Question

In: Physics

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.

Pi =

For parts (b) through (h) assume the initial pressure of the gas is 1.013 × 105P a

(b) What is the initial volume of the gas?

Vi =

Consider the isothermal process:

(c) What is the final pressure of the gas?

Pf =

(d) What is the work done on the gas[careful with the sign]?

W =

(e) What is heat leaving the system[careful with the sign]?

Q = Consider now the adiabetic process:

(f) What is the final pressure of the gas?

Pf =

(g) What is the final Temperature of the gas?

Tf =

(h) What is the work done on the gas

W =

(i) Plot the two processes in the same P vs V diagram qualitatively[but accurately] and label clearly the adiabatic and the isothermal curves. (P along vertical axis and V along horizontal axis)

Expert Solution

genius_generous answered 1 year ago

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?

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...

. Three moles of an ideal gas (CV,m =3/2R ) is compressed at 25℃, at pressure...

. Three moles of an ideal gas (CV,m =3/2R ) is compressed at 25℃, at pressure of 1 atm to 75 atm, with a surrounding maintained at 25℃. The process was performed at condition (i) Reversible and (ii) against constant external pressure of 0.80 atm. Calculate the following q, W, ∆U,∆H, for each path

Refer to diagram 2. A flask contains 78.2 moles of a monatomic ideal gas at pressure...

Refer to diagram 2. A flask contains 78.2 moles of a monatomic ideal gas at pressure 8.33 atm and volume 49 liters. point A on the graph. Now, the gas undergoes a cycle of three steps: - First there is an isothermal expansion to pressure 1.74 atm (point B on the graph). - Next, there is an isochoric process in which the pressure is raised to P1 (point C on the graph). - Finally, there is an isobaric compression back...

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.

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...

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

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm...

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm are expanded reversible to 1 atm end pressure. Calculate w, q, ΔU, ΔH values in case of expansion of this expansion by isothermal and adiabatic way.

Which of the following statements are correct for 2 moles of an ideal gas? 1) A...

Which of the following statements are correct for 2 moles of an ideal gas? 1) A plot of P versus T at constant V will give a straight line. 2) A plot of V versus T at constant P will give a straight line having a slope = R / P. 3) A plot of PV /T versus P will give a straight line having a zero slope. 4) A plot of PV versus T will give a straight line...

1.00 moles of a gas is at a temperature of 273 Kelvin and has a pressure...

1.00 moles of a gas is at a temperature of 273 Kelvin and has a pressure of 1.00x105Pa. What is its initial volume? STEP 1: Its pressure is doubled while keeping its volume constant. What is its temperature after this step? STEP 2: Its temperature is held constant while it it is reduced back to its initial pressure. What is the the volume after this step? Draw a PV diagram showing the two step (it doesn’t have to have numbers,...