Applications of Thermodynamics: Work

$16 \mathrm{g} \mathrm{of} {\mathrm{O}}_2$ at ${37}^{\mathrm{o}}\mathrm{C}$ is allowed to expand from $2\mathrm{L} \mathrm{to} 4\mathrm{L}$under reversible isothermal conditions. Assuming ideal behaviour, calculate the work done during this process. 

In a container $3.2 \mathrm{g}$ of oxygen gas is kept at $20 \mathrm{atm}$ and $300\mathrm{K}$. The gas is allowed to expand isothermally against constant external pressure of $1 \mathrm{atm}$ till the final pressure reaches to $1 \mathrm{atm}$. Calculate the magnitude of work done by the gas.(The nearest integer)

$82 \mathrm{L}$ of carbon dioxide are produced at a pressure of $1 \mathrm{atm}$ and $25°\mathrm{C}$ by the action of acid on metal carbonate. The work done by gas (in calories) in pushing back the atmosphere is ($\mathrm{R}=0.082 \mathrm{litre}-\mathrm{atm} {\mathrm{deg}}^{-1}{\mathrm{mol}}^{-1}$)

$0.1$ moles of a diatomic gas at $27°\mathrm{C}$ is heated at constant pressure, so that the volume is doubled. If $\mathrm{R}=2 \mathrm{cal}/\mathrm{mol}$, the work done by gas in $\mathrm{cal}$ will be

One mole of an ideal gas (not necessarily monoatomic) is subjected to the following sequence of steps.
(a) It is heated at constant volume from $298 \mathrm{K} \text{to} 373 \mathrm{K}$
(b) It is expanded freely into a vacuum to double volume.
(c) It is cooled reversibly at constant pressure to $298 \mathrm{K}$.
Calculate $\mathrm{q}, \mathrm{w}, ∆\mathrm{U}$ and $∆\mathrm{H}$ for the overall process.​

$0.5 \mathrm{mol}$ of diatomic gas at $27°\mathrm{C}$ is heated at constant pressure so that its volume is tripled. If $\mathrm{R}=8.3{\mathrm{Jmole}}^{-1}{{\mathrm{k}}^{-}}^1$ then work done is 

One mole of ${\mathrm{O}}_2$​ gas having a volume equal to $22.4 \mathrm{L}$ at $0°\mathrm{C}$ and $1\mathrm{atm}$ pressure is compressed isothermally so that its volume reduces to $11.2 \mathrm{L}$. The work done in this process is then

The work done when $2$ moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{L}$ to $10 \mathrm{L}$ at $300 \mathrm{K}$ is $\left(\mathrm{R}=0.0083 \mathrm{kJ} \mathrm{K} {\mathrm{mol}}^{-1}\right)$

For the free expansion of an ideal gas under adiabatic conditions, the correct option is

$3$ moles of an ideal gas expands isothermally against a constant pressure of $2$ Pascal from $20 \mathrm{L}\text{ to} 60$ L.The amount of work involved is

Two moles of $\mathrm{He}$ gas $(\gamma =5/3)$ are initially at temp $27°\mathrm{C}$ and occupy a volume of $20$ litres. The gas is first expanded at constant pressure until its volume is doubled. Then it undergoes reversible adiabatic change, until the volume become $110 \mathrm{lit}$, then predict the value of $\mathrm{T}/100$ (where $\mathrm{T}$ is the final temperature, ${\left(\frac{4}{11}\right)}^{2/3}=\frac{1}{2}$)

An ideal gas undergoes adiabatic expansion against constant external pressure. Which of the following is incorrect:

Calculate $\mathrm{\Delta G}\left(\mathrm{in} \mathrm{kJ}\right)$ (in magnitude) for the process, one mole of an ideal gas at $22.4 \mathrm{litres}$ is expanded isothermally and reversibly at $300 \mathrm{K}$ to a volume of $224 \mathrm{litres}$.

Give your answer as the nearest integer.

Which of the following is the SI unit of work?

Mechanical work is a _____ quantity.

Define mechanical work and give the formula to calculate work. Is work a vector or scalar quantity?

Why work done in a free expansion of ideal gas is zero?

The change in internal energy equals

Explain free expansion of an ideal gas.