Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 52

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Standard enthalpy and standard entropy changes for the oxidation of ammonia at $298 K$ are $- 382.64 {kJmol}^{- 1}$ and $- 145.6 {JK}^{- 1} {mol}^{- 1}$ respectively. Standard Gibb's energy change for the same reaction at $298 K$ is

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Important Questions on Thermodynamics

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 53

The work done during the expansion of a gas from a volume of

4 d m^{3} t o 6 {d m}^{3}

against a constant external pressure of 3 atm is

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 54

A reaction occurs spontaneously if

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 55

Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 56

The absolute enthalpy of neutralisation of the reaction,

MgO (s) + 2 HCl (aq) ⟶ {MgCl}_{2} (aq) + H_{2} O (ℓ)

will be:

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 57

Assume each reaction is carried out in an open container. For which reaction will

ΔH = ΔE

?

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 58

The enthalpy and entropy change for the reaction

{Br}_{2} (l) + {Cl}_{2} (g) \to 2 BrCl (g)

are

30 {kJmol}^{- 1}

and

105 {JK}^{- 1} {mol}^{- 1}

respectively
The temperature at which the reaction will be in equilibrium is

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 59

The enthalpy of combustion of

H_{2},

cyclohexene

(C_{6} H_{10})

and cyclohexane

(C_{6} H_{12})

are

- 241, - 3800

and

- 3920 kJ / mol

respectively. Heat of hydrogenation of cyclohexene is:

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Alpha Question Bank for Medical: Chemistry>Chapter 4 - Thermodynamics>Exercise 4>Q 60

Consider the following reactions:
( $i$ ) $H^{+} (aq) + {OH}^{-} (aq) = H_{2} O (ℓ) - x_{1} kJ {mol}^{- 1}$
( $ii$ ) $H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (ℓ) - x_{2} kJ {mol}^{- 1}$

( $iii$ ) ${CO}_{2} (g) + H_{2} (g) = CO (g) + H_{2} O (ℓ) - x_{3} kJ {mol}^{- 1}$

( $iv$ ) $C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 {CO}_{2} (g) + H_{2} O (ℓ) + x_{4} kJ {mol}^{- 1}$

Enthalpy of formation of $H_{2} O (ℓ)$ is: