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K2MnO4 + N2H4 = KOH + MnO2 + N2

Input interpretation

K_2MnO_4 potassium manganate + NH_2NH_2 diazane ⟶ KOH potassium hydroxide + MnO_2 manganese dioxide + N_2 nitrogen
K_2MnO_4 potassium manganate + NH_2NH_2 diazane ⟶ KOH potassium hydroxide + MnO_2 manganese dioxide + N_2 nitrogen

Balanced equation

Balance the chemical equation algebraically: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2MnO_4 + c_2 NH_2NH_2 ⟶ c_3 KOH + c_4 MnO_2 + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, H and N: K: | 2 c_1 = c_3 Mn: | c_1 = c_4 O: | 4 c_1 = c_3 + 2 c_4 H: | 4 c_2 = c_3 N: | 2 c_2 = 2 c_5 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 = 4 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2
Balance the chemical equation algebraically: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2MnO_4 + c_2 NH_2NH_2 ⟶ c_3 KOH + c_4 MnO_2 + c_5 N_2 Set the number of atoms in the reactants equal to the number of atoms in the products for K, Mn, O, H and N: K: | 2 c_1 = c_3 Mn: | c_1 = c_4 O: | 4 c_1 = c_3 + 2 c_4 H: | 4 c_2 = c_3 N: | 2 c_2 = 2 c_5 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 = 4 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

potassium manganate + diazane ⟶ potassium hydroxide + manganese dioxide + nitrogen
potassium manganate + diazane ⟶ potassium hydroxide + manganese dioxide + nitrogen

Equilibrium constant

Construct the equilibrium constant, K, expression for: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 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: 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2 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 K_2MnO_4 | 2 | -2 NH_2NH_2 | 1 | -1 KOH | 4 | 4 MnO_2 | 2 | 2 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2MnO_4 | 2 | -2 | ([K2MnO4])^(-2) NH_2NH_2 | 1 | -1 | ([NH2NH2])^(-1) KOH | 4 | 4 | ([KOH])^4 MnO_2 | 2 | 2 | ([MnO2])^2 N_2 | 1 | 1 | [N2] 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 = ([K2MnO4])^(-2) ([NH2NH2])^(-1) ([KOH])^4 ([MnO2])^2 [N2] = (([KOH])^4 ([MnO2])^2 [N2])/(([K2MnO4])^2 [NH2NH2])
Construct the equilibrium constant, K, expression for: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 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: 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2 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 K_2MnO_4 | 2 | -2 NH_2NH_2 | 1 | -1 KOH | 4 | 4 MnO_2 | 2 | 2 N_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2MnO_4 | 2 | -2 | ([K2MnO4])^(-2) NH_2NH_2 | 1 | -1 | ([NH2NH2])^(-1) KOH | 4 | 4 | ([KOH])^4 MnO_2 | 2 | 2 | ([MnO2])^2 N_2 | 1 | 1 | [N2] 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 = ([K2MnO4])^(-2) ([NH2NH2])^(-1) ([KOH])^4 ([MnO2])^2 [N2] = (([KOH])^4 ([MnO2])^2 [N2])/(([K2MnO4])^2 [NH2NH2])

Rate of reaction

Construct the rate of reaction expression for: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 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: 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2 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 K_2MnO_4 | 2 | -2 NH_2NH_2 | 1 | -1 KOH | 4 | 4 MnO_2 | 2 | 2 N_2 | 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 K_2MnO_4 | 2 | -2 | -1/2 (Δ[K2MnO4])/(Δt) NH_2NH_2 | 1 | -1 | -(Δ[NH2NH2])/(Δt) KOH | 4 | 4 | 1/4 (Δ[KOH])/(Δt) MnO_2 | 2 | 2 | 1/2 (Δ[MnO2])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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 = -1/2 (Δ[K2MnO4])/(Δt) = -(Δ[NH2NH2])/(Δt) = 1/4 (Δ[KOH])/(Δt) = 1/2 (Δ[MnO2])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K_2MnO_4 + NH_2NH_2 ⟶ KOH + MnO_2 + N_2 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: 2 K_2MnO_4 + NH_2NH_2 ⟶ 4 KOH + 2 MnO_2 + N_2 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 K_2MnO_4 | 2 | -2 NH_2NH_2 | 1 | -1 KOH | 4 | 4 MnO_2 | 2 | 2 N_2 | 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 K_2MnO_4 | 2 | -2 | -1/2 (Δ[K2MnO4])/(Δt) NH_2NH_2 | 1 | -1 | -(Δ[NH2NH2])/(Δt) KOH | 4 | 4 | 1/4 (Δ[KOH])/(Δt) MnO_2 | 2 | 2 | 1/2 (Δ[MnO2])/(Δt) N_2 | 1 | 1 | (Δ[N2])/(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 = -1/2 (Δ[K2MnO4])/(Δt) = -(Δ[NH2NH2])/(Δt) = 1/4 (Δ[KOH])/(Δt) = 1/2 (Δ[MnO2])/(Δt) = (Δ[N2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen formula | K_2MnO_4 | NH_2NH_2 | KOH | MnO_2 | N_2 Hill formula | K_2MnO_4 | H_4N_2 | HKO | MnO_2 | N_2 name | potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen IUPAC name | dipotassium dioxido-dioxomanganese | hydrazine | potassium hydroxide | dioxomanganese | molecular nitrogen
| potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen formula | K_2MnO_4 | NH_2NH_2 | KOH | MnO_2 | N_2 Hill formula | K_2MnO_4 | H_4N_2 | HKO | MnO_2 | N_2 name | potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen IUPAC name | dipotassium dioxido-dioxomanganese | hydrazine | potassium hydroxide | dioxomanganese | molecular nitrogen

Substance properties

| potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen molar mass | 197.13 g/mol | 32.046 g/mol | 56.105 g/mol | 86.936 g/mol | 28.014 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) melting point | 190 °C | 1 °C | 406 °C | 535 °C | -210 °C boiling point | | 113.5 °C | 1327 °C | | -195.79 °C density | | 1.011 g/cm^3 | 2.044 g/cm^3 | 5.03 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | decomposes | miscible | soluble | insoluble | insoluble surface tension | | 0.0667 N/m | | | 0.0066 N/m dynamic viscosity | | 8.76×10^-4 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | | | odorless
| potassium manganate | diazane | potassium hydroxide | manganese dioxide | nitrogen molar mass | 197.13 g/mol | 32.046 g/mol | 56.105 g/mol | 86.936 g/mol | 28.014 g/mol phase | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) | gas (at STP) melting point | 190 °C | 1 °C | 406 °C | 535 °C | -210 °C boiling point | | 113.5 °C | 1327 °C | | -195.79 °C density | | 1.011 g/cm^3 | 2.044 g/cm^3 | 5.03 g/cm^3 | 0.001251 g/cm^3 (at 0 °C) solubility in water | decomposes | miscible | soluble | insoluble | insoluble surface tension | | 0.0667 N/m | | | 0.0066 N/m dynamic viscosity | | 8.76×10^-4 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | | 1.78×10^-5 Pa s (at 25 °C) odor | | | | | odorless

Units

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KOH + KMnO4 + CH3COH = H2O + K2MnO4 + CH3COOK