Question

A cylinder contains 0.200 mol of carbon dioxide (CO2) gas at a temperature of 30.0 ∘C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The cylinder is placed on a hot plate and a 920 J of heat flows into the gas, thereby raising its temperature to 124 ∘C. Assume that the CO2 may be treated as an ideal gas.

What is the change in internal energy of the gas?

Express your answer in joules to three significant figures.

Answer #1

A cylinder contains 1.5 moles of ideal gas, initially at a
temperature of 113 ∘C. The cylinder is provided with a frictionless
piston, which maintains a constant pressure of 6.4×105Pa on the
gas. The gas is cooled until its temperature has decreased to 27∘C.
For the gas CV = 11.65 J/mol⋅K, and the ideal gas
constant R = 8.314 J/mol⋅K.
1.Find the work done by the gas during this process.
2.What is the change in the internal (thermal) energy of...

An equilibrium mixture contains 0.500 mol of each of the
products (carbon dioxide and hydrogen gas) and 0.200 mol of each of
the reactants (carbon monoxide and water vapor) in a 1.00-L
container. CO(g) +H20 (g) --> <-- CO2 (g) + H2 (g) How many
moles of carbon dioxide would have to be added at constant
temperature and volume to increase the amount of carbon monoxide to
0.300 mol once equilibrium has been reestablished?

An equilibrium mixture contains 0.450 mol of each of the
products (carbon dioxide and hydrogen gas) and 0.200 mol of each of
the reactants (carbon monoxide and water vapor) in a 1.00-L
container
CO(g) + H2O(g) <===> CO2(g) + H2(g)
How many moles of carbon dioxide would have to be added at
constant temperature and volume to increase the amount of carbon
monoxide to 0.300 mol once equilibrium has been reestablished?

A Carbon dioxide fire extinguisher initially contains 5.5lbm of
CO2 gas. In “real life” the CO2 would not be
all gas, but for this problem assume that it is. The CO2
gas has an initial pressure of 860psia and initial temperature of
+72oF. Immediately after putting out a fire, it has a
final pressure of 100psia and a final temperature of
-30oF. Assume ideal gas law behavior.
a) Show that the specific gas constant for CO2 gas is
approximately R=1131ft∙lbf/(slug∙R)....

A 18.0-L tank of carbon dioxide gas (CO2) is at a pressure of
9.60 ✕ 105 Pa and temperature of 21.0°C. (a) Calculate the
temperature of the gas in Kelvin. K (b) Use the ideal gas law to
calculate the number of moles of gas in the tank. mol (c) Use the
periodic table to compute the molecular weight of carbon dioxide,
expressing it in grams per mole. g/mol (d) Obtain the number of
grams of carbon dioxide in the...

A 22.0-L tank of carbon dioxide gas (CO2) is at a
pressure of 9.90 ? 105 Pa and temperature of 18.0°C.
(a) Calculate the temperature of the gas in Kelvin.
_______ K
(b) Use the ideal gas law to calculate the number of moles of gas
in the tank.
mol
(c) Use the periodic table to compute the molecular weight of
carbon dioxide, expressing it in grams per mole.
______ g/mol
(d) Obtain the number of grams of carbon dioxide...

A cylinder of monatomic ideal gas is sealed in a cylinder by a
piston. Initially, the gas occupies a volume of 3.00 L and the
pressure is initially 105 kPa. The cylinder is placed in an oven
that maintains the temperature at a constant value. 65.0 J of work
is then done on the piston, compressing the gas (in other words,
the gas does −65.0 J of work). The work is done very slowly so that
the gas maintains a...

Carbon dioxide (CO2) is compressed in a
piston–cylinder assembly from p1 = 0.7 bar,
T1 = 280 K to p2 = 14 bar.
The initial volume is 0.2 m3. The process is described
by pV1.25 = constant.
Assuming ideal gas behavior and neglecting kinetic and potential
energy effects, determine the work and heat transfer for the
process, each in kJ, using constant specific heats evaluated at 300
K, and data from Table A-23.

The following table provides some information on carbon dioxide
solubility in water.
C
(mol/L)
P
(atm)
k
(mol/L⋅atm)
T
(∘C)
3.80×10−2
1.00
20.0
4.90×10−2
20.0
1.00
3.40×10−2
25.0
At 1 atm, how many moles of CO2 are released by raising the
temperature of 1 liter of water from 20∘C to 25∘C?

One gram-mole of ideal gas is contained in a piston-cylinder
assembly. Cp=(7/2)R, Cv=(5/2)R. The gas expands from 3 to 1 atm.
Heat of 1000J is transferred to the gas during the process.
External pressure maintains at 1 atm throughout. Initial
temperature of the gas is 300K. Find work and internal energy
change.

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