Question

Consider 14.61 moles of an ideal diatomic gas. (a) Find the total heat capacity of the gas at (i) constant volume and (ii) constant pressure assuming that the molecules translate and vibrate but do not rotate. Be sure to clearly explain how the equipartition of energy is used to solve this problem. (b) Repeat problem (a) above except assume that the molecules translate, rotate and vibrate.

Answer #1

The heat capacity at constant pressure of a certain amount of a
diatomic gas is 13.2 J/K.
(a) Find the number of moles of the gas.
(b) What is the internal energy of the gas at T = 312
K?
(c) What is the molar heat capacity of this gas at constant
volume?
(d) What is the heat capacity of this gas at constant volume?

The heat capacity at constant pressure of a certain amount of a
diatomic gas is 13.2 J/K.
(a) Find the number of moles of the gas.
(b) What is the internal energy of the gas at T = 312
K?
(c) What is the molar heat capacity of this gas at constant
volume?
(d) What is the heat capacity of this gas at constant
volume?

Ivan heats at constant pressure 2.10 moles of a diatomic gas
starting at 300K. For this gas,
the molecules vibrate
above 500K. A total of 20,000J of heat is put into the
gas during this process.
a) Clearly show that the final temperature of the gas is TF =
599K.
b) How many joules of the (20,000J of) heat went into increasing
the kinetic energy of translation?
c) How many joules of the heat went into increasing the energies
associated...

Ivan heats at constant pressure 2.10 moles of a diatomic gas
starting at 300K. For this gas, the molecules vibrate above 500K. A
total of 20,000J of heat is put into the gas during this process.
a) Clearly show that the final temperature of the gas is TF = 599K.
b) How many joules of the (20,000J of) heat went into increasing
the kinetic energy of translation? c) How many joules of the heat
went into increasing the energies associated...

The heat capacity at constant volume of an ideal gas depends on:
Select one: a. The number of molecules b. Temperature c. None of
the options shown d. The volume e. The pressure

A three-step cycle is undergone by 3.8 mol of an ideal diatomic
gas: (1) the temperature of the gas is increased from 230 K to 710
K at constant volume; (2) the gas is then isothermally expanded to
its original pressure; (3) the gas is then contracted at constant
pressure back to its original volume. Throughout the cycle, the
molecules rotate but do not oscillate. What is the efficiency of
the cycle?

a machinr carries 2 moles of an ideal diatomic gas
thay is initially at a volume of 0.020 m^3 and a temperature of 37
C is heated to a constant volumes at the temperature of 277 C is
allowed to expand isothermally at the initial pressure, and finally
it is compressed isobarically to its original volume, pressure and
temperature.
1. determine the amount of heat entering the system during the
cycle.
2. calculate the net work affected by the gas...

21.3 moles of a diatomic ideal gas undergo three steps:
A to B is an isobaric (constant pressure P1
= 4.15x106 Pascal) expansion from volume
V1 = 0.0609 m3 to
V2 = 0.934 m3.
B to C is isochoric (constant volume)
C to A is isothermal (constant T).
During the isobaric expansion from A to B: find Q, the heat
transferred, in Joules. Give your answer in scientific
notation.
NOTE: A positive sign means heat has
been added; a negative...

A 1.79 mol diatomic gas initially at 274 K undergoes this cycle:
It is (1) heated at constant volume to 707 K, (2) then allowed to
expand isothermally to its initial pressure, (3) then compressed at
constant pressure to its initial state. Assuming the gas molecules
neither rotate nor oscillate, find (a) the net energy transferred
as heat to the gas (excluding energy transferred as heat out of the
gas), (b) the net work done by the gas, and (c)...

A 3.44 mol diatomic gas initially at 346 K undergoes this cycle:
It is (1) heated at constant volume to 909 K, (2) then allowed to
expand isothermally to its initial pressure, (3) then compressed at
constant pressure to its initial state. Assuming the gas molecules
neither rotate nor oscillate, find (a) the net energy transferred
as heat to the gas (excluding energy transferred as heat out of the
gas), (b) the net work done by the gas, and (c)...

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