For the reaction N 2 g -3 H 2 g - 2 NH 3 g - - H -93-6 kJ mol -1 - The concentration of H 2 at equilibrium will increase ifA- The volume of the system is decreasedB- N2 is added at constant volumeC- N H3 is removedD- The temperature is lowered

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Types of Equillibrium

For the react...

Question

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H = - 93.6 k J m o l^{- 1}$ . The concentration of $H_{2}$ at equilibrium will increase if

The temperature is lowered

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The volume of the system is decreased

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is added at constant volume

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is removed

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Solution

The correct option is B
The volume of the system is decreased

The choices a, c and d will decrease the concentration of $H_{2}$ . The choice b is correct since decreasing volumewill cause the reaction to move in the direction of increasing volume, i.e., towards the larger number ofgaseous species.

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Similar questions

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H = - 93.6 k J m o l^{- 1}$ . The amount (i.e. number of mole) of~ $H_{2}$ at equilibrium will
increase if

For the reaction $2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g), Δ H = 93.6 k J m o l^{- 1}$ . Which of the following is incorrect?

Q. An equilibrium mixture of

N_{2}, H_{2}

and

N H_{3}

700

K contains

0.036

N_{2}

and

0.15

H_{2}

. At this temperature,

K_{c}

for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

0.29

. What is the concentration of

N H_{3}

For the reaction $2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g), Δ H = 93.6 k J m o l^{- 1}$ . Which of the following facts does not hold well?

Q. The following concentration were obtained for the formation of

N H_{3}

form

N_{2}

and

H_{2}

at equilibrium for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

[N_{2}] = 1.5 \times 10^{- 2} M

[H_{2}] = 3.0 \times 10^{- 2} M

[N H_{3}] = 1.2 \times 10^{- 2} M

Calculate equilibrium constant.

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For the reaction N2(g)+3H2(g)⇌2NH3(g),ΔH=−93.6 kJ mol−1. The concentration of H2 at equilibrium will increase if

The correct option is B The volume of the system is decreased The choices a, c and d will decrease the concentration of H2. The choice b is correct since decreasing volumewill cause the reaction to move in the direction of increasing volume, i.e., towards the larger number ofgaseous species.

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H = - 93.6 k J m o l^{- 1}$ . The concentration of $H_{2}$ at equilibrium will increase if

The correct option is B
The volume of the system is decreased

The choices a, c and d will decrease the concentration of $H_{2}$ . The choice b is correct since decreasing volumewill cause the reaction to move in the direction of increasing volume, i.e., towards the larger number ofgaseous species.