H2SO4 + MgO = MgOH2SO4

H_2SO_4 sulfuric acid + MgO magnesium oxide ⟶ MgSO_4·H_2O magnesium sulfate monohydrate

Balance the chemical equation algebraically: H_2SO_4 + MgO ⟶ MgSO_4·H_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 MgO ⟶ c_3 MgSO_4·H_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and Mg: H: | 2 c_1 = 2 c_3 O: | 4 c_1 + c_2 = 5 c_3 S: | c_1 = c_3 Mg: | c_2 = 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 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + MgO ⟶ MgSO_4·H_2O

+ ⟶

sulfuric acid + magnesium oxide ⟶ magnesium sulfate monohydrate

Construct the equilibrium constant, K, expression for: H_2SO_4 + MgO ⟶ MgSO_4·H_2O 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: H_2SO_4 + MgO ⟶ MgSO_4·H_2O 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_2SO_4 | 1 | -1 MgO | 1 | -1 MgSO_4·H_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) MgO | 1 | -1 | ([MgO])^(-1) MgSO_4·H_2O | 1 | 1 | [MgSO4·H2O] 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 = ([H2SO4])^(-1) ([MgO])^(-1) [MgSO4·H2O] = ([MgSO4·H2O])/([H2SO4] [MgO])

Construct the rate of reaction expression for: H_2SO_4 + MgO ⟶ MgSO_4·H_2O 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: H_2SO_4 + MgO ⟶ MgSO_4·H_2O 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_2SO_4 | 1 | -1 MgO | 1 | -1 MgSO_4·H_2O | 1 | 1 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_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) MgO | 1 | -1 | -(Δ[MgO])/(Δt) MgSO_4·H_2O | 1 | 1 | (Δ[MgSO4·H2O])/(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 = -(Δ[H2SO4])/(Δt) = -(Δ[MgO])/(Δt) = (Δ[MgSO4·H2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | magnesium oxide | magnesium sulfate monohydrate formula | H_2SO_4 | MgO | MgSO_4·H_2O Hill formula | H_2O_4S | MgO | H_2MgO_5S name | sulfuric acid | magnesium oxide | magnesium sulfate monohydrate IUPAC name | sulfuric acid | oxomagnesium | magnesium sulfate hydrate

| sulfuric acid | magnesium oxide | magnesium sulfate monohydrate molar mass | 98.07 g/mol | 40.304 g/mol | 138.4 g/mol phase | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 10.371 °C | 2852 °C | 150 °C boiling point | 279.6 °C | 3600 °C | density | 1.8305 g/cm^3 | 3.58 g/cm^3 | 2.57 g/cm^3 solubility in water | very soluble | | soluble surface tension | 0.0735 N/m | | dynamic viscosity | 0.021 Pa s (at 25 °C) | | odor | odorless | odorless |