Calculate the standard heat of formation of propane, if its heat of combustion is -2220.2 kJ mol^-1. the heats of formation of CO_2(g) and H₂O(l) are -393.5 and -285.8 kJ mol^-1 respectively

If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

The heat of combustion of solid naphthalene (C₁₀H₁₀) at constant volume was -4984 kJ mol^-1 at 298 K. Calculate the value of enthalpy change.
Given: 
C₁₀H_8(s)+12O_2(g) ➝ 10CO_2(g)+4H₂O(l)
\(\Delta U\)=-4984 kJ mol^-1
\(\Delta U\)=-4984 kJ mol^-1,R=8.314 JK^-1 mol^-1
T=298 K

The standard heat of formation of H₂O_(l) from its elements and O₂ is -290.83 kJ mol^-1 and the standard entropy change for the same reaction is -330 JK-I at 25°C. Will the reaction be spontaneous at 25°C.
Given: \(\Delta{H^{o}}\)= -290.83 kJ mol^-1
= -290830 J mol^-1
\(\Delta{S^{o}}\) = -330 JK^-1
T = 25°C = 298 K

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K The molar heat of vaporisation of ethanol is 39.84 kJ mol^-1.

Distinguish between reversible and irreversible process

Write a short note on the following terms.
(i) Open System
(ii) Closed System
(iii) Isolated System
(iv) Homogeneous System
(v) Heterogeneous System

Discuss in detail about the variation of internal energy with respect to various thermodynamic processes

Explain the measurement of heat change at constant pressure with a neat diagram.

The enthalpy of combustion for H₂, C_(graphite) and CH₄ are -285.8, -393.5 and -890.4 kJ mol^-1respectively. Calculate the standard enthalpy of formation \(\Delta { H }_{ f }^{ 0 }\) for CH₄

Compute the standard free energy of the reaction at 27⁰C for the combustion of methane using the given data: CH₄(g) + 2O₂(g) ⟶ CO₂(g) + 2H₂O(l)

Calculate ΔG⁰ for the reaction. CO(g)+ \(\\ \frac { 1 }{ 2 } \)O₂(g) ⟶ CO₂(g), ΔH⁰ = - 282.84 kJ Given, S⁰(C0₂) =213.8Jk^-1 mol^-1, S^o (CO) = 197.9 Jk^-1 mol^-1 S⁰(O₂) = 205.0 Jk^-1 mol^-1

List the characteristics of entropy:

Explain about the characteristics of work.

Write the various definition of first law of thermodynamics.

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) ⇌ [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value of equilibrium constant.

The equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) ⇌ 2NO₂(g);
\(\Delta \mathrm{H}_{\mathrm{f}}^{\circ}=57.32 \mathrm{KJmol}^{-1}\)
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100^o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

At particular temperature K_C = 4 x 10^–2 for the reaction
H₂S(g) ⇌ H₂(g) + ½ S₂(g)
Calculate KC for each of the following reaction
i) 2H₂S (g) ⇌ 2H₂ (g) + S₂ (g)
ii) 3H₂S (g) ⇌ 3H₂ (g) + 3/2 S₂(g)

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

A sealed container was filled with 1 mol of A₂ (g), 1 mol B₂ (g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 1 for the reaction
A₂ (g) + B₂ (g) ⇌ 2AB (g)