Question

*Why is the following situation impossible?* An ideal gas
undergoes a process with the following parameters: *Q* =
10.0 J, *W* = 12.0 J, and Δ*T* = −2.00°C.

Answer #1

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2.15 mol of an ideal gas with CV,m=3R/2
undergoes the transformations described in the following list from
an initial state described by T=350.K and
P=5.00bar.
1) The gas undergoes a reversible adiabatic expansion until the
final pressure is one-fourth its initial value.
2) The gas undergoes an adiabatic expansion against a constant
external pressure of 1.25 bar until the final pressure is
one-fourth its initial value.
3)The gas undergoes an expansion against a constant external
pressure of zero bar until...

Consider 1.00 mol of an ideal gas (CV = 3/2 R)
occupying 22.4 L that undergoes an isochoric (constant volume)
temperature increase from 298 K to 342 K. Calculate ∆p, q , w, ∆U,
and ∆H for the change.
For Units, pressure in atm and the rest in J.

A certain ideal gas undergoes an isovolumetric process that
decreases the pressure. Does heat flow into or out of the gas
during this process? How do you know?

Consider the following four-process cycle that is carried out on
a system of monatomic ideal gas, starting from state 1 in which the
pressure is 88.0 kPa and the volume is 3.00 liters.
Process A is an isothermal process that triples the
volume;
process B is a constant volume process that returns the system to a
pressure of 88.0 kPa;
process C is an isothermal process that returns the system to a
volume of 3.00 liters;
and process D is...

1. a) Suppose 2 moles of a monatomic ideal gas
occupies 5 m3 at a pressure of 1600 Pa.
First: Find the temperature of the gas in Kelvin.
Answer: 481 K
Second: Find the total internal energy of the gas.
Answer:12000 J
1. b) Suppose the gas undergoes an isobaric
expansion to a volume of 7 m3.
(Don’t forget to include + and – in each of the
problems below)
First: Find Q
Answer: 8000 J
Second: Find W
Answer:...

Exactly 1.27 moles of an ideal gas undergoes an isothermal
expansion (T = 259 K) from state A to state B and then returns to
state A by another process. The volume of the gas in state B is
three times its initial volume.
(a) For the process AB, find the work done by the gas and its
change in entropy. work = J change in entropy = J/K
(b) Find the gas's change in entropy for the process BA....

1 mole of a gas undergoes a mechanically reversible isothermal
expansion from an initial volume 1 liter to a final volume 10 liter
at 25oC. In the process, 2.3 kJ of heat is absorbed in the system
from the surrounding. The gas follows the following formula:
V=RTP+b where V is the molar specific volume, and Tand Pare
temperature (abosolute) and gas pressure respectively. Given R=
8.314 J/(mol.K) and b= 0.0005 m3. Evaluate the following a) Work
(include sign) b) Change...

An ideal diatomic gas contracts in an isobaric process from 1.15
m3 to 0.600 m3 at a constant pressure of 1.70
✕ 105 Pa. If the initial temperature is 445 K, find the
work done on the gas, the change in internal energy, the energy
transfer Q, and the final temperature.
(a) the work done on the gas (in J)
(b) the change in internal energy (in J)
(c) the energy transfer Q (in J)
(d) the final temperature (in...

An ideal gas underwent a process in which it absorbed 7.5 J of
energy as heat and undergoes an expansion in which it performed 5.0
J of work on its surroundings. If the expansion was performed
against a pressure of 101325 Pa, what was the volume change (ΔV)
for the expansion? Express your result in units of m^3. (Note: 1 J
= 1 Pa m^3).

One mole of an ideal gas is compressed at a constant temperature
of 55 oC from 16.5 L to 12.8 L using a constant external
pressure of 1.6 atm. Calculate w, q, ΔH and ΔS for this
process.
w = (?) kJ
q = (?) kJ
ΔH = (?) kJ
ΔS = (?) J/(mol*K)

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