Search

H2SO4 + MnO2 + NaI = H2O + I2 + MnSO4 + NaHSO4

Input interpretation

H_2SO_4 (sulfuric acid) + MnO_2 (manganese dioxide) + NaI (sodium iodide) ⟶ H_2O (water) + I_2 (iodine) + MnSO_4 (manganese(II) sulfate) + NaHSO_4 (sodium bisulfate)
H_2SO_4 (sulfuric acid) + MnO_2 (manganese dioxide) + NaI (sodium iodide) ⟶ H_2O (water) + I_2 (iodine) + MnSO_4 (manganese(II) sulfate) + NaHSO_4 (sodium bisulfate)

Balanced equation

Balance the chemical equation algebraically: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 MnO_2 + c_3 NaI ⟶ c_4 H_2O + c_5 I_2 + c_6 MnSO_4 + c_7 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Mn, I and Na: H: | 2 c_1 = 2 c_4 + c_7 O: | 4 c_1 + 2 c_2 = c_4 + 4 c_6 + 4 c_7 S: | c_1 = c_6 + c_7 Mn: | c_2 = c_6 I: | c_3 = 2 c_5 Na: | c_3 = c_7 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 = 3 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_4
Balance the chemical equation algebraically: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 MnO_2 + c_3 NaI ⟶ c_4 H_2O + c_5 I_2 + c_6 MnSO_4 + c_7 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, Mn, I and Na: H: | 2 c_1 = 2 c_4 + c_7 O: | 4 c_1 + 2 c_2 = c_4 + 4 c_6 + 4 c_7 S: | c_1 = c_6 + c_7 Mn: | c_2 = c_6 I: | c_3 = 2 c_5 Na: | c_3 = c_7 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 = 3 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 1 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_4

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sulfuric acid + manganese dioxide + sodium iodide ⟶ water + iodine + manganese(II) sulfate + sodium bisulfate
sulfuric acid + manganese dioxide + sodium iodide ⟶ water + iodine + manganese(II) sulfate + sodium bisulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_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: 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_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 | 3 | -3 MnO_2 | 1 | -1 NaI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 MnSO_4 | 1 | 1 NaHSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 3 | -3 | ([H2SO4])^(-3) MnO_2 | 1 | -1 | ([MnO2])^(-1) NaI | 2 | -2 | ([NaI])^(-2) H_2O | 2 | 2 | ([H2O])^2 I_2 | 1 | 1 | [I2] MnSO_4 | 1 | 1 | [MnSO4] NaHSO_4 | 2 | 2 | ([NaHSO4])^2 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])^(-3) ([MnO2])^(-1) ([NaI])^(-2) ([H2O])^2 [I2] [MnSO4] ([NaHSO4])^2 = (([H2O])^2 [I2] [MnSO4] ([NaHSO4])^2)/(([H2SO4])^3 [MnO2] ([NaI])^2)
Construct the equilibrium constant, K, expression for: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_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: 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_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 | 3 | -3 MnO_2 | 1 | -1 NaI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 MnSO_4 | 1 | 1 NaHSO_4 | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 3 | -3 | ([H2SO4])^(-3) MnO_2 | 1 | -1 | ([MnO2])^(-1) NaI | 2 | -2 | ([NaI])^(-2) H_2O | 2 | 2 | ([H2O])^2 I_2 | 1 | 1 | [I2] MnSO_4 | 1 | 1 | [MnSO4] NaHSO_4 | 2 | 2 | ([NaHSO4])^2 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])^(-3) ([MnO2])^(-1) ([NaI])^(-2) ([H2O])^2 [I2] [MnSO4] ([NaHSO4])^2 = (([H2O])^2 [I2] [MnSO4] ([NaHSO4])^2)/(([H2SO4])^3 [MnO2] ([NaI])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_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: 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_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 | 3 | -3 MnO_2 | 1 | -1 NaI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 MnSO_4 | 1 | 1 NaHSO_4 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) NaI | 2 | -2 | -1/2 (Δ[NaI])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) MnSO_4 | 1 | 1 | (Δ[MnSO4])/(Δt) NaHSO_4 | 2 | 2 | 1/2 (Δ[NaHSO4])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[MnO2])/(Δt) = -1/2 (Δ[NaI])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = (Δ[MnSO4])/(Δt) = 1/2 (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2SO_4 + MnO_2 + NaI ⟶ H_2O + I_2 + MnSO_4 + NaHSO_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: 3 H_2SO_4 + MnO_2 + 2 NaI ⟶ 2 H_2O + I_2 + MnSO_4 + 2 NaHSO_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 | 3 | -3 MnO_2 | 1 | -1 NaI | 2 | -2 H_2O | 2 | 2 I_2 | 1 | 1 MnSO_4 | 1 | 1 NaHSO_4 | 2 | 2 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 | 3 | -3 | -1/3 (Δ[H2SO4])/(Δt) MnO_2 | 1 | -1 | -(Δ[MnO2])/(Δt) NaI | 2 | -2 | -1/2 (Δ[NaI])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) I_2 | 1 | 1 | (Δ[I2])/(Δt) MnSO_4 | 1 | 1 | (Δ[MnSO4])/(Δt) NaHSO_4 | 2 | 2 | 1/2 (Δ[NaHSO4])/(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 = -1/3 (Δ[H2SO4])/(Δt) = -(Δ[MnO2])/(Δt) = -1/2 (Δ[NaI])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[I2])/(Δt) = (Δ[MnSO4])/(Δt) = 1/2 (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sulfuric acid | manganese dioxide | sodium iodide | water | iodine | manganese(II) sulfate | sodium bisulfate formula | H_2SO_4 | MnO_2 | NaI | H_2O | I_2 | MnSO_4 | NaHSO_4 Hill formula | H_2O_4S | MnO_2 | INa | H_2O | I_2 | MnSO_4 | HNaO_4S name | sulfuric acid | manganese dioxide | sodium iodide | water | iodine | manganese(II) sulfate | sodium bisulfate IUPAC name | sulfuric acid | dioxomanganese | sodium iodide | water | molecular iodine | manganese(+2) cation sulfate |
| sulfuric acid | manganese dioxide | sodium iodide | water | iodine | manganese(II) sulfate | sodium bisulfate formula | H_2SO_4 | MnO_2 | NaI | H_2O | I_2 | MnSO_4 | NaHSO_4 Hill formula | H_2O_4S | MnO_2 | INa | H_2O | I_2 | MnSO_4 | HNaO_4S name | sulfuric acid | manganese dioxide | sodium iodide | water | iodine | manganese(II) sulfate | sodium bisulfate IUPAC name | sulfuric acid | dioxomanganese | sodium iodide | water | molecular iodine | manganese(+2) cation sulfate |

Random Queries

ion class of chromium(VI) cation vs sulfide anion
electronegativity of thulium
formula of zirconium(IV) cation vs molybdenum(III) cation
alternate names of aluminum oleate vs 2-amino-4-methylphenol
common compound names of potassium
H2SO4 + KMnO4 + K4Fe(CN)6 = H2O + K2SO4 + MnSO4 + K3Fe(CN)6
molar mass of phosphide(1-) anion vs phosphorus(IV) cation
flash point of sulfamic acid vs magnesium methyl carbonate
crystal class of urea vs karpatite
O2 + Si2H3 = H2O + SiO2