The equilibrium constants of the following reactions are:

The equilibrium constant (K) for the reaction ;
\({ 2NH }_{ 3 }+5/2{ O }_{ 2 }\overset { K }{ \rightleftharpoons } 2NO+{ 3H }_{ 2 }{ O },\) will be

Consider the following reversible reaction at equilibrium, A + B ⇌ C, If the concentration of the reactants A and B are doubled, then the equilibrium constant will ___________

For the formation of Two moles of SO₃(g) from SO₂ and O₂, the equilibrium constant is K₁. The equilibrium constant for the dissociation of one mole of SO₃ into SO₂ and O₂ is __________

In a chemical equilibrium, the rate constant for the forward reaction is 2.5 \(\times\)10² and the equilibrium constant is 50. The rate constant for the reverse reaction is ____________

Consider the reaction where K_P = 0.5 at a particular temperature
PCl₅(g) ⇌ PCl₃ (g) + Cl₂ (g)
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true ____________

In the reaction,
Fe (OH)₃ (s) ⇌ Fe³⁺(aq) + 3OH^–(aq),
if the concentration of OH^– ions is decreased by ¼ times, then the equilibrium concentration of Fe³⁺ will

The values of K_P1 and K_P2 for the reactions
X ⇌ Y + Z
A ⇌ 2B are in the ratio 9 : 1 if degree of dissociation and initial concentration of X and A be equal then total pressure at equilibrium P₁ and P₂ are in the ratio __________

If x is the fraction of PCl₅ dissociated at equilibrium in the reaction
PCl₅ ⇌ PCl₃ + Cl₂
then starting with 0.5 mole of PCl₅, the total number of moles of reactants and products at equilibrium is ___________

For the reaction AB (g) ⇌ A(g) + B(g), at equilibrium, AB is 20% dissociated at a total pressure of P, The equilibrium constant K_P is related to the total pressure by the expression __________

\({K_c\over K_p}\) for the reaction,
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is ___________

In the equilibrium,
2A(g) ⇌ 2B(g) + C₂(g)
the equilibrium concentrations of A, B and C₂ at 400 K are 1\(\times\)10^–4 M, 2.0 \(\times\)10^–3 M, 1.5 \(\times\)10^–4 M respectively. The value of K_C for the equilibrium at 400 K is ________

K₁ and K₂ are the equilibrium constants for the reactions respectively.
\({ N }_{ 2 }(g)+{ O }_{ 2 }(g)\overset { { K }_{ 1 } }{ \rightleftharpoons } 2NO(g)\)
\(2NO(g)+{ O }_{ 2 }(g)\overset { { K }_{ 2 } }{ \rightleftharpoons } { 2NO }_{ 2 }(g)\)
What is the equilibrium constant for the reaction NO₂(g) ⇌ ½N₂(g) + O₂(g)

Which one of the following is incorrect statement?

The formation of ammonia from N₂(g) and H₂(g) is a reversible reaction
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat
What is the effect of increase of temperature on this equilibrium reaction ______________

If K_b and K_f for a reversible reactions are 0.8 x 10^–5 and 1.6 x 10^–4 respectively, the value of the equilibrium constant is __________

The standard substance used in the enthalpy of combustion of a substance in bomb calorimeter is _______

For the process to occur under adiabatic conditions, the correct condition is __________ 

Which of the following properties is not a function of state?

Thermodynamics is applicable to ________

Which one of the following is an intensive property??

Which one of the following is an extensive property?

Two similar reactions are given below:
H₂(g)+\(\frac { 1 }{ 2 } \)O₂(g) \(\rightarrow\)H₂O(g); \(\Delta\)H = \(\Delta\)H₁
H₂(g)+\(\frac { 1 }{ 2 } \)O₂(g)\(\rightarrow\)H₂O(l); \(\Delta\)H =  \(\Delta\)H₂
In terms of magnitude, of \(\Delta\)H

In an adiabatic process, no transfer of heat takes place between the system and surroundings. Choose the convert option for free expansion of ideal gas under adiabatic conditions from the following:

Heat liberated when 100 ml of IN NaOH is neutralized by 300 ml of IN HCI __________

Identify the state quantity among the following:

Which of the following units represent largest amount of energy?

Entropy change involved in the conversion of 1 mole of liquid water at 373K to vapour at the same temperature will be (\(\Delta\)H_vap=2.257 kJg^-1) ____________

-\(\Delta\) G is the net work done by the system except ____________

An efficiency of an engine is always ____________

When solid melts there is ____________

Solve: ΔH=10 k cal mol^-1, ΔS=20 cal deg^-1 mol^-1 and T=300k. Then ΔG=?

The condition for standard free energy is _______

For a given reaction \(\triangle\)G obtained was having positive sign convention. State whether the reaction was spontaneous or non-spontaneous.

In an exothermic reaction, heat is evolved and system loses heat to the surroundings. For such system
(i) q_p will be negative
(ii) Δ_rH will be positive
(iii) q_p  will be positive
(iv) Δ_rH will be negative

The heat of neutralisation of strong acid and strong base is __________

Identify the suitable condition(s) which helps the adiabatic process to occur?
(i) ΔT = 0
(ii)ΔP = 0
(iii) q = 0
(iv) w = 0

In a compression process, P_ext is ___________

The gravitational work done by an object is __________

The SI unit of heat is ____________

Which among the following is a path function?

Which among the following is a state function?

Internal energy is denoted by the symbol_______

The process in which temperature of the system remains constant is called __________ process

A portion of matter under consideration, which is separated from rest of universe by real or imaginary boundaries is called_____________

ΔS is expected to be maximum for the reaction ____________

When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0° C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat of released from this combustion in KJ is _____________ (ΔH_c (CH₄) = - 890 KJ mol^-1 and ΔH_c (C₃H₈ = - 2220 KJ mol^-1)

The value of ΔH for cooling 2 moles of an ideal monatomic gas from 125° C to 25° C at constant pressure will be [given C_p = \(\frac{5}{2}\)R] ____________.

The enthalpies of formation of Al₂O₃ and Cr₂O₃ are -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2Al + Cr₂O₃ ⟶ 2Cr + Al₂O₃ is _______________

The intensive property among the quantities below is ____________

In a reversible process, the change in entropy of the universe is ____.