Advertisements
Advertisements
Question
Answer the following question.
One mole of an ideal gas is compressed from 500 cm3 against a constant pressure of 1.2 × 105 Pa. The work involved in the process is 36.0 J. Calculate the final volume.
Advertisements
Solution
Given:
Initial volume (V1) = 500 cm3
External pressure (Pext) = 1.2 × 105 Pa
Work (W) = 36.0 J
To find: Final volume (V2)
Formula: W = - Pext Δ V = - Pext (V2 - V1)
Calculation: Initial volume (V1) = 500 cm3 = 0.5 dm3
External pressure (Pext) = 1.2 × 105 Pa = 1.2 bar
Work (W) = 36.0 J = 36.0 J × `(1 "dm"^3 "bar")/(100 "J")` = 0.360 dm3 bar
Now, from formula,
W = - Pext Δ V = - Pext (V2 - V1)
∴ 0.360 dm3 bar = - 1.2 bar × (V2 - 0.5 dm3)
∴ `(0.360 "dm"^3 "bar")/(1.2 "bar")` = - (V2 - 0.5 dm3)
∴ 0.3 dm3 = - V2 + 0.5 dm3
∴ V2 = 0.2 dm3 = 200 cm3
The final volume (V2) = 200 cm3.
APPEARS IN
RELATED QUESTIONS
Answer the following in one or two sentences.
Comment on the statement:
no work is involved in an expansion of gas in a vacuum.
Answer the following question.
Calculate the work done during the synthesis of NH3 in which volume changes from 8.0 dm3 to 4.0 dm3 at a constant external pressure of 43 bar. In what direction the work-energy flows?
The value of 1dm3 bar is ______.
The work done in the dm3 bar when 200 mL of ethylene gas and 150 mL of HCl gas were allowed to react at 1 bar pressure is ______.
Derive an expression for pressure-volume work.
Three moles of an ideal gas are expanded isothermally from 15 dm3 to 20 dm3 at a constant external pressure of 1.2 bar. Calculate the amount of work in Joules.
Work done when 2 mole of an ideal gas is compressed from a volume of 5m3 to 2.5m3 at 300 K, under a pressure of 100 kpa is ______.
If, 2 moles of an ideal gas at 546 K has volume of 44.8 L, then what will be it's pressure?
Three moles of an ideal gas are expanded isothermally from a volume of 300 cm3 to 2.5 L at 300 K against a pressure of 1.9 atm. The work done in joules is ____________.
10 bar dm3 is approximately equal to ____________.
3 moles of an ideal gas is compressed from 50 dm3 to 30 dm3 against a constant external pressure of 3.039 × 105 N m−2. The work done in calories is ____________.
(1 J = 0.239 cal)
When 2 moles of an ideal gas are expanded isothermally from a volume of 12.5 L to 15.0 L against constant external pressure of 7 60 mm Hg. Calculate the amount of work done in joule?
If 200 mL of ethylene gas and 200 mL of HCl gas are allowed to react at 2 atmosphere pressure as per given reaction,
\[\ce{C2H_{4(g)} + HCl_{(g)} -> C2H5Cl_{(g)}}\]
Calculate pressure volume work in Joule.
Calculate the work done during compression of 2 mol of an ideal gas from a volume of 1m3 to 10 dm3 300K against a pressure of 100 KP a.
Two moles of an ideal gas are allowed to expand from a volume of 10 dm3 to 2 m3 at 300 K against a pressure of 101.325 KPa. Calculate the work done.
Calculate the work done during the expansion of 2 moles of an ideal gas from 10 dm3 to 20 dm3 at 298 K in a vacuum.
Write the sign convention of work done during expansion of gas.
Calculate the constant external pressure required to expand 2 moles of an ideal gas from volume 15 dm³ to 20 dm³ if amount of work done is -600 J.
[Note: The question has been modified to get the correct answer.]
