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N2O4 AT 2 ATM...

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N2O4 AT 2 ATM IS INTRODUCED IN A 12L RIGID VESSEL AT 300 K .TEMP. IS INCRESED TO 600K DUE TO WHICH 50% OF N2O4 DISSOCIATE INTO NO2.CALCULATE FINAL PRESSURE OF SYSTEM

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N_{2} O_{4}

dissociates into gaseous

N O_{2}

according to the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

at 300 K and 1 atm pressure, the degree of dissociation of

N_{2} O_{4}

is 0.2. If one mole of

N_{2} O_{4}

gas is contained in a vessel, then the density of the equilibrium mixture is :

27^{o} C

and 1 atm pressure,

N_{2} O_{4}

is 20% dissociation into

N O_{2}

. What is the density of equilibrium mixture of

N_{2} O_{4}

N O_{2}

27^{o} C

60^{o}

N_{2} O_{4}

is 50% dissociated into

N O_{2}

36.6 g N_{2} O_{4} (g)

is introduced into a

1.0 - l i t r e

27^{\circ} C

. The following equilibrium reaction occurs:

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); K_{p} = 0.1642 a t m

.
(a) Calculate

K_{c}

of the equilibrium reaction?
(b) What are the number of moles of

N_{2} O_{4}

N O_{2}

at equilibrium?
(c) What is the total gas pressure in the flask at equilibrium?
(d) What is the percent dissociation of

N_{2} O_{4}

340

1

N_{2} O_{4}

66 %

dissociated into

N O_{2}

. What volume does

10

N_{2} O_{4}

occupy under these conditions?

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