$a A (g) + b B (g) ⇌ c C (g) + d D (g)$
In the above reaction, low pressure and high temperature conditions shift equilibrium in backward direction, so the correct set from the following is:

(a + b) > (c + d), Δ H > 0

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

(a + b) < (c + d), Δ H > 0

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

(a + b) < (c + d), Δ H < 0

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

(a + b) > (c + d), Δ H < 0

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

Open in App

Solution

The correct option is A $(a + b) > (c + d), Δ H < 0$
When pressure is decreased, the equilibrium will shift in a direction in which there is increase in the number of moles. Due to this, the pressure will increase and nullify the decrease in the pressure.

When the temperature of an exothermic reaction is increased, the reaction will proceed in the backward direction so as to absorb heat and nullify the effect of increasing temperature.

This will decrease the value of the $Q_{c}$ . In other words, the equilibrium will shift to left. The equilibrium shifts in backward direction by low pressure and high temperature.

This indicates that the total number of moles of reactants is greater than the total number of moles of products or $(a + b) > (c + d)$ . This also indicates that the reaction is exothermic or $Δ H < 0$ .

Suggest Corrections

Similar questions

For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b)

Q. A hypothetical reaction

A \to 2 B

, proceeds through following sequence of steps:
(i)

A \to C; Δ H = q

(ii)

C \to D; Δ H = v

(iii)

\frac{1}{2} D \to B; Δ H = x

Then the heat of reaction is:

For an equilibrium reaction A (g) + B (g) $⇌$ C (g) + D (g), $Δ H$ = -ve. An increase in temperature would cause

Q. In the reaction,

A + B \to C + D; Δ H = 25 k J m o l^{- 1}

. The activation energy is greater than 25 kJ.
if true enter 1, else enter 0.

Q. The correct statement for an exergonic gaseous reaction

A + B ⟶ 3 C

will be:

Join BYJU'S Learning Program

aA(g)+bB(g)⇌cC(g)+dD(g)In the above reaction, low pressure and high temperature conditions shift equilibrium in backward direction, so the correct set from the following is:

$a A (g) + b B (g) ⇌ c C (g) + d D (g)$
In the above reaction, low pressure and high temperature conditions shift equilibrium in backward direction, so the correct set from the following is: