Advertisements
Advertisements
प्रश्न
At 33K, N2O4 is fifty percent dissociated. Calculate the standard free energy change at this temperature and at one atmosphere.
Advertisements
उत्तर
Given T = 33 K
\[\ce{N2O4 ⇌ 2NO2}\]
Initial concentration: 100% and 0
Concentration dissociated: 50%
Concentration remaining at equilibrium: 50% and 100%
Keq = `100/50` = 2
∆G0 = −2.303 RT log Keq
∆G0= −2.303 × 8.314 × 33 × log 2
∆G0 = −190.18 J mol−1
APPEARS IN
संबंधित प्रश्न
Define is Gibb’s free energy.
The equilibrium constant of a reaction is 10, what will be the sign of ∆G? Will this reaction be spontaneous?
What are the conditions for the spontaneity of a process?
List the characteristics of Gibbs free energy.
For the reaction \[\ce{Ag2O_{(s)} -> 2Ag_{(s)} + 1/2O2_{(g)}}\]: ΔH = 30.56 kJ mol−1 and ΔS = 6.66 JK−1 mol−1 (at 1 atm). Calculate the temperature at which ΔG is equal to zero. Also predict the direction of the reaction
- at this temperature and
- below this temperature.
What is the equilibrium constant Keq for the following reaction at 400 K?
\[\ce{2NOCl_{(g)} ⇌ 2NO_{(g)} + Cl2_{(g)}}\], given that H0 = 77.2 kJ mol−1 and ∆S0 = 122 JK−1 mol−1
When 1-pentyne (A) is treated with 4N alcoholic KOH at 175°C, it is converted slowly into an equilibrium mixture of 1.3% 1-pentyne (A), 95.2% 2-pentyne (B) and 3.5% of 1, 2 pentadiene (C) the equilibrium was maintained at 175°C, calculate ΔG0 for the following equilibria.
\[\ce{B ⇌ A}\] `Δ"G"_1^0` = ?
\[\ce{B ⇌ C}\] `Δ"G"_2^0` = ?
Find out the value of the equilibrium constant for the following reaction at 298 K, \[\ce{2NH3_{(g)} + CO2_{(g)} ⇌ NH2CONH2_{(aq)} + H2O_{(l)}}\] Standard Gibbs energy change, `∆"G"_"r"^0` at the given temperature is –13.6 kJ mol−1.
