You visited us 49 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Oxides of Nitrogen

Two moles of ...

Question

Two moles of gas $A_{2}$ are mixed with two moles of gas $B_{2}$ in a flask of volume 1 lit. If at equilibrium 0.5 moles of $A_{2}$ are obtained. Then find out $K_{p}$ for reaction.
$A_{2} (g)_{+} B_{2} (g) ⇌ 2 A B (g)$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D 36
$K_{p}$ is the equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is a unitless number, although it relates the pressures.
$K p =$ $\frac{(1.5 \times 2)^{2}}{(0.5 \times 0.5)} = 36$
Hence, the answer is 36.

Suggest Corrections

Similar questions

Q. Two moles of gas

A_{2}

are mixed with two moles of gas

B_{2}

in a flask of volume 1lit. If at equilibrium 0.5 moles of

A_{2}

is obtained. Then find out Kp for reaction

A_{2} (g) + B_{2} (g) \to 2 A B (g)

Q. The equilibrium constant of the reaction,

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)

100^{o} C

16.

Initially equal moles of

A_{2} & B_{2}

are taken in

2 L

container. Then find mole % of

A_{2}

in equilibrium mixture.

Q. The equilibrium constant of the reaction

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)

100

50

. If a one litre flash containing one mole of

A_{2}

is connected to a two litre flask containing two moles of

B_{2}

how many moles will be formed at

373 K

The equilibrium constant of the reaction $A 2 (g) + B 2 (g) ⇌ 2 A B (g)$ at $100^{\circ} C$ is 50.

If one litre flask containing one mole of $A_{2}$ is connected to a two litre flask containing two moles of $B_{2}$ the number of moles of AB formed at 373 K will be -

Q.
2mol of

A_{2}

gas in one flask (1 lit volume) is allowed to react with 4 mol of

B_{2}

gas presence in another flask (3 lit volume) as

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g); K_{c} = 4 a t 27^{o} C .

What is the concentration of AB when equilibrium is established?

Join BYJU'S Learning Program

Two moles of gas A2 are mixed with two moles of gas B2 in a flask of volume 1 lit. If at equilibrium 0.5 moles of A2 are obtained. Then find out Kp for reaction.A2(g)+B2(g)⇌2AB(g)

Two moles of gas $A_{2}$ are mixed with two moles of gas $B_{2}$ in a flask of volume 1 lit. If at equilibrium 0.5 moles of $A_{2}$ are obtained. Then find out $K_{p}$ for reaction.
$A_{2} (g)_{+} B_{2} (g) ⇌ 2 A B (g)$