Advertisements
Advertisements
प्रश्न
Following data is given for the reaction: \[\ce{CaCO3 (S) -> CaO (s) + CO2 (g)}\]
\[\ce{∆_fH^Θ [CaO(s)] = - 635.1 kJ mo^{-1}}\]
\[\ce{∆_fH^Θ [CO2(g)] = - 393.5 kJ mol^{-1}}\]
\[\ce{∆_fH^Θ [CaCO3(s)] = - 1206.9 kJ mol^{-1}}\]
Predict the effect of temperature on the equilibrium constant of the above reaction.
उत्तर
\[\ce{∆_rH^Θ = ∆_fH^Θ [CaO(s)] + ∆_fH^Θ [CO2(g)] – ∆_fH^Θ [CaCO3(s)]}\]
∴ \[\ce{∆_rH^Θ = 178.3 kJ mol^{-1}}\]
The reaction is endothermic. Hence, according to Le-Chatelier’s principle, reaction will proceed in forward direction on increasing temperature.
APPEARS IN
संबंधित प्रश्न
A mixture of 1.57 mol of N2, 1.92 mol of H2 and 8.13 mol of NH3 is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant, Kc for the reaction
\[\ce{N2 (g) + 3H2 (g)⇌2NH3 (g)}\] is 1.7 × 102
Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?
Which of the following options will be correct for the stage of half completion of the reaction A ⇌ B.
For the reaction \[\ce{N2O4 (g) ⇌ 2NO2 (g)}\], the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct?
(i) The reaction is endothermic.
(ii) The reaction is exothermic.
T
(iv) The entropy of the system increases.
The value of \[\ce{K_c}\] for the reaction \[\ce{2HI (g) ⇌ H2 (g) + I2 (g)}\] is 1 × 10–4 At a given time, the composition of reaction mixture is \[\ce{[HI]}\] = 2 × 10–5 mol, \[\ce{[HI]}\] = 1 × 10–5 mol and \[\ce{[I2]}\] = 1 × 10–5 mol In which direction will the reaction proceed?
How can you predict the following stages of a reaction by comparing the value of Kc and Qc?
(i) Net reaction proceeds in the forward direction.
(ii) Net reaction proceeds in the backward direction.
(iii) No net reaction occurs.
