H2SO4 + Zn(NO3)2 = HNO3 + ZnSO4

Input interpretation

Image
Text

H_2SO_4 sulfuric acid + Zn(NO3)2 ⟶ HNO_3 nitric acid + ZnSO_4 zinc sulfate

Balanced equation

Image
Text

Balance the chemical equation algebraically: H_2SO_4 + Zn(NO3)2 ⟶ HNO_3 + ZnSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 Zn(NO3)2 ⟶ c_3 HNO_3 + c_4 ZnSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Zn and N: H: | 2 c_1 = c_3 O: | 4 c_1 + 6 c_2 = 3 c_3 + 4 c_4 S: | c_1 = c_4 Zn: | c_2 = c_4 N: | 2 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 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + Zn(NO3)2 ⟶ 2 HNO_3 + ZnSO_4

+ Zn(NO3)2 ⟶ +

Names

Image
Text

sulfuric acid + Zn(NO3)2 ⟶ nitric acid + zinc sulfate

Equilibrium constant

Image
Text

Construct the equilibrium constant, K, expression for: H_2SO_4 + Zn(NO3)2 ⟶ HNO_3 + ZnSO_4 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 + Zn(NO3)2 ⟶ 2 HNO_3 + ZnSO_4 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 Zn(NO3)2 | 1 | -1 HNO_3 | 2 | 2 ZnSO_4 | 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) Zn(NO3)2 | 1 | -1 | ([Zn(NO3)2])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 ZnSO_4 | 1 | 1 | [ZnSO4] 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) ([Zn(NO3)2])^(-1) ([HNO3])^2 [ZnSO4] = (([HNO3])^2 [ZnSO4])/([H2SO4] [Zn(NO3)2])

Rate of reaction

Image
Text

Construct the rate of reaction expression for: H_2SO_4 + Zn(NO3)2 ⟶ HNO_3 + ZnSO_4 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 + Zn(NO3)2 ⟶ 2 HNO_3 + ZnSO_4 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 Zn(NO3)2 | 1 | -1 HNO_3 | 2 | 2 ZnSO_4 | 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) Zn(NO3)2 | 1 | -1 | -(Δ[Zn(NO3)2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) ZnSO_4 | 1 | 1 | (Δ[ZnSO4])/(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[Zn(NO3)2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[ZnSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)