Question

A piston having 0.033 mol of gas at 35.0 C expands from 0.77 L
to 2.00 L. Calculate the work performed if the expansion occurs
**(a)** against an external pressure of 0.455 atm, and
**(b)** reversibly

Answer #1

**a) We know**

**work done for a system against an external
pressure**

** dW = - Pext dV**

**Here,**

**
Pext = 0.455 atm and dV = (Final Volume)V2 - (Initial Volume)V1 = 2
- 0.77 = 1.23 L**

**So, dW = - 0.455 x 1.23 = 0.56 atm L = 0.56 x 0.101 kJ =
0.057 kJ**

**b) For a reversible process Pext = Pint = P = nRT
/V**

**So, work done dW = -Integration of PdV = - nRT ln
V2/V1**

**Here, n = no of mole = 0.033 mol**

**R = 0.0821 Latm K-1 mol-1**

**T = 35 ^{o}C = 273 + 35 = 308 K**

**V2 = Final volume = 2 L**

**V1 = Initial volume = 0.77 L**

**dW = - 0.033 x 0.0821 x 308 ln 2 / 0.77**

** = 0.834 x 0.954 =
0.796 atm L = 0.796 x 0.101 kJ = 0.080 kJ**

A cylinder with a moving piston expands from an initial volume
of 0.250 L against an external pressure of 1.00 atm . The expansion
does 277 J of work on the surroundings. What is the final volume of
the cylinder?

A system expands from a volume of 1.00 L to 2.00 L against a
constant external pressure of 1.00 atm. What is the work (w) done
by the system? (1 L·atm = 101.3 J)

A 2.00-mol sample of a diatomic ideal gas expands slowly and
adiabatically from a pressure of 5.04 atm and a volume of 13.0 L to
a final volume of 31.0 L.
(a) What is the final pressure of the gas?
atm
(b) What are the initial and final temperatures?
initial
K
final
K
(c) Find Q for the gas during this process.
kJ
(d) Find ΔEint for the gas during this
process.
kJ
(e) Find W for the gas during...

Consider an ideal gas enclosed in a 1.00 L container at an
internal pressure of 10.0 atm.
Calculate the work, w, if the gas expands against a constant
external pressure of 1.00 atm to a final volume of 20.0 L.
w=____J
Now calculate the work done if this process is carried out in
two steps.
1. First, let the gas expand against a constant external
pressure of 5.00 atm to a volume of 4.00 L
2. From there, let the...

A 19.0-L volume of an ideal gas in a cylinder with a piston is
at a pressure of 2.8 atm. Enough weight is suddenly removed from
the piston to lower the external pressure to 1.4 atm. The gas then
expands at constant temperature until its pressure is 1.4 atm.
Find the change in enthalpy, ?H, for this change in
state.
Express your answer using two significant figures.
Find the heat, q, associated with this change in
state.
Express your answer...

The gas inside a cylinder expands against a constant external
pressure of 0.943 atm from a volume of
3.35 L to a volume of 14.40 L. In
doing so, it turns a paddle immersed in 0.951 L of
liquid octane (C8H18).
Calculate the temperature rise of the liquid, assuming no loss of
heat to the surroundings or frictional losses in the mechanism.
Take the density of liquid
C8H18 to be
0.703 g cm-3 and its specific heat to
be 2.22...

The air within a piston equipped with a cylinder absorbs 545 J
of heat and expands from an initial volume of 0.107 L to a final
volume of 0.853 L against an external pressure of 1.00 atm. What is
the change in internal energy of the air within the piston?

14.3 10.0 L of an ideal diatomic gas at 2.00 atm and 275K are
contained in a cylinder with a piston. The gas first expands
isobarically to 20.0 L (step 1). It then cools at constant volume
back to 275 K (step 2), and finally contracts isothermally back to
10.0 L (step 3). a) Show the series of processes on a pV diagram.
b) Calculate the temperature, pressure, and volume of the system at
the end of each step in...

14.3 10.0 L of an ideal diatomic gas at 2.00 atm and 275K are
contained in a cylinder with a piston. The gas first expands
isobarically to 20.0 L (step 1). It then cools at constant volume
back to 275 K (step 2), and finally contracts isothermally back to
10.0 L (step 3).
a) Show the series of processes on a PV diagram.
b) Calculate the temperature, pressure, and volume of the system
at the end of each step in...

10.0 L of an ideal diatomic gas at 2.00 atm and 275 K are
contained in a cylinder with a piston. The gas first expands
isobarically to 20.0 L (step 1). It then cools at constant volume
back to 275 K (step 2), and finally contracts isothermally back to
10.0 L (step 3).
a) Show the series of processes on a pV diagram.
b) Calculate the temperature, pressure, and volume of the system
at the end of each step in...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 4 minutes ago

asked 14 minutes ago

asked 14 minutes ago

asked 17 minutes ago

asked 30 minutes ago

asked 33 minutes ago

asked 35 minutes ago

asked 44 minutes ago

asked 48 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago