1. Questions

Chemistry

A reaction: A(aq) + B(aq) <-> C(aq)

has a standard free-energy change of –4.65 kJ/mol at 25 °C.

What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

Im not even sure where to start. Can you walk me through this please?

  1. 👍
  2. 👎
  3. 👁
Katherine

  1. I can show you how.
    dG = -RT*lnK
    dG = -4.65 kJ/mol = 4650 J/mol
    substitute in the above and solve for K. Then
    ............A + B ==> C
    I..........0.3..0.4...0
    C..........-x...-x....x
    E........0.3-x...4-x..x
    Substitute the E line into the Keq expression (use K from the first calculation with delta G) and solve for x. Then x, 0.3-x and 0.4-x will give you the equilibrium concns.

    1. 👍
    2. 👎
    DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem

    For the reaction, 3C2H2(g) ===> C6H6 at 25°C, the standard enthalpy change is -631 kJ and the standard entropy change is -430 J/K, Calculate the standard free energy change (in kJ) at 25°C. What is the formula that relates

  2. chemistry

    calculate the lattice energy of sodium oxide (Na2O) from the following data: Ionization energy of Na(g): 495 kJ/mol Electron affinity of O2 for 2e: 603 kJ/mol Energy to vaporize Na(s): 109 kJ/mol O2(g) bond energy: 499 kJ/mol

  3. Chemistry

    C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance So (J/mol∙K) ∆Hºf (kJ/mol) C2H2(g) 200.9 226.7 H2(g) 130.7 0 C2H6(g) -

  4. Chemistry

    The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) --> SnCl4(l)

  1. Chemistry

    Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –44.2 kJ·mol–1. C2H4(G)+H20 ---> C5H5OH ΔS°rxn= ______

  2. Chemistry

    The standard molar Gibbs free energy of formation of NO2 (g) at 298 K is 51.30 kJ · mol −1 and that of N2O4 (g) is 97.82 kJ · mol −1 . What is the equilibrium constant at 25 ◦ C for the reaction 2 NO2(g) N2O4(g) ?

  3. Chemistry/hydrolysis of ATP

    Cells use the hydrolysis of ATP as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose. C6H12O6(s)+6O2(g)¨6CO2(g)+6H2O(l)

  4. chemistry

    The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) --> SnCl4(l)

  1. ap chemistry

    The energy change H associated with the reaction NBr3(g) + 3H2O(g) ! 3HOBr(g) + NH3(g)is +81 kJ/mol rxn. These bond energy values might be useful:O-H 459 kJ/mol; N-H 386 kJ/mol;O-Br 201kJ/mol. The strength of the N Br bond is

  2. Chemistry

    For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g) + O2(g) --> 2NO2(g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for

  3. Chemistry

    C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance/ So (J/mol∙K) /∆Hºf (kJ/mol) C2H2(g) / 200.9 / 226.7 H2(g)/ 130.7 / 0

  4. chemistry

    for the reaction 3C2H2=> C6H6 at 25 C, the standard enthalpy change is -631 KJ and the standard entropy change is -430 J/K. calculate the standard free energy change at 25 C. show all work!

You can view more similar questions or ask a new question.