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[" For a reaction,"4M(s)+nO(2)(g)rarr2M(...

[" For a reaction,"4M(s)+nO_(2)(g)rarr2M_(2)O_(n)(s)," the free energy "],[" change is plotted as a function of temperature.The temperature "],[" below which the oxide is stable could be inferred from the plot "],[" as the point at which: "]

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For a reaction 4 M(s) +nO_2(g) to 2M_2O_n(s) , the free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :

For a reaction 4 M(s) +nO_2(g) to 2M_2O_n(s) , the free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :

Among-the plots of P versus V at constant temperature as given below, which one corresponds to Boyle’s law ?

For the cell reaction , Cu^(2+)(aq)(C_2) +Zn(s) rarrZn^(2+)(aq)(C_1)+Cu(s) , the change in free energy (Delta G) at a given temperature is a function of :

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For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-