At what temperature does the reduction of lead oxide to lead by carbon becomes spontaneous? `PbO + C rarr Pb(s) + CO(g)`. For the reaction `DeltaH` and `DeltaS` are `108.4 kJ mol^-1` and `190 kJ^-1 mol^-1` respectively/

a) Explain the effect of temperature on the spontaneity of a process based on Gibbs equation. b) For a reaction 2A(g)+B(g)rightarrow2D(g) , enthalpy and entropy changes are - 20.5 kJ mol^-1 and -50.4 J K^-1mol^-1 respectively. Predict whether the reaction occurs at 25^oC.

Given PbO _((s)) + C _((s)) to Pb _((s)) + CO _((g)) , Delta H = 108 kJ mol ^(-1) and Delta S = 190 JK ^(-1) mol ^(-1, reduction of PbO _((s)) is spontaneous

Calculate the standard free energy change for the reaction, Zn+ Cu^(2+) rarr Cu + Zn^(2+) Given that standard free energy (G°) for Zn2+(aq), Cu2+(aq), are -147.2 kJ mol-1 and 65.0 kJ mol-1 respectively.

a) Name the instrument used for measuring the DeltaU of a process. b) What is the value of DeltaG for a reaction at equilibrium? c) DeltaH and DeltaS of a reaction are 30.56 and 0.666 kJ/mol respectively at 1 atm pressure. Calculate the temperature at which the reaction is in equilibrium.

Calculate the standard enthalpy change for the reaction CH_4(g) +2O_2(g) rarr CO_2(g)+2H_2O(l) Given that the standard enthalpies of formation of CH_4(g),CO_2(g), and H_2O(l) are -74.8 kJ mol^-1, -393.5 kJ mol^-1 and -285.8 kJ mol^-1 respectively.

The enthalpy of formation of NaCl(s) is -411.2 kJ mol^(-1). The enthalpy of sublimation of Na(s), its ionization enthalpy in the gaseous state, the bond energy of chlorine, its electron gain enthalpy are 108.4, 495.6, 242 and -348.6 kJ mol^(-1) respectively. The energy required to break one mole of solid sodium chloride into its ions in the gaseous state is (in kJ)