Question

A container is filled with an ideal diatomic gas to a pressure
and volume of *P*_{1} and *V*_{1},
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 as necessary.)

Q=?

Answer #1

**Solution:**

Given,

Initial values, P_{1} and V_{1}, Using ideal gas
equation

T_{1} = P_{1}V_{1}/nR .

Step 1 : Constant volume, Pressure is increased to
3P_{1}

T_{2} = 3P_{1}V_{1}/nR .

The heat energy added in this step, C_{v} = 5/2R for
diatomic

Q_{1} = nC_{v}T

= n[5/2]R*[3P_{1}V_{1} -
P_{1}V_{1}]/nR

= 5P_{1}V_{1}.

Step 2: Constant pressure, Volume increased to
2V_{1}

T_{3} = 3P_{1}(2V_{1})/nR =
6P_{1}V_{1}/nR

The heat energy added in this step C_{p} = 7/2R for
diatomic,

Q_{2} = nC_{p}T

= n[7/2]R[6P_{1}V_{1} -
3P_{1}V_{1}]/nR

= 10.5P_{1}V_{1}.

the total Heat added is,

Q_{net} = Q_{1} + Q_{2}

**= 15.5P _{1}V_{1}.**

I hope you understood the problem and got your answers, If yes rate me!! or else comment for a better solutions.

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...

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 monatomic gas is taken through two steps; first its pressure
is increased from P1 to
2.80P1 at constant volume. Then its volume is
increased from V1 to 1.50V1
at constant pressure.
(a) How much heat is transferred to the gas during this entire
process if V1 = 6.92 ✕ 10−3
m3 and P1 = 1.21 atm?
J
(b) How much heat would be transferred during the entire process,
if the gas was a diatomic one?

In the initial state, an ideal gas has pressure p1, volume V1
and temperature T1. Now the gas changes its state by effecting a
state change so that it reaches the pressure p2, the volume V2 and
the temperature T2 in the new state. The pressure doubles during
this state change, which is an isochore process.
a) Find the work W performed during the isochore process.
b) The heat Q is exchanged between the gas and the surroundings
during the...

A two mole sample of an ideal diatomic gas expands
slowly and adiabatically from a pressure of 5 atm. and a volume of
10 liters up to a final volume of 30 liters.
a) What is the final pressure of the gas ?,
b) Whatis the heat, work and internal energy?

Physics_2_2.5
An ideal monatomic gas is in a vessel with the volume V1 = 1m3
under the pressure p1 = 2 105 Pa. The gas is first heated at a
constant pressure to the Volume V2 = 3m3 and then at constant
volume to the pressure p2 = 5 105 Pa. Find the amount of heat Q
supplied to the gas.
A clear process is highly appreciated! Thank you so much for the
help!

9. A 2mole sample of diatomic gas is placed in a sealed
container. The initial volume of the container is 2m3 but then the
lid is pushed down, causing 2500J of mechanical work to be done on
the gas to compress it isobarically to 1.5m3. a) What is the
pressure of the gas? (2pts) b) What is the thermal energy lost
through heat by the gas? (4pts)

A rigid adiabatic container is divided into two parts containing
n1 and n2 mole of ideal gases respectively, by a movable and
thermally conducting wall. Their pressure and volume are P1, V1 for
part 1 and P2, V2 for part 2 respectively. Find the final pressure
P and temperature T after the two gas reaches equilibrium. Assume
the constant volume specific heats of the two gas are the same.

See diagram 4.
58 moles of a diatomic ideal gas undergo three steps:
A to B is an isobaric (constant pressure P1 = 5.71x10^6 Pascal)
expansion from volume V1 = 0.025 m3 to V2 = 0.661 m3.
B to C is isochoric (constant volume)
C to A is isothermal (constant T).
Find PC, the pressure at point C, in Pascals. Express in
scientific notation.

a
diatomic gas is in a container with a fixed volume of 0.275 m^3.
Assume the diatomic gas has five degrees of freedom.
Part A: what is the temperature of the gas if there are 5.00
mol present and the gas is under a pressure of 1.60 atm?
_____ K
Part B: if the gas is to be heated by 230K how much heat is
necessary to accomplish this task?
_______J
Part C: Repeat parts (a) and (b) for a...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 19 minutes ago

asked 19 minutes ago

asked 26 minutes ago

asked 27 minutes ago

asked 34 minutes ago

asked 44 minutes ago

asked 52 minutes ago

asked 53 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago