Nature of heat and work

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?

Define path function.

The conditions for a system to be able to completely obtain all the work possible is

Which process has maximum work done?

$1$ calorie $=$ _____ joule.(write answer up to $2$ decimal)

If the work is done by the system,${\mathrm{w}}_{\mathrm{ad}}$ will be negative because _____ .

According to IUPAC conventions work done on the surroundings is :

Which of the following statements are correct as per IUPAC sign convention ?

For next two question please follow the same

The pressure-volume graphs of various thermodynamics processes are shown:



Work is the mode of transference of energy. It has been observed that reversible work done by the system is maximum obtainable work.

w_rev > w_irr

The works of isothermal and adiabatic processes are different from each other.

$-{\text{w}}_{\text{isothermal reversible}}={\text{2.303 nRT log}}_{10}\left(\frac{{\text{V}}_2}{{\text{V}}_1}\right)$

$={\text{2.303 nRT log}}_{10}\left(\frac{{\text{P}}_1}{{\text{P}}_2}\right)$

$-{\text{w}}_{\text{adiabatic reversible}}={\text{C}}_{\text{V}}\left({\text{T}}_1-{\text{T}}_2\right)$

If w₁, w₂, w₃ and w₄ are magnitude of work done in isothermal, adiabatic, isobaric and isochoric reversible processes, respectively, then the correct sequence (for expansion) would be

The work done during the expansion of a gas from $4\mathrm{ }\mathrm{d}{\mathrm{m}}^3$ to $6\mathrm{ }\mathrm{d}{\mathrm{m}}^3$ against a constant external pressure of $3\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{m}$ is $(1\mathrm{ }\mathrm{L}\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{m}=101.32\mathrm{ }\mathrm{J})$

Calculate the work done in each of the following reactions. State whether work is done on or by the system.

Decomposition of $2 \mathrm{moles}$of${\mathrm{NH}}_4{\mathrm{NO}}_3$ at $100°\mathrm{C}$

${\mathrm{NH}}_4{\mathrm{NO}}_3 \left(\mathrm{s}\right) \to {\mathrm{N}}_2\mathrm{O} \left(\mathrm{g}\right) + 2{\mathrm{H}}_3\mathrm{O} \left(\mathrm{g}\right)$

Calculate the work done in each of the following reactions. State whether work is done on or by the system.

The oxidation of one mole of ${\mathrm{SO}}_2$ at $50°\mathrm{C}$.

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right) + {\mathrm{O}}_2 \left(\mathrm{g}\right) \to 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$

$2.8 \mathrm{x} {10}^{-2} \mathrm{Kg}$ of nitrogen is expanded isothermally and reversibly at $300\mathrm{K}$ from $15.15 \mathrm{x} {10}^5 {\mathrm{Nm}}^{-2}$ when the work done is found to be$-17.33 \mathrm{kJ}$. Find the final pressure.

Three moles of an ideal gas are compressed isothermally and reversibly to a volume of $2 \mathrm{L}$. The work done is $2.983 \mathrm{kJ}$ at $22°\mathrm{C}$. Calculate the initial volume of the gas.

Calculate the maximum work when$24 \mathrm{g}$ of oxygen are expanded isothermally and reversibly from a pressure of $1.6\times {10}^5 \mathrm{Pa}$ to $100 \mathrm{kPa}$ at$298 \mathrm{K}$.

One mole of an ideal gas is compressed from $500 {\mathrm{cm}}^3$ against a constant pressure of $1.216\times {10}^5 \mathrm{Pa}$. The work involved in the process is$36.50 \mathrm{J}$. Calculate the final volume.

Three moles of an ideal gas are expanded isothermally from a volume of$300 {\mathrm{cm}}^3$ to $2.5 \mathrm{L}$ at$300 \mathrm{K}$ against a pressure of $1.9 \mathrm{atm}$. Calculate the work done in $\mathrm{L} \mathrm{atm}$ and joules.

In what reaction of the following, work is done by the system on the surroundings?