Heat capacity (Cp) is an extensive property but specific heat (C) is an intensive property. What will be the relation between Cp and C for 1mole of water?

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

What an ideal gas expands into vacuum, there is neither adsorption nor evolution of heat. Why?

Increase in enthalpy of the surroundings is equal to decrease in enthalpy of the system. Will the temperature of system and surroundings be the same when they are in thermal equilibrium?

Given that \(\Delta H\) = 0 for mixing of two gases. Explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not?

500 J of heat was supplied to a system at constant volume. It resulted in the increase of temperature of the system from 20^oC and 25^oC. What is the change in internal energy of the system?

A sample of 1.0 mole of a monatomic ideal gas is taken through a cyclic process of expansion and compression as shown in the figure. What will be the value of \(\Delta H\) for the cycle as a whole?

Standard vaporisation enthalpy of benzene at boiling point is 30.8 KJ mol^-1. For how long would 100W electric heater have to operate in order to vaporise a 100g sample at that temperature
(power = energy/time and 1W = 1Js^-1)?

Expansion of a gas in vacuum is called free expansion. Calculate the work done and the change in internal energy when 1L of ideal gas expands isothermally into vacuum until its total volume is 5 L?

The value of \({ \Delta }_{ f }{ H }^{ \Theta }\) for NH₃ is -91.8 kJ mol^-1. Calculate enthalpy change for the following reaction.
\(2{ NH }_{ 3 } \ (g)\longrightarrow { N }_{ 2 }(g) \ + \ { 3H }_{ 2 }(g)\)

Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions..\(\Delta _{ f }H^{ \circ }=-286kJmol^{ -1 }\)

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);
\({ \Delta }_{ f }{ H }^{ o }=-178.3 \ kJ \ { mol }^{ -1 }\)

A man takes a diet equivalent to 10000 kJ per day and does work, in expending his energy in all forms equivalent to 12500 kJ per day. What is change in internal energy per day?If the energy lost was stored as sucrose (1632 kJ pre 100g), how many days should it take to lose 2kg of his weight?(Ignore water loss)

Calculate the standard Gibbs energy change for the formation of propane at 298 K.
3 C (graphite) + 4H₂(g) → C₃H₈ (g)
\(\triangle _{ f }{ H }^{ o }for\quad propane,{ C }_{ 3 }{ H }_{ 8 }(g)=270.2J{ K }^{ -1 }{ mol }^{ -1 }\)
\({ S }_{ m }^{ o }C(graphite)=5.70J{ K }^{ -1 }{ mol }^{ -1 }\)
\( and \ { S }_{ m }^{ 0 }{ H }_{ 2 }(g)=130.7J{ K }^{ -1 }{ mol }^{ -1 }\)

An intimate mixture of Fe₂O₃ and Al is used in a solid fuel rocket. Calculate the fuel value per gram and fuel value pre cc of mixture.Heats of formation and densities are as follows.
\({ \triangle }_{ f }H\)(Al₂O₃) = 399 kcal/mol, \({ \triangle }_{ f }H\)(Fe₂O₃) = 199 kcal/mol (Density of Fe₂O₃ = 5.2g/cc. Density of Al =2.7g/cc)

Calculate the standard enthalpy of formation of CH₃OH(l) from the following data:
\( CH_{ 3 }OH(l)+\frac { 3 }{ 2 } O_{ 2 }(g)\rightarrow CO_{ 2 }(g)+2H_{ 2 }O(l);\Delta _{ r }{ H }^{ o }=-726 \ kJ \ { mol }^{ -1 }\)
\( C_{ (graphite) }+O_{ 2 }(g)\rightarrow CO_{ 2 }(g);\Delta _{ c }{ H }^{ o }=-393 \ kJ \ { mol }^{ -1 }\)
\( H_{ 2 }(g)+\frac { 1 }{ 2 } O_{ 2 }(g)\rightarrow H_{ 2 }O(l);\Delta _{ f }{ H }^{ o }=-286 \ kJ \ { mol }^{ -1 }\)

For oxidation of iron, \(4Fe(s)+{ 3O }_{ 2 }(g)\rightarrow 2{ Fe }_{ 2 }{ O }_{ 3 }(s)\) entropy change is -549.4 JK^-1mol^-1 at 298K. Inspite of negative entropy change of this reaction, why is the reaction spontaneous? (\({ \triangle }_{ r }{ H }^{ \circleddash }\)for this reaction is -1648 x 10³ Jmol^-1)

Use the following data to calculate \(\Delta _{ lattice }H^{ \circleddash } \ forNaBr.\Delta _{ sub }H^{ \circleddash }\)for sodium metal
= 108.4 KJ mol^-1 ,ionisation enthalphy of sodium
= 495 KJ mol^-1 , electron gain enthalphy  of bromine.
= -325 KJ mol^-1 , bond dissociation enthalpy of bromine
= 192 KJ mol^-1 , \(\Delta _{ sub }H^{ \circleddash }\)for NaBr(s) = -360.1KJ mol^-1
This question is based upon the concept of Born-Haber cycle as well as Hess's law. Following steps are used to solve this problem.
\(Na(s)\rightarrow Na(g);\Delta _{ sub }H^{ \circleddash }\)
\( Na(s)\rightarrow Na^{ + }(g)+e^{ - }(g);IE\)
\(\frac { 1 }{ 2 } Br_{ 2 }(g)\rightarrow Br(g);\Delta _{ diss }H^{ \circleddash }\)
\( Br(g)+e^{ - }(g)\rightarrow Br^{ - }(g);\Delta _{ eg }H^{ \circleddash }\)
\(Applying\quad Hess'law\)
\( \Delta _{ f }H^{ \circleddash }=\Delta _{ sub }H^{ \circleddash }+IE+\Delta _{ diss }H^{ \circleddash }+\Delta _{ eg }H^{ \circleddash }+U\)

Sodium carbonate, Na₂ CO₃ can be obtained by heating sodium hydrogen carbonate, NaHCO₃ as 2 NaHCO₃(s) \(\longrightarrow \) Na₂CO₃ (s) + CO₂(g).The essential data are
NaHCO₃(s)  Na₂CO₃ (s) Na₂(g) H₂O(g)

Calculate the temperature above which  NaHCO₃ decomposes to give products at 1 bar.