an ideal gas has a pressure of 3.55 atm, and a volume...

If 4.71 moles of an ideal gas has a pressure of 3.55 atm, and a volume of 26.09 L, what is the temperature of the sample in degrees Celsius?

Expert Solution

Ans. Using ideal gas equation-

PV = nRT - equation 1

Where, P = pressure in atm

V = volume in L

n = number of moles

R = universal gas constant= 0.0821 atm L mol^-1K^-1

Putting the values in equation 1-

3.55 atm x 26.09 L = 4.71 mol x (0.0821 atm L mol^-1K^-1) x T

Or, T = 92.61650 atm L / (0.386691 atm L K^-1)

Hence, T = 239.52 K

Hence, temperature, T = (239.52 – 273.15)⁰C = -33.63⁰C

queen_honey_blossom answered 2 years ago

The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature.

The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature. If the initial volume of the as is 472 mL. what is the final volume of the gas? A 4.00 L sample of gas is cooled from 71 CC to a temperature at which its volume is 2.60 L. What is this new temperature? Assume no change in pressure of the gas. A scuba diver releases a...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ; the volume of the gas changes from 3.20×10-2 m3 to 4.50×10−2 m3 . a. Calculate the initial temperature of the gas. b. Calculate the final temperature of the gas. c. Calculate the amount of work the gas does in expanding. d. Calculate the amount of heat added to the gas. e. Calculate the change in internal energy of the gas.

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ; the volume of the gas changes from 3.30×10−2 m3 to 4.50×10−2 m3 . a) Calculate the initial temperature of the gas. b) Calculate the final temperature of the gas. c) Calculate the amount of work the gas does in expanding. d) Calculate the amount of heat added to the gas. e) Calculate the change in internal energy of the gas

An ideal monatomic gas originally at a pressure of 3x105 Pascals and 75 moles and volume...

An ideal monatomic gas originally at a pressure of 3x105 Pascals and 75 moles and volume 1.2 m3 & Ti is expanded isothermally to a volume of 3.5 m3 at which point it has pressure P1. It then experiences an isovolumic process to a lower pressure P2, T2. Finally, it is compressed adiabatically back to its original state and returns to its original pressure, temperature, and volume. Find: Ti , P1 , P2 , T2 ΔE1 of gas, ΔE2 of...

3. 2 moles of an ideal gas at 17oC has a pressure of 760mm mercury, and...

3. 2 moles of an ideal gas at 17oC has a pressure of 760mm mercury, and is compressed once isothermally and then adiabatically until its volume is halved [in each case reversibly and from identical initial conditions]. The gas constant is 8.314J/kg. The density of the mercury is 13.60g/cm3 . [Express all your answers in MKS units e.g. volume in cubic meter, pressure in Pascal, Temperature in Kelvin, etc.] (a) Express the pressure of the gas in units of Pascal....

A piston contains 620 moles of an ideal monatomic gas that initally has a pressure of...

A piston contains 620 moles of an ideal monatomic gas that initally has a pressure of 2.92 × 105 Pa and a volume of 4.1 m3. The piston is connected to a hot and cold reservoir and the gas goes through the following quasi-static cycle accepting energy from the hot reservoir and exhausting energy into the cold reservoir. The pressure of the gas is increased to 5.92 × 105 Pa while maintaining a constant volume. The volume of the gas...

A fixed number of moles of an ideal gas are kept in a container of volume...

A fixed number of moles of an ideal gas are kept in a container of volume V and an absolute temperature T. If T doubles while V is held constant, the new net internal energy of the gas will be ________ times the original internal energy of the gas. A: 1/4 B: 1/2 C: 1/sqrt(2) D: equal to E: sqrt(2) F: 2 G: 4 If T and V are both doubled, the new r.m.s. velocity of the molecules in the...

A sample of an ideal gas at 1.00 atm and a volume of 1.46 L was...

A sample of an ideal gas at 1.00 atm and a volume of 1.46 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 10.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

A sample of an ideal gas at 1.00 atm and a volume of 1.02 L was...

A sample of an ideal gas at 1.00 atm and a volume of 1.02 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 45.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

If 5.0 moles of an ideal gas occupies a volume of 9.3 L, what volume will...

If 5.0 moles of an ideal gas occupies a volume of 9.3 L, what volume will 15.0 moles of the gas occupy? A mixture of oxygen, hydrogen, carbon dioxide and methane gases has a total pressure of 1.3 atm. If the partial pressure of hydrogen is 2.4 psi, the partial pressure of carbon dioxide is 110 torr and the partial pressure of methane is 0.22 atm, how many mmHg does the oxygen exert? For the reaction below, how many mL...

Question