Advertisements
Advertisements
प्रश्न
∆S is expected to be maximum for the reaction
पर्याय
\[\ce{Ca_{(S)} + 1/2O2_{(g)} -> CaO_{(S)}}\]
\[\ce{C_{(S)} + O2_{(g)} -> CO2_{(g)}}\]
\[\ce{N2_{(g)} + O2_{(g)} -> 2NO_{(g)}}\]
\[\ce{CaCO3_{(S)} -> CaO_{(S)} + CO2_{(g)}}\]
Advertisements
उत्तर
\[\ce{CaCO3_{(S)} -> CaO_{(S)} + CO2_{(g)}}\]
APPEARS IN
संबंधित प्रश्न
The correct thermodynamic conditions for the spontaneous reaction at all temperature is
The values of ∆H and ∆S for a reaction are respectively 30 kJ mol–1 and 100 JK–1 mol–1. Then the temperature above which the reaction will become spontaneous is
What is the unit of entropy?
Identify the state and path functions out of the following:
- Enthalpy
- Entropy
- Heat
- Temperature
- Work
- Free energy
1 mole of an ideal gas, maintained at 4.1 atm and at a certain temperature, absorbs heat 3710 J and expands to 2 litres. Calculate the entropy change in the expansion process.
30.4 kJ is required to melt one mole of sodium chloride. The entropy change during melting is 28.4 JK−1 mol−1. Calculate the melting point of sodium chloride.
You are given normal boiling points and standard enthalpies of vapourisation. Calculate the entropy of vapourisation of liquids listed below.
| Liquid | Boiling points (°C) | ΔH (kJ mol−1) |
| Ethanol | 78.4 | + 42.4 |
Cyanamide (NH2CN) is completely burnt in excess oxygen in a bomb calorimeter, ΔU was found to be −742.4 kJ mol−1, calculate the enthalpy change of the reaction at 298 K.\[\ce{NH2CN_{(s)} + 3/2 O2_{(g)} -> N2_{(g)} + CO2_{(g)} + H2O_{(l)}}\] ΔH = ?
Calculate the enthalpy of hydrogenation of ethylene from the following data.
Bond energies of C − H, C − C, C = C and H − H are 414, 347, 618 and 435 kJ mol−1.
For the reaction at 298 K: \[\ce{2A + B -> C}\]
ΔH = 400 KJ mol−1; ΔS = 0.2 KJ K−1 mol−1 Determine the temperature at which the reaction would be spontaneous.
