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Ideal Gas Equation

For the react...

Question

For the reaction,

$2 C O + O_{2} \to 2 C O_{2}; Δ H = - 560 K J$ .

Two moles of CO and one mole of $O_{2}$ are taken in a container of volume 1 L. They completely form two moles of $C O_{2}$ the gases deviate appreciably from ideal behaviour. If the pressure in the vessel changes from 70 to 40 atm, then the magnitude (absolute value) of $Δ U$ at 500 K is $x k J$ .

The value of $0.01 x$ is ______(nearest integer).

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Solution

As we know,
$Δ H = Δ U + Δ (P V)$

Volume is constant.

$Δ H = Δ U + V Δ P$

Substituting the given values,
$Δ U = Δ H + V Δ P$

$= - 560 + 1 \times 30 \times 0.1$
$= - 557 k J$

$∵ 1 L - a t m = 0.1 k J$

The value of $0.01 x = 5.57 ≃ 6$

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Similar questions

2 C O + O_{2} \to 2 {C O}_{2}; △ H = 560 k J

Two moles of CO and one mole of

O_{2}

are taken in a container of volume 1 L. They completely form two moles of

{C O}_{2}

, the gases deviated appreciably from ideal behavior. If the pressure in the vessel change from 70 to 40 atm, find the magnitude (absolute value) of

△ U

at 500 K. (1 L atm = 0.1 kJ)

2

C O

1

O_{2}

are taken in a container of volume

1

2

C O_{2}

according to equation

2 C O + O_{2} \to 2 C O_{2}, Δ H = - 560 K J

.

In this process, pressure changes from

70 a t m

40 a t m

. Find out value of

Δ U

500 K

.

[Given: gases deviates apprecially from ideal nature.

1 a t m - l i t r e = 0.1 K J

Q. The dissociation of

C O_{2}

can be expressed as

2 C O_{2} ⇌ 2 C O + O_{2}

. If the 2 moles of

C O_{2}

is taken initially and 40% of the

C O_{2}

is dissociated equilibrium then total number of moles at equilibrium is:

Q. At STP, a container has

1

A r

2

C O_{2}

3

O_{2}

4

N_{2}

. Without changing the total pressure if one mole of

O_{2}

is removed, the partial pressure of

O_{2}

Q. For the reaction,

2 N O (g) + O_{2} (g) \to 2 N O_{2} (g)

Δ H

- 113.1 kJ

6.0 moles

N O

3.0 moles

O_{2}

1.0 atm

300 K

N O_{2}

. Calculate the work done against a pressure of

1.0 atm

R = \frac{1}{12} {L atm mol}^{- 1} K^{- 1}

)

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