Explanation
Heat required to raise the temperature of a body by 1 k is called thermalcapacity of the body.
50 ml of 1 M KOH + 50 ml of 0.5 M H2SO4 will involve complete neutralisation
250 ml of 4 N NaOH ≡ 500 ml of 2 N NaOH. This will completelyneutralise 500 ml of 2 N HCl.Heat evolved from 1000 ml of 1 N HCl = x (Given) ∴ Heat evolved from 500 ml of 2 N HCl = x
(c)
Eqn. (i) +Eqn. (ii) + Eqn. (iii) gives, X = 131 ‒ 282 ‒ 242 = ‒ 393 kJ.
Eqn. (ii) – Eqn. (i) gives, ΔH = −241.84 −(−285.77) = 43.93kJ.
Average value = (498 + 428)/2= 463 kJ.
Energy absorbed in the dissociation of 1 mole of H2O = 2 × 109 = 218 kcal.This will be the energy released when 1 mole of H2O is formed.
For isothermal expansion of ideal gas, ΔE = 0.
Greater the bond dissociation energy,smaller is the size.
In the given process , there is no transfer of heat or matter between thermodynamic system and its surroundings , hence it is an adiabatic process .
Therefore, q = 0 ,change in internal energy ΔU = 0 . Hence, T = 0(T1 = T2) and P1V1 = P2V2.
Work done in reversible process is maximum .Thus (Tf) irreversible > (Tf) reversible
NH4OH and CH3COOH both are weak.
∆T = T2 – T1 = 298.45 – 298.0 = 0.45 K
∴ Heat produced in calorimeter having capacity 2.5kJK-1 = 0.45×2.5 = 1.125 kJ
∴ Heat produced from 28g of compound = (1.125×28)/3.5 = 9kJ.
If we add the given 3 equations, we get the equation, C(g) + O2(g) → CO2(g),
∆H = ?
∴ ∆H = (131 – 282 – 242) kJ
∆H = -393 kJ
Bond dissociates energies of C – C, C – H and H – H bond are 347, 413 and 354 KJ/mol.
Hence the order is H – H > - C – H > - C – C.
We need the below additional information to determine the average energy for C-H bond formation would be:
The heat of combustion is the energy released as heat when a substance undergoes complete combustion with oxygen under standard conditions. The chemical reaction is typically a hydrocarbon or other organic molecule reacting with oxygen to form carbon-dioxide and water and release heat. ∴ the reaction is,
CH4(g) + 2O2(g) → CO2(g) – 2H2O(l) + heat.
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