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Calculate the temperature above which th...

Calculate the temperature above which the reaction of lead oxide to lead in the following reaction become spontaneous.
`PbO(s) + C(s) rarr Pb(s) + CO(g)`
Given `Delta H = 108.4 kJ mol^(-1), Delta S = 190 JK^(-1) mol^(-1)`

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Above 570.5 K
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Calculate the temperature above which the reduction of lead oxide to lead in the following reaction become spontaneous. PbO(s) + C(s) rightarrow Pb(s) + CO(g) Given Delta H = 118.4 kJ mol^(-1), Delta S = 200 JK^(-1) mol^(-1) .

At what temperature does the reduction of lead oxide to lead by carbon becomes spontaneous? PbO +C rarr Pb(s) +CO(g) For the reacion, DeltaH and DeltaS at 25^(@)C are 108.4 kJ mol^(-1) and 190 J K^(-1) mol^(-1) respectively.

Calculate the free energy change for the following reaction at 300 K. 2CuO_((s)) rarr Cu_(2)O_((s))+(1)/(2)O_(2(g)) Given Delta H = 145.6 kJ mol^(-1) and Delta S = 116.JK^(-1) mol^(-1)

Calculate the temperature above which the given reaction become spontaneous. C_((s)) + H_(2)O_((g)) rarr CO_((g)) + H_(2(g)) DeltaH^(@) = + 131.3 KJ//"mole" , DeltaS^(@) = + 0.1336 KJ//"mole" K

The temperature at which the given reaction is at equilibrium Ag_(2)O_(s) rightarrow 2Ag(s) + 1/2 O_(2)(g) Delta H = 40.5 kJ mol^(-1) and DeltaS= 0.086 k J mol^(-1) K^(-1)

The temperature at which the reaction : Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) is at equilibrium is …….., Given Delta H=30.5 KJ mol^(-1) and Delta S = 0.5 KJ mol^(-1) :

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