Question

Three moles of a monatomic ideal gas are heated at a constant volume of 2.90 m3. The amount of heat added is 5.10 103 J.

(a) What is the change in the temperature of the gas?

_____K

(b) Find the change in its internal energy.

_____J

(c) Determine the change in pressure.

_____Pa

Answer #1

8. Three moles of a monatomic ideal gas are
heated at a constant volume of 2.10 m³. The amount of heat added is
5.3 x 10^3J. Determine the change in pressure.

17) Three moles of an ideal monatomic gas expand at a constant
pressure of 2.70 atm ; the volume of the gas changes from 3.10×10−2
m3 to 4.60×10−2 m3 .
Part A
Calculate the initial temperature of the gas.
Part B
Calculate the final temperature of the gas.
Part C
Calculate the amount of work the gas does in expanding.
Part D
Calculate the amount of heat added to the gas.
Part E
Calculate the change in internal energy of...

Three moles of an ideal monatomic gas expand at a constant
pressure of 2.90atm : the volume of the gas changes from
3.30*10^-2m^3 to 4.50*10^-2m^3.
Part A, Calculate the initial temperature of the gas.
Part B, Calculate the final temperature of the gas.
Part C, Calculate the amount of work the gas does in
expanding.
Part D, Calculate the amount of heat added to the gas.
Part E, Calculate the change in internal energy of the gas.

An ideal monatomic gas is contained in a vessel of constant
volume 0.330 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 24.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. Your response differs
from the...

An ideal monatomic gas is contained in a vessel of constant
volume 0.400 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 18.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. 80.99 Correct: Your
answer is...

An ideal monatomic gas expands isothermally from 0.600 m3 to
1.25 m3 at a constant temperature of 730 K. If the initial pressure
is 1.02 ? 105 Pa find the following.
(a) the work done on the gas
J
(b) the thermal energy transfer Q
J
(c) the change in the internal energy
J

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...

3. An ideal monatomic gas expands isothermally from .500 m3 to
1.25 m3 at a constant temperature of 675 K. If the initial pressure
is 1.00 ∙ 105 Pa, find (a) the work done by the gas, (b) the
thermal energy transfer Q, and (c) the change in the internal
energy.

The heat capacity at constant volume of a certain amount of a
monatomic gas is 53.7 J/K.
(a) Find the number of moles of the gas. in mol
(b) What is the internal energy of the gas at T = 286
K? in kJ
(c) What is the heat capacity of the gas at constant pressure?
in J/k

In this problem, 0.90 mole of a monatomic ideal gas is initially
at 285 K and 1 atm.
(a) What is its initial internal energy?
_____ kJ
(b) Find its final internal energy and the work done by the gas
when 420 J of heat are added at constant pressure.
final internal energy ________kJ
work done by the gas _______kJ
(c) Find the same quantities when 420 J of heat are added at
constant volume.
finale internal energy ________kJ
work...

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