/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 87 Balance each of the following ox... [FREE SOLUTION] | 91影视

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Chapter 4: Problem 87

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\) d. \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)

Short Answer

Expert verified
a. \(C_2H_6(g) + O_2(g) \rightarrow 2 CO_2(g) + 7 H_2O(g)\) b. \(Mg(s) + 2 HCl(aq) \rightarrow Mg^{2+}(aq) + 2 Cl^-(aq) + H_2(g)\) c. \(Co^{3+}(aq) + Ni(s) \rightarrow Co^{2+}(aq) + Ni^{2+}(aq)\) d. \(Zn(s) + H_2SO_4(aq) \rightarrow ZnSO_4(aq) + H_2(g)\)

Step by step solution

01

Identify the oxidation states

Identify the oxidation states of each element in the reactants and products. C2H6: C = -3, H = +1, O = 0 CO2: C = +4, O = -2 H2O: H = +1, O = -2
02

Find the changes in oxidation states

Determine the changes in oxidation states for each element that undergoes a change. C : -3 -> +4 (change of +7) O : 0 -> -2 (change of -2)
03

Balance the changes in oxidation states

Balance the changes in oxidation states by multiplying the number of atoms by the oxidation states changes. C : 2 atoms * (+7) = +14 O : 2 atoms * (-2) = -4 Since C has 14 units increment and O has 4 units decrement, we must multiply the whole H2O by 7 to balance the oxidation states. C2H6(g) + O2(g) -> 2 CO2(g) + 7 H2O(g) b. Mg(s) + HCl(aq) -> Mg2+(aq) + Cl^-(aq) + H2(g)
04

Identify the oxidation states

Identify the oxidation states of each element in the reactants and products. Mg: 0 HCl: H = +1, Cl = -1 Mg2+: +2 Cl^-: -1 H2: 0
05

Find the changes in oxidation states

Determine the changes in oxidation states for each element that undergoes a change. Mg: 0 -> +2 (change of +2) H: +1 -> 0 (change of -1)
06

Balance the changes in oxidation states

Balance the changes in oxidation states by balancing the number of atoms that change oxidation states. In this case, we see that 1 Mg atom changes from Mg to Mg2+ and 2 H atoms from HCl change to H2. So, we just need to multiply HCl by 2 to balance the equation. Mg(s) + 2 HCl(aq) -> Mg2+(aq) + 2 Cl^-(aq) + H2(g) c. Co3+(aq) + Ni(s) -> Co2+(aq) + Ni2+(aq)
07

Identify the oxidation states

Identify the oxidation states of each element in the reactants and products. Co3+: +3 Ni: 0 Co2+: +2 Ni2+: +2
08

Find the changes in oxidation states

Determine the changes in oxidation states for each element that undergoes a change. Co: +3 -> +2 (change of -1) Ni: 0 -> +2 (change of +2)
09

Balance the changes in oxidation states

Balance the changes in oxidation states by balancing the number of atoms that change oxidation states. In this case, since the changes in oxidation states are already balanced, the equation is already balanced: Co3+(aq) + Ni(s) -> Co2+(aq) + Ni2+(aq) d. Zn(s) + H2SO4(aq) -> ZnSO4(aq) + H2(g)
10

Identify the oxidation states

Identify the oxidation states of each element in the reactants and products. Zn: 0 H2SO4: H = +1, S = +6, O = -2 ZnSO4: Zn = +2, S = +6, O = -2 H2: 0
11

Find the changes in oxidation states

Determine the changes in oxidation states for each element that undergoes a change. Zn: 0 -> +2 (change of +2) H: +1 -> 0 (change of -1)
12

Balance the changes in oxidation states

Balance the changes in oxidation states by balancing the number of atoms that change oxidation states. In this case, we see that 1 Zn atom changes from Zn to Zn2+ and 2 H atoms change from H2SO4 to H2. So, the equation is already balanced: Zn(s) + H2SO4(aq) -> ZnSO4(aq) + H2(g)

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Most popular questions from this chapter

A standard solution is prepared for the analysis of fluoxymesterone \(\left(\mathrm{C}_{20} \mathrm{H}_{29} \mathrm{FO}_{3}\right)\), an anabolic steroid. A stock solution is first prepared by dissolving \(10.0 \mathrm{mg}\) of fluoxymesterone in enough water to give a total volume of \(500.0 \mathrm{~mL}\). A \(100.0-\mu \mathrm{L}\) aliquot (portion) of this solution is diluted to a final volume of \(100.0 \mathrm{~mL}\). Calculate the concentration of the final solution in terms of molarity.

A solution is prepared by dissolving \(0.5842 \mathrm{~g}\) oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make \(100.0 \mathrm{~mL}\) of solution. A \(10.00-\mathrm{mL}\) aliquot (portion) of this solution is then diluted to a final volume of \(250.0\) \(\mathrm{mL}\). What is the final molarity of the oxalic acid solution?

What acid and what base would react in aqueous solution so that the following salts appear as products in the formula equation? Write the balanced formula equation for each reaction. a. potassium perchlorate b. cesium nitrate c. calcium iodide

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \overline{\mathrm{SO}}_{4}\). A \(0.205-\mathrm{g}\) sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The \(\mathrm{BaSO}_{4}\) that is formed is filtered, dried, and weighed. Its mass is \(0.298 \mathrm{~g}\). What mass of \(\mathrm{SO}_{4}{ }^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}{ }^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

A student titrates an unknown amount of potassium hydrogen phthalate \(\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\right.\), often abbreviated \(\mathrm{KHP}\) ) with \(20.46 \mathrm{~mL}\) of a \(0.1000 M\) NaOH solution. KHP (molar mass \(=204.22\) \(\mathrm{g} / \mathrm{mol}\) ) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?
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