Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
Given, n = 1 mole
P = 4.1 atm
V = 2 Lit
T = ?
q = 3710 J
∆S = `"q"/"T"`
∆S = `"q"/(("PV"/"nR"))`
∆S = `"nRq"/"PV"`
∆S = `(1 xx 0.082 "lit atm K"^-1 xx 3710 "J")/(4.1 "atm" xx 2 "lit")`
∆S = 37.10 JK−1
APPEARS IN
संबंधित प्रश्न
The correct thermodynamic conditions for the spontaneous reaction at all temperature is
∆S is expected to be maximum for the reaction
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
Calculate the entropy change in the system, and surroundings, and the total entropy change in the universe during a process in which 245 J of heat flows out of the system at 77°C to the surrounding at 33°C.
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 |
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) |
| Toluene | 110.6 | + 35.2 |
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 = ?
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.
