Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 11

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Which one of the following equations does not correctly represent the first law of thermodynamics for the given process ?

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Important Questions on Thermodynamics

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 12

∆ E

is always positive when

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 13

Based on first law of thermodynamics, which one of the following is correct?

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 14

∆ U

is equal to

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 15

A gas is allowed to expand in a well insulated container against a constant external pressure of

2 \cdot 5 atm

from an initial volume of

2 \cdot 50 L

to a final volume of

4 \cdot 50 L

. The change in internal energy

∆ U

of the gas in joules will be

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 16

Standard enthalpy of vaporization

∆_{vap} H^{\circ}

for water at

100 ° C

is

40 \cdot 66 kJ {mol}^{- 1}

. The internal energy change of vaporization of water at

100 ° C (in kJ {mol}^{- 1})

is-

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 17

The value of enthalpy change

(∆ H)

for the reaction

C_{2} H_{5} OH (l) + 3 O_{2} (g) \to 2 {CO}_{2} (g) + 3 H_{2} O (l) at 27 ° C is - 1366 \cdot 5 kJ {mol}^{- 1}

. The value of internal energy change for the above reaction at this temperature will be:

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 18

One mole of a non-ideal gas undergoes a change of state

(2 \cdot 0 atm, 3 \cdot 0 L, 95 K) \to (4 \cdot 0 atm, 5 \cdot 0 L, 245 K)

with a change in internal energy,

∆ U

= 30 \cdot 0 L atm

. The change in enthalpy

(∆ H)

of the process in

L atm

is

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Pradeep's Chemistry Vol 1>Chapter 7 - Thermodynamics>Competition Focus>Q 19

Two moles of an ideal gas expand isothermally and reversibly from

1 litre

to

10 litre

at

300 K

. The enthalpy change (in

kJ

) for the process is