Question
In: Physics
A hydrostatic system consists of 0.1 moles of an ideal gas whose specific heat capacity at...
A hydrostatic system consists of 0.1 moles of an ideal gas whose
specific heat capacity at constant volume, ??, is equal to 3?2
where R is the gas constant equal to 8.31 J mol–1 K–1. Its initial
pressure and volume are 32 Pa and 8 m3. In its final state, the
pressure is just 1 Pa and its volume increases eightfold. The
particular thermodynamic process can be represented on an indicator
diagram as a straight line joining the initial and final
states.
(a) Determine a relationship between the pressure and the volume of
the gas that represents the thermodynamic process.
(b) Establish a relationship between the temperature and the volume
of the gas valid for the thermodynamic process.
(c) Determine the volume of the gas when the temperature is a
maximum.
(d) Determine the temperature of the gas at the initial and final
states, and the maximum temperature attained by the gas in the
process.
(e) Imagine that the gas, while following the thermodynamic process
outlined above, is at some arbitrary state such that its volume is
V. This state is somewhere between the initial and final states.
Determine the heat exchange that occurs while the gas is traversing
(along the process) from the initial to the arbitrary state. Your
expression should be a function of V only.
(f) With reference to part (e), determine that volume which
corresponds to maximum heat exchange. Hence determine the
corresponding temperature.
Solutions
genius_generous answered 2 years agoRelated Solutions
3.0 moles of an ideal gas with a molar heat capacity at constant volume of 4.9...
3.0
moles of an ideal gas with a molar heat capacity at constant volume
of 4.9 cal/(mol·K) and a molar heat capacity at constant pressure
of 6.9 cal/(mol·K) starts at 300 K and is heated at constant
pressure to 320 K, then cooled at constant volume to its original
temperature. How much heat flows into the gas during this two-step
process?
The ideal gas heat capacity of nitrogen varies with temperature. It is given by: Cp =...
The ideal gas heat capacity of nitrogen varies with temperature.
It is given by: Cp = 29.42-(2.170 *10-3) T +
(0.0582*10-5) T2 + (1.305*10-8)
T3 – (0.823*10-11) T4. T is in K
and Cp is in Joule/(mole K). Assuming that N2 is an ideal gas:
A) How much internal energy (per mole) must be added to nitrogen
to increase its temperature from 450 to 500 K.
B) Repeat part A for an initial temperature of 273 K and final
temperature...
A 2.00 mol sample of an ideal gas with a molar specific heat of CV =...
A 2.00 mol sample of an ideal gas with a molar specific heat of
CV =
5
2
R
always starts at pressure 1.00 ✕
105
Pa and temperature 350 K. For each of the following
processes, determine the final pressure (Pf, in kPa), the final volume
(Vf, in
L), the final temperature (Tf, in K), the change in
internal energy of the gas (ΔEint,
in J), the energy added to the gas by heat (Q, in J), and
the...
A 2.00 mol sample of an ideal gas with a molar specific heat of CV =...
A 2.00 mol sample of an ideal gas with a molar specific heat of
CV = (5/2)R always
starts at pressure 2.00 ✕ 105 Pa and temperature 300 K.
For each of the following processes, determine the final pressure
(Pf, in kPa), the final volume
(Vf, in L), the final temperature
(Tf, in K), the change in internal
energy of the gas (ΔEint, in J), the energy
added to the gas by heat (Q, in J), and the work done...
A 1.50 mol sample of an ideal gas with a molar specific heat of CV =...
A 1.50 mol sample of an ideal gas with a molar specific heat of
CV = 5/2 R always
starts at pressure 2.00 ✕ 105 Pa and temperature 250 K.
For each of the following processes, determine the final pressure
(Pf, in kPa), the final volume
(Vf, in L), the final temperature
(Tf, in K), the change in internal
energy of the gas (ΔEint, in J), the energy
added to the gas by heat (Q, in J), and the work...
Heat Capacity Learning Goal: To understand the concepts of heat capacity, specific heat, and molar heat...
Heat Capacity
Learning Goal:
To understand the concepts of heat capacity, specific heat, and
molar heat capacity.
Heat capacity, C, is the amount of energy required to
raise the temperature of a substance by exactly 1 degree Celsius.
The energy needed to warm an object increases as the mass of that
object increases. We see this in our everyday life. For example, we
know that it takes much more energy to heat a large tank of water
than a small...
An ideal gas has a constant volume specific heat cv as a function of temperature. Find...
An ideal gas has a constant volume specific heat cv as a
function of temperature. Find the
change in internal energy and enthalpy if the gas is heated from a
temperature of 300K to 600K.
cv(T) = 716.66 + 0.4T + 0.000667T2 J/kg.K
Also, sketch the constant pressure specific heat as a function
of temperature and mention the
point T = 400K on the cp – T diagram. Assume that the gas constant
of the given ideal gas is
286.9...
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) When 117 J of energy is supplied as heat to 2.00 moles of an ideal...
(a)
When 117 J of energy is supplied as heat to 2.00 moles of an ideal
gas at constant
pressure, the temperature rises by 2.00 K. Calculate the molar heat
capacity at constant
pressure, CP,m and the molar heat capacity at constant volume, CV,m
for the gas. By
considering the two heat capacities, determine whether the gas is
monatomic or diatomic.
(b)
Explain what isothermal processes and adiabatic processes are,
and the differences
between them, taking care to explain the...
In the specific heat experiment, critical factors are the heat capacity of the calorimeter, the temperature...
In the specific heat experiment, critical factors are the heat
capacity of the calorimeter, the temperature of the holt sample,
and the final temperature of the calorimeter. What effect could
influence the temperature of the hot sample at the instant it is
inserted into the calorimeter? What issues surround the measurement
of the final calorimeter temperature?
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