A net redox reaction occurs when iodine (I2) is added to an aqueous solution in a copper (Cu) cup. Write a balanced net redox reaction. On the reactant side, write the oxidizing agent first, followed by the reducing agent. On the product side, give the reduced form of the oxidizing agent, followed by the oxidized from of the reducing agents. (Some points will be taken off if you put them in the wrong order.) Be sure to include coefficients, if greater than 1, to balance the reaction. a) +b) →c) +d) Ox1 Red2 Red1 Ox2 e) How many electrons are transferred in the reaction? f) What is the standard cell potential, E∘?
Consider the following balanced redox reaction ClO2-(aq) + H2O(I) + 2Cu+(aq) → ClO-(aq) + 2OH-(aq) + 2Cu2+(aq) Which of the following statements is true? ClO2-(aq) is the oxidizing agent and is oxidized. ClO2-(aq) is the reducing agent and is reduced. ClO2-(aq) is the oxidizing agent and is reduced. ClO2-(aq) is the reducing agent and is oxidized.
Balance the following redox reaction if it occurs in H2SO4. What are the coefficients in front of C8H18O2 and H2SO4 in the balanced reaction? C8H18O2(aq) + Na2Cr2O7(aq) → C8H14O4(aq) + Cr2(SO4)3(aq) C8H18O2 = 1, H2SO4 = 16 C6H18O2 = 3, H2SO4 = 16 C6H18O2 = 2, H2SO4 = 16 C6H18O2 = 2, H2SO4 = 4 C8H18O2 = 3, H2SO4 = 8
The entropy change for the process H2O(s) → H2O(l) is 41.4 J/K and requires that the surroundings transfer 21.7 kJ of heat to the system. Calculate the change in entropy for the universe in kJ/K at 48.0 ∘C.
Calculate the standard entropy change for the following reaction at 25 ∘C. 2S (s, rhombic) +3O2 (g) → 2SO3 (g) Round your answer to 4 significant digits. Note: Reference the Thermodynamic properties of pure substances table for additional information.
An example of a reaction that experiences a big decrease in entropy, ΔS < 0, yet is spontaneous because of the release of a large quantity of heat, ΔH = -598 kJ, is the formation of benzene from acetylene 3C2H2(g) → C6H6(g) The change in free energy under standard condition is: ΔG∘ = -500 kJ/mol. Calculate the equilibrium constant, K, for the reaction at T = 298 K. 2×10^16 6×10^-3 78×10^-65 4×10^87