Search

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

Random Queries

chemical types of 3-chloro-2-hydroxypropyl methacrylate
molar mass of diocide
density of 2-thienyllithium vs lead(II) oxalate
H2SO4 + Fe2O3 + CuI = H2O + I2 + CuSO4 + FeSO4
relative molecular mass of benzene vs chloroform
CAS number of lead(II) zirconate vs uranium dioxide
atomic radius of hydrogen vs cadmium
DOT numbers of beryllium hydride
molar mass of lithium fluoride vs sodium bromate
formula of mercuric oxide vs osmium nonacarbonyl