Ncert Solutions Chemistry Class 11th

For a real at 25°C temperature and high pressure (99 bar) the value of compressibility factor is 2, so the value of Vander Waal's constant 'b' should be__________* 10^-² L mol^-¹. (Nearest Integer)

(Given R = 0.083 L bar K^-¹ mol^-¹)

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For real gas under high pressure,

$Z = 1 + \frac{P b}{R T} \Rightarrow b = \frac{R T}{P} = \frac{0.083 * 298}{99}$

= 0.25 * 10^-2 L mol^-1

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The molar heat capacity for an ideal gas at constant pressure is 20.785JK^-1 mol^-1. The change in internal energy is 5000 J upon heating it from 300 K to 500 K. The number of moles of the gas at constant volume is __________. (Nearest Integer)

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$C_{P, m} = C_{v, m} + R$

$C_{v, m} = 20.785 - 8.314 = 12.471 J K^{- 1} m o l^{- 1}$

$n = \frac{5000}{12.471 * 200} = \frac{25}{12.471} \approx 2$

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Amongst the following, the number of oxide(s) which are paramagnetic in nature is Na₂O, KO₂, NO₂, N₂O, ClO₂, NO, SO₂, Cl₂O (Nearest Integer)

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$K O_{2}, N O_{2}, C l O_{2}, N O$ are paramagnetic.

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While performing a thermodynamics experiment, a student made the following observation.

HCl + NaOH → NaCl + H₂O $Δ H$ = -57.3 kJ mol^?1

CH₃COOH + NaOH → CH₃COONa + H₂O $Δ H$ = -55.3 kJ mol^-1

The enthalpy of ionization of CH₃COOH as calculated by the student is _________kJ mol^-1. (nearest integer)

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$Δ H_{i o n i z a t i o n} o f C H_{3} C O O H = - 55.3 (- 57.3)$

= 2 KJ/mole

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A sealed flask with a capacity of 2 dm³ contains 11g of propane gas. The flask is so weak that it will burst if the pressure becomes 2 MPa. The minimum temperature at which the flask will burst is _________ $° C$ . [Nearest integer]

(Given: R = 8.3 JK^-1 mol^-1. Atomic masses of C and H are 12u and 1u, respectively)

(Assume that propane behaves as an ideal gas.)

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V = 2 $l$ , n = 0.25 Moles, P = 2 * 106 Pa, R = 8.314 J/mol.k

PV = nRT

$2 * 1 0^{6} * 2 * 1 0^{- 3} = 0.25 * 8.314 * T$

T = 1654.7 $\approx$ 1655 K

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The number of sp³hybridised carbons in an acyclic neutral compound with molecular formula C₄H₅N is __________.

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Degree of unsaturation = 4 + 1 - $(\frac{5 - 1}{2}) = 3$

sp³ hybridized only one carbon

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While estimating the nitrogen present in an organic compound by Kjeldahl's method, the ammonia evolved from 0.25 g of the compound neutralized 2.5 mL of M H₂SO₄. The percentage of nitrogen present in organic compound is _________.

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Organic compound -> NH₃

$2 N H_{3} + H_{2} S O_{4} \to {(N H_{4})}_{2} S O_{4}$

No. of millimoles of NH₃ = 2 * no. of milimoles of H₂SO₄

= 2 * 2 * 2.5

= 10 milimoles

= No. of milimoles of N

Mass of nitrogen = $\frac{10}{100} * 14 = 0.14 g m$

% of Nitrogen in compound = $\frac{0.14}{0.25} * 100$

= 56%

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The pressure of a moist gas at $27 ° C$ is 0.04 atm. The volume of the container is doubled at the same temperature. The new pressure of the moist gas is _______ * 10^-1atm. (Nearest integer)

(Given: The vapour pressure of water at $27 ° C$ is 0.4 atm)

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Pressure of gas = pressure of moist gas – Vapour pressure of water

= 4 atm – 0.4 atm

= 3.6 atm

On doubling the volume, pressure of gas is halved :

Total pressure = $(\frac{3.6}{2} + 0.4) = 2.2 a t m$

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The number of stereoisomers formed in a reaction of

$(\pm) P h (C = O) C (O H) (C N) P h w i t h H C N i s____________.$

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'x' g of molecular oxygen(O₂) is mixed with 200g of neon (Ne). The total pressure of the non-reactive mixture of O₂ and Ne in the cylinder is 25 bar. The partial pressure of Ne is 20 bar at the same temperature and volume. The value of 'x' is_________.

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