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QUESTION: 1

**Direction (Q. Nos. 1-15) This section contains 15 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.**

**Q.
Assign the sign of work done (based on SI convention) in the following chemical changes taking place against external atmospheric pressure :**

Solution:

Work done = - (change in moles) RT For work done positive change in moles negative and vice versa We only cosider the moles that are in gass phase.

QUESTION: 2

For the following process, H_{2} (g) → 2 H(g), it absorbs 436 kJ mol^{-1}. Thus,

Solution:

It is not mentioned that the process is isobaric. If we assume that process is isobaric, then change in internal energy = 436 kJ mol^{-1}. The data of absorption gives us the value of q.

QUESTION: 3

Suppose the elements X and Y combine to form two compounds XY_{2} and X_{3}Y_{2}. When 0.1 mole of XY_{2} weighs 10 g and 0.05 mole of X_{3}Y_{2} weighs 9 g, the atomic weights of X and Y are

Solution:

Let atomic weight of x = M_{x}

atomic weight of y = M_{y }

we know,

mole = weight /atomic weight

a/c to question,

mole of xy_{2} = 0.1

so,

0.1 = 10g/( M_{x} +2M_{y})

M_{x} + 2M_{y} = 100g -------(1)

for x_{3}y_{2} ; mole of x_{3}y_{2} = 0.05

0.05 = 9/( 3M_{x} + 2M_{y} )

3M_{x} + 2M_{y} = 9/0.05 = 9 × 20 = 180 g ---(2)

solve eqns (1) and (2)

2M_{x} = 80

M_{x} = 40g/mol

and M_{y} = 30g/mole

QUESTION: 4

Five moles of an ideal gas at 27° C are allowed to expand isothermally from an initial pressure of 10.0 atm to a final pressure of 4.0 atm against a constant external pressure of 1.0 atm. Thus, work done will be

Solution:

Work done during isothermal irreversible process is given by the formula w = -p_{ext} (nrt/p_{2}-nrt/p_{1})

QUESTION: 5

56 g of iron reacts with dilute H_{2}SO_{4} at 27° C . W ork done (in cals) in

I. closed vessel of fixed volume and

II. an open vessel is

Solution:

Use ∆H=∆U+∆NgRT FOR 1. we need to find work done in constant volume that is ∆U which will be 0 as it is nCv∆T and since ∆T is zero so ∆U is zero .

For 2. we need to Find ∆H =∆U+∆NgRT Since ∆U is zero so∆H=∆NgRT

R=2 T =300and ∆Ng is = -1

QUESTION: 6

Consider the following properties.

Select intensive and extensive properties.

Solution:

Intensive means that the property is mass independent. We can see that Boiling point, pH, EMF of cell and surface tension are intensive pont .

While Extensive property depends on mass and in given options Volume and entropy are mass dependents.

QUESTION: 7

Consider the following properties.

**State functions are **

**[IITJEE2009]**

Solution:

First 4 are fundamental examples of state functions as they are path independent. Since reversible expansion depends on the path followed by process, so it is a path function. However, irreversible expansion work is independent of the path and so, it is a state function.

QUESTION: 8

For an endothermic reaction when ΔH represents the enthalpy of the reaction in kJ mol^{-1}, the minimum value for the energy of activation will be

**[IIT JEE 1992]**

Solution:

In endothermic reactions, the energy of reactants is less than that of the products. Potential energy diagram for endothermic reactions is,

Where Ea = activation energy of forwarding reaction

Ea' = activation energy of backwards reaction

ΔH = enthalpy of the reaction

From the above diagram,

Ea = Ea' + ΔH

Thus, Ea > ΔH

QUESTION: 9

One mole of an ideal gas is put through a series of changes as shown in the figure in which 1,2,3 mark the three stages of the system. Pressure at the stages 1, 2, and 3 respectively will be (in bar)

Solution:

Applying ideal gas eqn. at 1

p×22.4 = 1×0.0821×298 (since vol. Is in L. R should haave constaant with lit in it.)

p = 1.09 atm. To convert it into bar, we multiply it by 1.01 or we have 1.03 bar

Similarly at 2 and 3, we get value of pressure at 2 and 3.

The most closest answer is option d

QUESTION: 10

An ideal gas expands in volume from 1 × 10^{–3}m^{3} to 1 × 10^{–2}m^{3} at 300K against a constant pressure of 1 × 10^{5}Nm^{–2}. The work done is

**[AIEEE 2004]**

Solution:

QUESTION: 11

One mole each of CaC_{2}, AI_{4}C_{3} and Mg_{2}C_{3} reacts with H_{2}O in separate open flasks at 25° C. Numerical value of the work done by the system is in order

Solution:

i) CaC_{2} + 2H_{2}O → C_{2}H_{2}(g) + Ca(OH)_{2}

ii) Mg_{2}C_{3} + 4H_{2}O → CH_{3-}C≡CH(g) + 2Mg(OH)_{2}

iii) Al_{4}C_{3} + 12H_{2}O → 3CH_{4}(g) + 4Al(OH)_{3}

Work done = -∆n_{g}RT

Or W ∝ ∆n_{g}

Wecan see that in case iii) we have maximum no of moles in the product side(∆n_{g} = 3). So work done will be maximum in case iii). After that in i) and ii), we have the same number of moles on the product side(∆n_{g} = 1), so work done will be the same.

Therefore, option c is correct.

QUESTION: 12

Bond energy of (N— H)bond is x kJ mol^{-1} under standard state. Thus, change in internal energy in the following process is

Solution:

The correct answer is Option B.

H−N−H (three N-H) bonds

∣

H

Thus, ΔE=3xKJmol^{-1}

QUESTION: 13

Temperature of one mole of helium gas is increased by 2°. Thus, increase in internal energy is

Solution:

∆U = nfRT/2

Since He is monoatomic, so f(degree of freedom) = 3

∆U = 3×1×2×2/2 (We have taken R = 2 cal K^{-1} mol ^{-1})

= 6 cal

QUESTION: 14

The internal energy change when a system goes from state A to B is 40kJ/mole. If the system goes from A to B by a reversible path and returns to state A by an irreversible path what would be the net change in internal energy?

Solution:

We know that for a cyclic process the net change in internal energy is equal to zero and change in the internal energy does not depend on the path by which the final state is reached.

QUESTION: 15

The density of ice at 0°C is 0.915 g cm^{-3} and that of liquid water at 0°C is 1.0 g cm^{-3}. Work done for melting 1 mole of ice at 1.00 bar is

Solution:

*Answer can only contain numeric values

QUESTION: 16

**Direction (Q. Nos. 16 - 18) This section contains 3 questions. when worked out will result in an integer from 0 to 9 (both inclusive).**

**Q. **Temperature of one mole of an ideal gas is increased by 1° at constant pressure. What is mechanical work done (in cals)?

Solution:

From ideal gas equation

PV=nRT

hence PV=W

W = nR∆T

W = 1×2×1 = 2cal

*Answer can only contain numeric values

QUESTION: 17

A sample of gas changes from p_{1} V_{1} and T_{1}, to p_{2}, V_{2} and T_{2} by one path and then back to and T_{1}, by another path. How many of the following must be zero for the gas in this cycle?

Solution:

∆T, ∆p, ∆V and ∆U = 0 (also they are state function)

∆U = q+w. So, q and w are not zero.

Hence we have 4 parameters equal to zero after the whole process.

*Answer can only contain numeric values

QUESTION: 18

What will be the temperature change of 1.00 mole of CH_{3}OH(g) if 100 J of heat is added to it under constant volume conditions?

Solution:

For heat added at constant volume, Work doe = 0

∆U = _{T1}∫^{T2} nC_{v,md}T

Or ∆U = nC_{v,m}∆T

∆T = ∆U/nC_{v,m} = 100/1×33.33 = 3

So, the correct answer is 3

QUESTION: 19

**Direction (Q. Nos. 19-20) This section contains a paragraph, wach describing theory, experiments, data etc. three Questions related to paragraph have been given.Each question have only one correct answer among the four given options (a),(b),(c),(d).**

**The following diagram represents the (p-V) changes of a gas.**

**Select isochoric changes**

Solution:

Isochoric change is one in which volume doesn't change(remains constant) From P_{1} to P_{2} , volume is constant(V_{1}) (also work done = 0)

QUESTION: 20

**The following diagram represents the (p-V) changes of a gas.**

**Total work done is**

Solution:

Work done is the area enclosed by PV graph with volume axis.

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