Question

Suppose 660 J of heat flows into a diatomic ideal gas that is held at constant volume.

1. How many joules of this energy goes into the translational kinetic energy of the gas?

2. How many joules of the heat energy goes into the rotational kinetic energy of the gas?

Answer #1

for diatomic ideal gas

number of freedoms = 5

number of degree of freedom of translational kinetic energy = 3

number of degree of freedom of rotational kinetic energy = 2

1.

translational kinetic energy of the gas = 660 * 3/(2 + 3)

translational kinetic energy of the gas = 396 J

**the translational kinetic energy of the gas is 396
J**

2. rotational kinetic energy of the gas = 660 - 396

rotational kinetic energy of the gas = 264 J

**the rotational kinetic energy of the gas is 264
J**

Neon gas (a monatomic gas) and hydrogen gas (a diatomic gas) are
both held at constant volume in separate containers. Each container
contains the same number of moles n of each gas. You find
that it takes an input of 300 J of heat to increase the temperature
of the hydrogen by 2.50°C.
Part A
How many modes does a single hydrogen gas molecule have? (Assume
the vibrational modes are "frozen out").
3, all rotational kinetic
6, 3 translational kinetic...

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 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?

1. Under constant-volume conditions, 4200 J of heat is added to
1.4 moles of an ideal gas. As a result, the temperature of the gas
increases by 103 K. How much heat would be required to cause the
same temperature change under constant-pressure conditions? Do not
assume anything about whether the gas is monatomic, diatomic,
etc.
2. A system gains 3080 J of heat at a constant pressure of 1.36
× 105 Pa, and its internal energy increases by 4160...

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.

When 18.5 J was added as heat to a particular ideal gas, the
volume of the gas changed from 36.8 cm3 to 59.4
cm3 while the pressure remained constant at 0.944 atm.
(a) By how much did the internal energy of the gas
change? If the quantity of gas present is 1.38 x 10-3
mol, find the molar specific heat of the gas at
(b) constant pressure and (c)
constant volume.

A container is filled with an ideal diatomic gas to a pressure
and volume of P1 and V1,
respectively. The gas is then warmed in a two-step process that
increases the pressure by a factor of five and the volume by a
factor of three. Determine the amount of energy transferred to the
gas by heat if the first step is carried out at constant volume and
the second step at constant pressure. (Use any variable or symbol
stated above...

A container is filled with an ideal diatomic gas to a pressure
and volume of P1 and V1,
respectively. The gas is then warmed in a two-step process that
increases the pressure by a factor of three and the volume by a
factor of two. Determine the amount of energy transferred to the
gas by heat if the first step is carried out at constant volume and
the second step at constant pressure. (Use any variable or symbol
stated above...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 33 minutes ago

asked 50 minutes ago

asked 59 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago