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- -6 -5 -4 -3 -2 -1 +1 +2 +3 +4 +5 PbsO.(s) + H*(aq) + 2CI (aq) = Pb(s) + HSO. (aq) + Cl2(g)2 Ba2+ (aq) + Cr20,2 (aq) + H2O (I) 2 BaCro4 (s) + 2 H* (aq) Dichromate forms orange aqueous solutions and barium chromate is a white solid. Ba(NO3)2 is placed into a test tube of aqueous K2Cr207 forming a colorless solution with a noticeable amount of white solid at the bottom. Use Le Chatelier's Principles to answer the following questions. A. What would you expect to observe if HC was added to the test tube? Explain why the expected observation occurred. B. What could you add to the test tube to increase the amount of solid that would form? Explain why you chose that substance. C. You cool the test tube and notice an increase in the amount of solid formed in the solution. Explain what that suggests about the above reaction?Complete the following reactions below. If no reaction occurred, write NR. Cu(s) + CusO4(aq) –> Cu(s) + ZnSO4(aq) -> Zn(s) + ZnSO4(aq) - Zn(s) + CuSO4(aq) ->
- Write a Nernst Equation for : 6Fe2+ (aq) + Cr2O7 2- (aq) + 14 H+ (aq) --à 2 Cr3+(aq) + 7H2O(l) + 6Fe3+(aq)Predict the products of the following reactions. Ag+(aq) + Mg(s) → Cu2+(aq) + Ag(s) → Zn2+(aq) + Pb(s) → Mg2+(aq) + Fe(s) → Pb(s) + AgNO3(aq) → Ag+(aq) + Mg2+(aq) →Write the expression Kc for the following reactions. (a) Fe2+(aq) + Ce4+(aq) ⇋ Fe3+(aq) + Ce3+(aq) (b) CaCO3(s) ⇋ CaO(s) + CO3(g)
- Given the following reaction, which occurs in acid solution: CH3CH2OH(l) + Cr2O72-(aq) -> CH3COOH(aq) + Cr3+(aq) Balance this equation using the half equation method.Determine the oxidizing agent in the following reaction: 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(1). Fe2+ BrO3- H+ Br- Fe3+Although KOH, R6OH, and CSOH have little association between metal and hydroxide in aqueous solution, Lit and Na+ do form complexes with OH : [LIOH(aq)] Lit + OH- = LIOH(aq) K1 [Li* ][OH¯] = 0.83 [NAOH(aq)] Na+ + OH = NaOH(aq) K1 = [Na+ ][OH ] = 0.20 Prepare a table showing initial and final concentrations of Lit, OH, and LIOH(aq) in 1.00 F LIOH solution. Calculate the fraction of lithium in the form LİOH(aq) at equilibrium. fraction as LIOH(aq):
- The following oxidation-reduction reactions take place in basic medium. For each reaction, (i) Assign oxidation state for each atom in the equation; (ii) Indicate oxidation half-equation and reduction half-equation; (iii) Balance the equation by half-equation method; (iv) Indicate which reactant is oxidizing agent and which reducing agent. (v) State and verify whether the pH of the medium decreases, increases, or remains constant as the reaction proceeds.Complete the following chemical equations : (i) MnO4 (aq) + S2O32- (aq) + H2O (1)→(ii) Cr2O72- (aq) + Fe2+ (aq) + H+ (aq)→Given: 2H+(aq) + 2e– → H2(g); 0.00 VRb+(aq) + e– → Rb(s); –2.98 VF2(g) + 2e– → 2F–(aq); 2.87 VAl3+(aq) + 3e– → Al(s); –1.66 VPb2+(aq) + 2e– → Pb(s); –0.13 V Under standard-state conditions, which are the strongest reducing and oxidizing agents? Group of answer choices H+ and F2 Rb and Pb2+ Al3+ and F2 Rb and F2 Rb and F–