Given the balanced equation representing an oxidation – reduction reaction2Al + 3Cu 2+ →→2Al3+ + 3CuWhich statement is true about this reaction?Question 4Answera.Each Al loses 3e- and each Cu2+ gains 2e-b.Each Al loses 2e- and each Cu2+ gains 3e-c.Each Al3+ gains 2e- and each Cu loses 3e-d.Each Al3+ + gains 3e- and each Cu loses 2e-

Consider the following equation representing an oxidation reduction reaction: Zn(s) + CuSO4(aq) →→ ZnSO4(aq) + Cu(s), Which statement is true about this reaction?Question 21Answera.Cu is oxidizedb.Oxygen is reducedc.Zn is oxidizedd.S is reduced

Consider the following reaction.→+2Nas  Cu2+aq + 2Na+aq  CusPart 1 of 4Which species is being oxidized? Select the single best answer.Na+Cu2+NaCuPart 2 of 4Which species is being reduced? Select the single best answer.Na+CuCu2+Na

Consider the reaction shown in the following balanced equation:2 Cu2S (s) + 3 O2 (g) → 2 Cu2O (s) + 2 SO2 (g)You have 1.00 mole each of Cu2S and O2.How many moles of Cu2O can be produced if 1.00 mole of Cu2S reacts? Answer 1 Question 1How many moles of Cu2O can be produced if 1.00 mole of O2 reacts? Answer 2 Question 1The amount of Cu2O that can be produced is smaller from 1.00 mole of Answer 3 Question 1 than the other reagent. Therefore, Answer 4 Question 1 is the limiting reagent and Answer 5 Question 1 is the reagent in excess when 1.00 mole of each is available.  Consider instead that you have 1.00 g each of Cu2S (molar mass of Cu2S is 159 g mol−1) and O2 (molar mass of O2 is 32.0 g mol−1).1.00 g of Cu2S is Answer 6 Question 1 moles of Cu2S and would produce Answer 7 Question 1 moles of Cu2O if all the Cu2S reacts. 1.00 g of O2 is Answer 8 Question 1 moles of O2 and would produce Answer 9 Question 1 moles of Cu2O if all the O2 reacts.The amount of Cu2O that can be produced is smaller from 1.00 g of Answer 10 Question 1 than the other reagent. Therefore, Answer 11 Question 1 is the limiting reagent and Answer 12 Question 1 is the reagent in excess when 1.00 g of each is available.

5. Copy out and balance the following equations:a ...Cu+O2 → ...CuOb N2+...H2...NH3 c...Na + O2...Na2Oc ...NaOH + H2SO4 Na2SO4 + ...H2Oe ...Al+...Cl2 → ...AlCl3f ...Fe+...H2O...Fe3O4+...H2

Is it possible to have a reaction in which oxidation occurs and reduction does not.Question 2Answera.Falseb.True