For the reaction, 2Cl(g)toCl_(2)(g), what are the signs of DeltaH and DeltaS ?
For A _((g)) + B _((s)) to 2 C _((g)) , Delta H and Delta S respectively are 50 KJ and 100 J/K respectively. Then at 228 ^(@)C
An equilibrium reaction X + Y hArr W +Z, Delta H= +ve is spontaneous in the forward direction. Then corresponding sign of Delta G and Delta S should be respectively
From the following data at 25^(@)C {:("Reaction ",Delta_(r) H^(@) kJ//mol),((1)/(2)H_(2)(g) + (1)/(2)O_(2)(g) rarr OH (g),42),(H_(2)(g) + (1)/(2)O_(2)(g) rarr H_(2)O_(g),-242),(H_(2)(g) rarr 2H(g),436),(O_(2)(g) rarr 2O(g),495):} Which of the following statement(s) is/are correct: Statement (a): Delta_(r)H^(@) for the reaction H_(2)O(g) rarr 2H(g) + O(g) Statement (b): Delta_(r)H^(@) for the reaction OH(g) rarr H(g) + O(g) is Statement (c) : Enthalpy of formation of H(g) is -218 kJ/mol Statement (d): Enthalpy of formation of OH(g) is 42 kJ/mol
For the reaction: 2H_(2(g)) + O_(2(g)) rarr 2H_2O_((g)) , DeltaH = -571 kJ bond energy of (H-H) = 435 kJ, of (O = O) = 498kJ , then the average bond energy of O-H bond using the above data
The enthalpy of the reaction H_(2(g)) + O_(2(g)) rarr H_2O_((g)) is DeltaH_1 and that of H_(2(g)) + O_(2(g)) rarr H_(2)O_((l)) is Delta H_2 . Then
For the reaction 2H_(2(g)) + o_(2(g)) rarr 2H_(2)O_((g)), Delta H^(@) = - 573.2 kJ . The heat of decomposition of water per mol is:
in manufacture of NO, the reaction N_(2(g)) + O_(2(g)) hArr 2NO_((g)). Delta H + ve is favourable if :
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
