show work 2. Consider the following reaction:HCO, (aq) = H+(aq)+ CO?-(aq)at room temperature (298 K).a) What is AGran when the equilibrium concentrations are AGn+59.0 kJ/mol and [HCO, (aq)]M, and pH is 5.3.10 M, [CO? (aq)]= 1.30×10-4b) Would the reaction be spontaneous in forward direction at pH 10 (withall other concentrations as above)?c) What is the value for equilibrium constant?d) Is this a redox reaction? (i.e., does the oxidation state of the carbonchange?)

∆G = ∆G° + RT ln Q here Q = reaction quotient if ∆Grxn is negative then reaction is spontaneous…

2. Consider the following reaction: HCO, (ag) = H*(aq) + CO?-(aq) at room temperature (298 K). a) What is AGræn when the equilibrium concentrations are AGn +59.0 kJ/mol and [HCO5 (aq)] = 3.10 M, [CO?-(aq)] = 1.30×10-4 M, and pH is 5. b) Would the reaction be spontaneous in forward direction at pH 10 (with all other concentrations as above)? c) What is the value for equilibrium constant? d) Is this a redox reaction? (i.e., does the oxidation state of the carbon change?)