Question

13)One mole of neon gas is heated from 358 K to 426 K at
constant pressure. Note that neon has a molar specific heat of
*c* = 20.79 J/mol · K for a constant–pressure process.

(a) Calculate the energy *Q* transferred to the
gas.

kJ

(b) Calculate the change in the internal energy of the gas.

kJ

(c) Calculate the work done *on* the gas.

kJ

Answer #1

Given,

Molar specific heat, c = 20.79 J/mol · K

Number of moles of Neon gas (monoatomic)= 1 mole

Universal gas Constant, R = 8.314 J/mol · K

a) The energy transferred is given by,

b) For a monoatomic gas (neon gas), the change in internal energy is given by,

c) According to first law of thermodynamics.

A cylinder of volume 0.320 m3 contains 11.1 mol of
neon gas at 19.1°C. Assume neon behaves as an ideal gas.
(a) What is the pressure of the gas?
Pa
(b) Find the internal energy of the gas.
J
(c) Suppose the gas expands at constant pressure to a volume of
1.000 m3. How much work is done on the gas?
J
(d) What is the temperature of the gas at the new volume?
K
(e) Find the internal energy...

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...

Under constant pressure, the temperature of 1.70 mol of an ideal
monatomic gas is raised 15.5 K. (a) What is the work W done by the
gas? J (b) What is the energy transferred as heat Q? J (c) What is
the change ΔEint in the internal energy of the gas? J (d) What is
the change ΔK in the average kinetic energy per atom? J

One mole of an ideal gas is compressed at a constant temperature
of 55 oC from 16.5 L to 12.8 L using a constant external
pressure of 1.6 atm. Calculate w, q, ΔH and ΔS for this
process.
w = (?) kJ
q = (?) kJ
ΔH = (?) kJ
ΔS = (?) J/(mol*K)

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)...

Calculate the change in entropy (in J/K) when 38.7 g of nitrogen
gas is heated at a constant pressure of 1.50 atm from 22.9 ºC to
88.2 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp
is 29.1 J/(mol-K) .)

Calculate the change in entropy (in J/K) when 52.8 g of nitrogen
gas is heated at a constant pressure of 1.50 atm from 16.5 ºC to
62.8 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp
is 29.1 J/(mol-K) .)

One mole of NH3(g) is reversibly heated from 300 K to 1300 K at
1.00 bar pressure. Calculate q, w, ∆U, ∆H and ∆S.
Data
The molar heat capacity of NH3(g) is given by the equation
Cpm(T) = a0 + a1T + a2T^2 with constants a0 = 24.295, a1 = 0.03990,
−7.814 × 10−6 .
Cpm is in units of J K−1 mol−1 and T is in units of K.
Hints: dq = dH = CpdT and dS = dq/T...

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?

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