H2O + KMnO4 + C4H8 = KOH + MnO2 + C4H10O2

H_2O water + KMnO_4 potassium permanganate + (CH_3)_2C=CH_2 isobutylene ⟶ KOH potassium hydroxide + MnO_2 manganese dioxide + C_2H_5OCH_2CH_2OH 2-ethoxyethanol

Balance the chemical equation algebraically: H_2O + KMnO_4 + (CH_3)_2C=CH_2 ⟶ KOH + MnO_2 + C_2H_5OCH_2CH_2OH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 KMnO_4 + c_3 (CH_3)_2C=CH_2 ⟶ c_4 KOH + c_5 MnO_2 + c_6 C_2H_5OCH_2CH_2OH Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, K, Mn and C: H: | 2 c_1 + 8 c_3 = c_4 + 10 c_6 O: | c_1 + 4 c_2 = c_4 + 2 c_5 + 2 c_6 K: | c_2 = c_4 Mn: | c_2 = c_5 C: | 4 c_3 = 4 c_6 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 3/2 c_4 = 1 c_5 = 1 c_6 = 3/2 Multiply by the least common denominator, 2, to eliminate fractional coefficients: c_1 = 4 c_2 = 2 c_3 = 3 c_4 = 2 c_5 = 2 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 H_2O + 2 KMnO_4 + 3 (CH_3)_2C=CH_2 ⟶ 2 KOH + 2 MnO_2 + 3 C_2H_5OCH_2CH_2OH

+ + ⟶ + +

water + potassium permanganate + isobutylene ⟶ potassium hydroxide + manganese dioxide + 2-ethoxyethanol

Construct the equilibrium constant, K, expression for: H_2O + KMnO_4 + (CH_3)_2C=CH_2 ⟶ KOH + MnO_2 + C_2H_5OCH_2CH_2OH Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 4 H_2O + 2 KMnO_4 + 3 (CH_3)_2C=CH_2 ⟶ 2 KOH + 2 MnO_2 + 3 C_2H_5OCH_2CH_2OH Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2O | 4 | -4 KMnO_4 | 2 | -2 (CH_3)_2C=CH_2 | 3 | -3 KOH | 2 | 2 MnO_2 | 2 | 2 C_2H_5OCH_2CH_2OH | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 4 | -4 | ([H2O])^(-4) KMnO_4 | 2 | -2 | ([KMnO4])^(-2) (CH_3)_2C=CH_2 | 3 | -3 | ([(CH3)2C=CH2])^(-3) KOH | 2 | 2 | ([KOH])^2 MnO_2 | 2 | 2 | ([MnO2])^2 C_2H_5OCH_2CH_2OH | 3 | 3 | ([C2H5OCH2CH2OH])^3 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([H2O])^(-4) ([KMnO4])^(-2) ([(CH3)2C=CH2])^(-3) ([KOH])^2 ([MnO2])^2 ([C2H5OCH2CH2OH])^3 = (([KOH])^2 ([MnO2])^2 ([C2H5OCH2CH2OH])^3)/(([H2O])^4 ([KMnO4])^2 ([(CH3)2C=CH2])^3)

Construct the rate of reaction expression for: H_2O + KMnO_4 + (CH_3)_2C=CH_2 ⟶ KOH + MnO_2 + C_2H_5OCH_2CH_2OH Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 4 H_2O + 2 KMnO_4 + 3 (CH_3)_2C=CH_2 ⟶ 2 KOH + 2 MnO_2 + 3 C_2H_5OCH_2CH_2OH Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2O | 4 | -4 KMnO_4 | 2 | -2 (CH_3)_2C=CH_2 | 3 | -3 KOH | 2 | 2 MnO_2 | 2 | 2 C_2H_5OCH_2CH_2OH | 3 | 3 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term H_2O | 4 | -4 | -1/4 (Δ[H2O])/(Δt) KMnO_4 | 2 | -2 | -1/2 (Δ[KMnO4])/(Δt) (CH_3)_2C=CH_2 | 3 | -3 | -1/3 (Δ[(CH3)2C=CH2])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) MnO_2 | 2 | 2 | 1/2 (Δ[MnO2])/(Δt) C_2H_5OCH_2CH_2OH | 3 | 3 | 1/3 (Δ[C2H5OCH2CH2OH])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/4 (Δ[H2O])/(Δt) = -1/2 (Δ[KMnO4])/(Δt) = -1/3 (Δ[(CH3)2C=CH2])/(Δt) = 1/2 (Δ[KOH])/(Δt) = 1/2 (Δ[MnO2])/(Δt) = 1/3 (Δ[C2H5OCH2CH2OH])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| water | potassium permanganate | isobutylene | potassium hydroxide | manganese dioxide | 2-ethoxyethanol formula | H_2O | KMnO_4 | (CH_3)_2C=CH_2 | KOH | MnO_2 | C_2H_5OCH_2CH_2OH Hill formula | H_2O | KMnO_4 | C_4H_8 | HKO | MnO_2 | C_4H_10O_2 name | water | potassium permanganate | isobutylene | potassium hydroxide | manganese dioxide | 2-ethoxyethanol IUPAC name | water | potassium permanganate | 2-methylprop-1-ene | potassium hydroxide | dioxomanganese | 2-ethoxyethanol

| water | potassium permanganate | isobutylene | potassium hydroxide | manganese dioxide | 2-ethoxyethanol molar mass | 18.015 g/mol | 158.03 g/mol | 56.11 g/mol | 56.105 g/mol | 86.936 g/mol | 90.12 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) melting point | 0 °C | 240 °C | -140 °C | 406 °C | 535 °C | -90 °C boiling point | 99.9839 °C | | -6.9 °C | 1327 °C | | 135 °C density | 1 g/cm^3 | 1 g/cm^3 | 0.5942 g/cm^3 (at 20 °C) | 2.044 g/cm^3 | 5.03 g/cm^3 | 0.93 g/cm^3 solubility in water | | | insoluble | soluble | insoluble | miscible surface tension | 0.0728 N/m | | 0.0123 N/m | | | 0.0282 N/m dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.084×10^-6 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | | 0.00214 Pa s (at 20 °C) odor | odorless | odorless | | | | sweet | ether