Search

NaOH + H2O2 + AgNO3 = H2O + O2 + NaNO3 + Ag

Input interpretation

NaOH sodium hydroxide + H_2O_2 hydrogen peroxide + AgNO_3 silver nitrate ⟶ H_2O water + O_2 oxygen + NaNO_3 sodium nitrate + Ag silver
NaOH sodium hydroxide + H_2O_2 hydrogen peroxide + AgNO_3 silver nitrate ⟶ H_2O water + O_2 oxygen + NaNO_3 sodium nitrate + Ag silver

Balanced equation

Balance the chemical equation algebraically: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_2O_2 + c_3 AgNO_3 ⟶ c_4 H_2O + c_5 O_2 + c_6 NaNO_3 + c_7 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Ag and N: H: | c_1 + 2 c_2 = 2 c_4 Na: | c_1 = c_6 O: | c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 3 c_6 Ag: | c_3 = c_7 N: | c_3 = c_6 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_2 = 1 c_3 = c_1 c_4 = c_1/2 + 1 c_5 = c_1/4 + 1/2 c_6 = c_1 c_7 = c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag
Balance the chemical equation algebraically: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_2O_2 + c_3 AgNO_3 ⟶ c_4 H_2O + c_5 O_2 + c_6 NaNO_3 + c_7 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Ag and N: H: | c_1 + 2 c_2 = 2 c_4 Na: | c_1 = c_6 O: | c_1 + 2 c_2 + 3 c_3 = c_4 + 2 c_5 + 3 c_6 Ag: | c_3 = c_7 N: | c_3 = c_6 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_2 = 1 c_3 = c_1 c_4 = c_1/2 + 1 c_5 = c_1/4 + 1/2 c_6 = c_1 c_7 = c_1 The resulting system of equations is still underdetermined, so an additional coefficient must be set arbitrarily. Set c_1 = 2 and solve for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 2 c_7 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag

Structures

+ + ⟶ + + +
+ + ⟶ + + +

Names

sodium hydroxide + hydrogen peroxide + silver nitrate ⟶ water + oxygen + sodium nitrate + silver
sodium hydroxide + hydrogen peroxide + silver nitrate ⟶ water + oxygen + sodium nitrate + silver

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag 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 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 AgNO_3 | 2 | -2 H_2O | 2 | 2 O_2 | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) H_2O | 2 | 2 | ([H2O])^2 O_2 | 1 | 1 | [O2] NaNO_3 | 2 | 2 | ([NaNO3])^2 Ag | 2 | 2 | ([Ag])^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 = ([NaOH])^(-2) ([H2O2])^(-1) ([AgNO3])^(-2) ([H2O])^2 [O2] ([NaNO3])^2 ([Ag])^2 = (([H2O])^2 [O2] ([NaNO3])^2 ([Ag])^2)/(([NaOH])^2 [H2O2] ([AgNO3])^2)
Construct the equilibrium constant, K, expression for: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag 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 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 AgNO_3 | 2 | -2 H_2O | 2 | 2 O_2 | 1 | 1 NaNO_3 | 2 | 2 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) H_2O_2 | 1 | -1 | ([H2O2])^(-1) AgNO_3 | 2 | -2 | ([AgNO3])^(-2) H_2O | 2 | 2 | ([H2O])^2 O_2 | 1 | 1 | [O2] NaNO_3 | 2 | 2 | ([NaNO3])^2 Ag | 2 | 2 | ([Ag])^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 = ([NaOH])^(-2) ([H2O2])^(-1) ([AgNO3])^(-2) ([H2O])^2 [O2] ([NaNO3])^2 ([Ag])^2 = (([H2O])^2 [O2] ([NaNO3])^2 ([Ag])^2)/(([NaOH])^2 [H2O2] ([AgNO3])^2)

Rate of reaction

Construct the rate of reaction expression for: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag 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 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 AgNO_3 | 2 | -2 H_2O | 2 | 2 O_2 | 1 | 1 NaNO_3 | 2 | 2 Ag | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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[NaOH])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + H_2O_2 + AgNO_3 ⟶ H_2O + O_2 + NaNO_3 + Ag 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 NaOH + H_2O_2 + 2 AgNO_3 ⟶ 2 H_2O + O_2 + 2 NaNO_3 + 2 Ag 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 NaOH | 2 | -2 H_2O_2 | 1 | -1 AgNO_3 | 2 | -2 H_2O | 2 | 2 O_2 | 1 | 1 NaNO_3 | 2 | 2 Ag | 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) H_2O_2 | 1 | -1 | -(Δ[H2O2])/(Δt) AgNO_3 | 2 | -2 | -1/2 (Δ[AgNO3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) O_2 | 1 | 1 | (Δ[O2])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(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[NaOH])/(Δt) = -(Δ[H2O2])/(Δt) = -1/2 (Δ[AgNO3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[O2])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | hydrogen peroxide | silver nitrate | water | oxygen | sodium nitrate | silver formula | NaOH | H_2O_2 | AgNO_3 | H_2O | O_2 | NaNO_3 | Ag Hill formula | HNaO | H_2O_2 | AgNO_3 | H_2O | O_2 | NNaO_3 | Ag name | sodium hydroxide | hydrogen peroxide | silver nitrate | water | oxygen | sodium nitrate | silver IUPAC name | sodium hydroxide | hydrogen peroxide | silver nitrate | water | molecular oxygen | sodium nitrate | silver
| sodium hydroxide | hydrogen peroxide | silver nitrate | water | oxygen | sodium nitrate | silver formula | NaOH | H_2O_2 | AgNO_3 | H_2O | O_2 | NaNO_3 | Ag Hill formula | HNaO | H_2O_2 | AgNO_3 | H_2O | O_2 | NNaO_3 | Ag name | sodium hydroxide | hydrogen peroxide | silver nitrate | water | oxygen | sodium nitrate | silver IUPAC name | sodium hydroxide | hydrogen peroxide | silver nitrate | water | molecular oxygen | sodium nitrate | silver

Random Queries

ions of cobaltous nitrate hexahydrate
alternate names of lead(IV) acetate
CAS number of praseodymium(III) nitrate pentahydrate
formula of mixed sulfur
name of barium tetracyanoplatinate vs pyridinium dichromate
alternate names of telluride anion vs iodide anion
iodine vs ruthenium vs tellurium vs indium vs niobium
alternate names of mercury(II) fluoride
groups of group 14 elements
molar mass of magnesium molybdate