Respuesta :
Answer : The expansion work done against a constant external pressure is, -1063.65 J
Explanation :
First we have to calculate the moles of dry ice [tex](CO_2)[/tex].
[tex]\text{Moles of }CO_2=\frac{\text{Mass of }CO_2}{\text{Molar mass of }CO_2}[/tex]
Given:
Molar mass of [tex]CO_2[/tex] = 44 g/mole
Mass of [tex]CO_2[/tex] = 19.2 g
Now put all the given values in the above expression, we get:
[tex]\text{Moles of }CO_2=\frac{19.2g}{44g/mol}=0.436mol[/tex]
Now we have to calculate the volume of dry ice.
Using ideal gas equation:
[tex]PV=nRT[/tex]
where,
P = Pressure of [tex]CO_2[/tex] gas = 0.995 atm
V = Volume of [tex]CO_2[/tex] gas = ?
n = number of moles [tex]CO_2[/tex] = 0.436 mole
R = Gas constant = [tex]0.0821L.atm/mol.K[/tex]
T = Temperature of [tex]CO_2[/tex] gas = [tex]22^oC=273+22=295K[/tex]
Putting values in above equation, we get:
[tex]0.995atm\times V=0.436mole\times (0.0821L.atm/mol.K)\times 295K[/tex]
[tex]V=10.6L[/tex]
As initially, volume of dry ice is negligible. So,
Volume expanded = Volume of dry ice
Thus,
Expansion work = -(Pressure × Volume)
Expansion work = -0.995 atm × 10.6 L
Expansion work = -10.5 L.atm
Conversion used : (1 L.atm = 101.3 J)
Expansion work = -10.5 × 101.3 = -1063.65 J
Therefore, the expansion work done against a constant external pressure is, -1063.65 J
Answer:
The expansion work done against constant external pressure is 1073.2 J.
Explanation:
Given:
The mass of dry ice (solid [tex]\rm CO_2[/tex]) is [tex]m=19.2\rm \; g[/tex].
The constant external pressure is, [tex]P=0.995\rm \; atm[/tex]
Constant temperature is [tex]T=22^{\circ}\rm C=295 \;K[/tex].
Now, the dry ice is evaporated (expanded) and it is required to find the work done.
Carbon dioxide is behaving like an ideal gas. So, it will follow the ideal gas equation.
[tex]PV=nRT[/tex]
where n is the number of moles and R is the gas constant.
The value of gas constant is, [tex]8.314 \rm \;J K^{-1} mol^{-1}[/tex].
Now, the molar mass of carbon dioxide is 44 g. So, the number of moles will be,
[tex]n=\dfrac{\texttt{given mass}}{\texttt{molar mass}}\\n=\dfrac{19.2}{44}\\n=0.44[/tex]
Ideal gas equation at final condition will be,
[tex]P(V+\Delta V)=nRT[/tex] because pressure, temperature, and moles remain constant.
So, the net work done in the process will be [tex]P\Delta V[/tex], which can be calculated as, (initial volume V is negligible as compared to the volume of gas)
[tex]P(V+\Delta V)=nRT\\P(\Delta V)=nRT \texttt{ (initial volume is neglected)}\\W=P\Delta V=0.44\times 8.314\times 295\\W=1073.2\rm \; J[/tex]
Therefore, the expansion work done against constant external pressure is 1073.2 J.
For more details, refer the link:
https://brainly.com/question/14030557?referrer=searchResults
