In: Chemistry

For 1 mol of an ideal gas, Pexternal = P = 1 atm. The temperature is changed from 125ºC to 25.0ºC, and CV,m = 3/2R. Calculate (all units are J) q= , w= , ∆U= , and ∆H= . Please enter your answers with 2 decimals in E notation, such as 2.33E4 (=23345). If the answer is negative, please do not forget the negative sign. If answer is zero, please just enter 0 without decimal.

Suppose 1.0 mol of an ideal gas is initially at P=4.0
atm and T=400 K. It is expanded irreversibly and adiabatically
against a constant pressure of 1.0 atm until the volume has
doubled.
(a) Calculate the final volume of the gas.
(b) Calculate w, q, and energy change ΔU of this process, in
joules.
(c) Calculate the final temperature of the gas.
(d) Calculate the entropy change ΔS of the ideal gas in the
process.
(e) What is the entropy...

An ideal gas with 7 degrees of freedom begins at a pressure of
8.5 atm, temperature of 25 degrees Celsius and volume of 120L.
A) How many moles of gas are there?
B) The gas expands isobarically to 200L. What is the new
temperature?
C) How much work was done in the expansion?
D) By how much did the internal energy increase?
E) What amount of heat flowed into the gas?
G) The gas then depressurizes isochorically to the original...

The temperature of 2.00 mol of an ideal monatomic gas is raised
15.0 K at constant volume. What are (a) the work W done by the gas,
(b) the energy transferred as heat Q , (c) the change
?Eint in the internal energy of the gas, and (d) the
change ?K in the average kinetic energy per atom

An ideal monatomic gas at an initial temperature of 500 K is
expanded from 5.0 atm to a final pressure of 1.0 atm. Calculate
w, q, DU, and (where applicable)
DH and DT when the expansion is performed (a)
reversibly and isothermally, and (b) reversibly and
adiabatically.
Help Please!!!

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...

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.

1. A sample of nitrogen gas at a pressure of 0.947 atm and a
temperature of 213 °C, occupies a volume of 687 mL. If the gas is
cooled at constant pressure until its volume is 570 mL, the
temperature of the gas sample will be 2. A helium-filled weather
balloon has a volume of 615 L at 23 °C and 754 mm Hg. It is
released and rises to an altitude of 7.93 km, where the pressure is
323...

Use the ideal gas law to complete the table:
P
V
n
T
1.06 atm
1.25 L
0.105 mol
___
115 torr
___
0.249 mol
309 K
___
28.2 mL
1.81×10−3 mol
26.0 ∘C
0.565 atm
0.440 L
___
257 K

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
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.

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