H2S + KClO3 = H2SO4 + KCl

H_2S (hydrogen sulfide) + KClO_3 (potassium chlorate) ⟶ H_2SO_4 (sulfuric acid) + KCl (potassium chloride)

Balance the chemical equation algebraically: H_2S + KClO_3 ⟶ H_2SO_4 + KCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 KClO_3 ⟶ c_3 H_2SO_4 + c_4 KCl Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, Cl, K and O: H: | 2 c_1 = 2 c_3 S: | c_1 = c_3 Cl: | c_2 = c_4 K: | c_2 = c_4 O: | 3 c_2 = 4 c_3 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 4/3 c_3 = 1 c_4 = 4/3 Multiply by the least common denominator, 3, to eliminate fractional coefficients: c_1 = 3 c_2 = 4 c_3 = 3 c_4 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2S + 4 KClO_3 ⟶ 3 H_2SO_4 + 4 KCl

+ ⟶ +

hydrogen sulfide + potassium chlorate ⟶ sulfuric acid + potassium chloride

| hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride molecular enthalpy | -20.6 kJ/mol | -397.7 kJ/mol | -814 kJ/mol | -436.5 kJ/mol total enthalpy | -61.8 kJ/mol | -1591 kJ/mol | -2442 kJ/mol | -1746 kJ/mol | H_initial = -1653 kJ/mol | | H_final = -4188 kJ/mol | ΔH_rxn^0 | -4188 kJ/mol - -1653 kJ/mol = -2535 kJ/mol (exothermic) | | |

| hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride molecular free energy | -33.4 kJ/mol | -296.3 kJ/mol | -690 kJ/mol | -408.5 kJ/mol total free energy | -100.2 kJ/mol | -1185 kJ/mol | -2070 kJ/mol | -1634 kJ/mol | G_initial = -1285 kJ/mol | | G_final = -3704 kJ/mol | ΔG_rxn^0 | -3704 kJ/mol - -1285 kJ/mol = -2419 kJ/mol (exergonic) | | |

| hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride molecular entropy | 206 J/(mol K) | 143 J/(mol K) | 157 J/(mol K) | 83 J/(mol K) total entropy | 618 J/(mol K) | 572 J/(mol K) | 471 J/(mol K) | 332 J/(mol K) | S_initial = 1190 J/(mol K) | | S_final = 803 J/(mol K) | ΔS_rxn^0 | 803 J/(mol K) - 1190 J/(mol K) = -387 J/(mol K) (exoentropic) | | |

K_c = ([H2SO4]^3 [KCl]^4)/([H2S]^3 [KClO3]^4)

rate = -1/3 (Δ[H2S])/(Δt) = -1/4 (Δ[KClO3])/(Δt) = 1/3 (Δ[H2SO4])/(Δt) = 1/4 (Δ[KCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride formula | H_2S | KClO_3 | H_2SO_4 | KCl Hill formula | H_2S | ClKO_3 | H_2O_4S | ClK name | hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride

| hydrogen sulfide | potassium chlorate | sulfuric acid | potassium chloride molar mass | 34.08 g/mol | 122.5 g/mol | 98.07 g/mol | 74.55 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -85 °C | 356 °C | 10.371 °C | 770 °C boiling point | -60 °C | | 279.6 °C | 1420 °C density | 0.001393 g/cm^3 (at 25 °C) | 2.34 g/cm^3 | 1.8305 g/cm^3 | 1.98 g/cm^3 solubility in water | | soluble | very soluble | soluble surface tension | | | 0.0735 N/m | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | odor | | | odorless | odorless