Choose the correct answer. A thermodynamic state function is a quantity _______.

A reaction, A + B → C + D + q is found to have a positive entropy change. The reaction will be _______.

As per the available data: ______.

In the equation, \({ N }_{ 2 }(g)+3{ H }_{ 2 }(g)\rightleftharpoons 2N{ H }_{ 3 }(g)\) what would be the sign of work done?

At 1 atm will the \({ \triangle }_{ f }{ H }^{ \circ }\) be zero for Cl₂(g) and Br₂ (g)? Explain.

The fact that enthalpy is a state function forms the basis of a very useful law. Name the law.

Which one of the following is not extensive state function?

Carbon monoxide is allowed to expand isothermally and reversibly from 10\({ m }^{ 3 }\) to 20\({ m }^{ 3 }\) at 300K and work obtained is 4.754kJ. Calculate the number of moles of carbon monoxide.

Standard molar enthalpy of formation, \({ \Delta }_{ f }{ H }^{ o }\) is just a special case of enthalpy of reaction, \({ \Delta }_{ r }{ H }^{ o }\). Is the \({ \Delta }_{ f }{ H }^{ o }\) for the following reaction same as \({ \Delta }_{ f }{ H }^{ o }\) ? Give reason for your answer.
CaO(s) + CO₂(g)\(\longrightarrow \)CaCO₃(s);
\({ \Delta }_{ f }{ H }^{ o }=-178.3 \ kJ \ { mol }^{ -1 }\)

The enthalpy of vaporization of liquid diethyl ether (C₂H₅)_2O is 26.0 KJ mol^-1 at its boiling point (35.0^oC). Calculate △S^o for the conversion of Vapour to liquid at 35^o C.

For the reaction
2A(g)+B(g)→2D(g)Δ U^θ=−10.5 kJ and Δ S^θ=–44.1 JK⁻¹.
Calculate Δ Gθ for the reaction, and predict whether the reaction may occur spontaneously.

If the same gas expands isothermally in a reversible manner, then what will be the value of work done?

The reaction of cyanamide, NH₂CN (s), with dioxygen was carried out in a bomb calorimeter, and ∆U was found to be –742.7 kJ mol^–1 at 298 K. Calculate enthalpy change for the reaction at 298 K.
\({ NH }_{ 2 }CN(s)+\frac { 3 }{ 2 } { O }_{ 2 }(g)\rightarrow { N }_{ 2 }(g)+{ CO }_{ 2 }(g)+{ H }_{ 2 }O(l)\)

When 20.0 g of ammonium nitrate (NH₄NO₃) is dissolved in 125 g of water in a coffee cup calorimeter. (Treat heat capacity of water as the heat capacity of the calorimeter and its contents).