SCERT Maharashtra solutions for Chemistry [English] 12 Standard HSC chapter 4 - Chemical Thermodynamics [Latest edition]

An intensive property amongst the following is ______.

The value of 1dm³ bar is ______.

The work done in the dm3 bar when 200 mL of ethylene gas and 150 mL of HCl gas were allowed to react at 1 bar pressure is ______.

The work done in vacuum when 300 m mole of an ideal gas expands until its volume is increased by 2.3 dm³ at 1 bar pressure is ______ mole.

For an Isothermal process

For an Isochoric process

The change in internal energy in a reaction when 2kJ of heat is released by the system and 6 kJ of work is done on the system will be ______.

Write the expression to calculate maximum work done when 1 mole of an ideal gas expands isothermally and reversibly from V₁ to V₂.

Write the mathematical relation between ΔH and ΔU during the formation of one mole of CO₂ under standard conditions.

The standard enthalpy of formation of water is - 286 kJ mol^-1. Calculate the enthalpy change for the formation of 0.018 kg of water.

Write the mathematical expression of the First Law of Thermodynamics for  Isothermal Process

What is the sign convention when work is done on the system by the surrounding?

Write the expression showing the relation between enthalpy change and internal energy change for gaseous phase reaction.

Calculate enthalpy of formation of HCl if bond enthalpies of H₂, Cl₂ and HCl are 434 kJ mol^-1, 242 kJ mol^–1 and 431 kJ mol^–1 respectively.

Define the Standard enthalpy of combustion.

Define the Enthalpy of sublimation.

State and explain Hess’s law of constant heat summation.

Write the features of reversible processes.

Derive an expression for pressure-volume work.

The enthalpy change of the following reaction:

\[\ce{CH_{4(g)} + Cl_{2(g)} -> CH3Cl_{(g)} + HCl_{(g)}ΔH^0 = –104 kJ}\]

Calculate C – Cl bond enthalpy. The bond enthalpies are:

Calculate the standard enthalpy of combustion of CH_4(g) if Δ_fH°(CH₄) = – 74.8 kJ mol^–1, Δ_fH°(CO₂) = – 393.5 kJ mol^–1 and Δ_fH°(H₂O) = – 285.8 kJ mol^–1.

Define an isolated system.

Three moles of an ideal gas are expanded isothermally from 15 dm³ to 20 dm³ at a constant external pressure of 1.2 bar, calculate the amount of work in Joules.

Answer the following in one or two sentences.

What is enthalpy of fusion?

Answer the following question.

Derive the expression for the maximum work.

Derive the expression for work done in chemical reaction. Write the relationship between ∆H and ∆U for an isochoric process.

Define standard enthalpy of formation.

0.022 kg of CO₂ is compressed isothermally and reversibly at 298 K from an initial pressure of 100 kPa when the work obtained is 1200 J, calculate the final pressure.

Define the Enthalpy of vaporization.

Define the Standard enthalpy of combustion.

Why work done in vacuum is zero?

Define the Enthalpy of atomization.

Define the Extensive properties.

Calculate the standard enthalpy of formation of liquid methanol from the following data:

1. \[\ce{CH3OH_{(l)} + \frac{3}{2} O_{2(g)} -> CO_{2(g)} + 2H2O_{(l)}}\]     ∆H° = – 726 kJ mol^–1
2. \[\ce{C_{(Graphite)} + O_{2(g)} -> CO_{2(g)}}\]          ∆_cH° = – 393 kJ mol^–1
3. \[\ce{H_{2(g)} + \frac{1}{2} O_{2(g)} -> H2O_{(l)}}\]          ∆_fH° = – 286 kJ mol^–1 

Define the Bond enthalpy.

Define the Enthalpy of ionisation.

Calculate the standard enthalpy of the reaction.

\[\ce{2Fe_{(s)} + \frac{3}{2} O_{2(g)} -> Fe2O_{3(s)}}\]

Given:

Answer in brief.

How much heat is evolved when 12 g of CO reacts with NO₂? The reaction is:

4CO_(g)  2NO_2(g) → 4CO_2(g) + N_2(g), Δ_rH° = - 1200 kJ

Write an application of Hess’s law.

Does the following reaction represent a thermochemical equation?

\[\ce{CH_{4(g)} + 2O_{2(g)} -> CO_{2(g)} + 2H2O_{(g)}}\], ∆_fH° = –900 kJ mol^–1

Classify the following into intensive and extensive properties.

Pressure, volume, mass, temperature.

Define state function and write two examples of it.