Search

H2O + Li2SO3 + Cu(HCOO)2 = LiHSO3 + (CuOH)2SO3 + LiHCOO

Input interpretation

H_2O water + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO
H_2O water + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO

Balanced equation

Balance the chemical equation algebraically: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Li2SO3 + c_3 Cu(HCOO)2 ⟶ c_4 LiHSO3 + c_5 (CuOH)2SO3 + c_6 LiHCOO Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Li, S, Cu and C: H: | 2 c_1 + 2 c_3 = c_4 + 2 c_5 + c_6 O: | c_1 + 3 c_2 + 4 c_3 = 3 c_4 + 5 c_5 + 2 c_6 Li: | 2 c_2 = c_4 + c_6 S: | c_2 = c_4 + c_5 Cu: | c_3 = 2 c_5 C: | 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO
Balance the chemical equation algebraically: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Li2SO3 + c_3 Cu(HCOO)2 ⟶ c_4 LiHSO3 + c_5 (CuOH)2SO3 + c_6 LiHCOO Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, Li, S, Cu and C: H: | 2 c_1 + 2 c_3 = c_4 + 2 c_5 + c_6 O: | c_1 + 3 c_2 + 4 c_3 = 3 c_4 + 5 c_5 + 2 c_6 Li: | 2 c_2 = c_4 + c_6 S: | c_2 = c_4 + c_5 Cu: | c_3 = 2 c_5 C: | 2 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_5 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 2 c_4 = 2 c_5 = 1 c_6 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO

Structures

+ Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO
+ Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO

Names

water + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO
water + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO 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 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO 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_2O | 2 | -2 Li2SO3 | 3 | -3 Cu(HCOO)2 | 2 | -2 LiHSO3 | 2 | 2 (CuOH)2SO3 | 1 | 1 LiHCOO | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) Li2SO3 | 3 | -3 | ([Li2SO3])^(-3) Cu(HCOO)2 | 2 | -2 | ([Cu(HCOO)2])^(-2) LiHSO3 | 2 | 2 | ([LiHSO3])^2 (CuOH)2SO3 | 1 | 1 | [(CuOH)2SO3] LiHCOO | 4 | 4 | ([LiHCOO])^4 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 = ([H2O])^(-2) ([Li2SO3])^(-3) ([Cu(HCOO)2])^(-2) ([LiHSO3])^2 [(CuOH)2SO3] ([LiHCOO])^4 = (([LiHSO3])^2 [(CuOH)2SO3] ([LiHCOO])^4)/(([H2O])^2 ([Li2SO3])^3 ([Cu(HCOO)2])^2)
Construct the equilibrium constant, K, expression for: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO 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 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO 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_2O | 2 | -2 Li2SO3 | 3 | -3 Cu(HCOO)2 | 2 | -2 LiHSO3 | 2 | 2 (CuOH)2SO3 | 1 | 1 LiHCOO | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2O | 2 | -2 | ([H2O])^(-2) Li2SO3 | 3 | -3 | ([Li2SO3])^(-3) Cu(HCOO)2 | 2 | -2 | ([Cu(HCOO)2])^(-2) LiHSO3 | 2 | 2 | ([LiHSO3])^2 (CuOH)2SO3 | 1 | 1 | [(CuOH)2SO3] LiHCOO | 4 | 4 | ([LiHCOO])^4 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 = ([H2O])^(-2) ([Li2SO3])^(-3) ([Cu(HCOO)2])^(-2) ([LiHSO3])^2 [(CuOH)2SO3] ([LiHCOO])^4 = (([LiHSO3])^2 [(CuOH)2SO3] ([LiHCOO])^4)/(([H2O])^2 ([Li2SO3])^3 ([Cu(HCOO)2])^2)

Rate of reaction

Construct the rate of reaction expression for: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO 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 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO 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_2O | 2 | -2 Li2SO3 | 3 | -3 Cu(HCOO)2 | 2 | -2 LiHSO3 | 2 | 2 (CuOH)2SO3 | 1 | 1 LiHCOO | 4 | 4 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Li2SO3 | 3 | -3 | -1/3 (Δ[Li2SO3])/(Δt) Cu(HCOO)2 | 2 | -2 | -1/2 (Δ[Cu(HCOO)2])/(Δt) LiHSO3 | 2 | 2 | 1/2 (Δ[LiHSO3])/(Δt) (CuOH)2SO3 | 1 | 1 | (Δ[(CuOH)2SO3])/(Δt) LiHCOO | 4 | 4 | 1/4 (Δ[LiHCOO])/(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[H2O])/(Δt) = -1/3 (Δ[Li2SO3])/(Δt) = -1/2 (Δ[Cu(HCOO)2])/(Δt) = 1/2 (Δ[LiHSO3])/(Δt) = (Δ[(CuOH)2SO3])/(Δt) = 1/4 (Δ[LiHCOO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2O + Li2SO3 + Cu(HCOO)2 ⟶ LiHSO3 + (CuOH)2SO3 + LiHCOO 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 H_2O + 3 Li2SO3 + 2 Cu(HCOO)2 ⟶ 2 LiHSO3 + (CuOH)2SO3 + 4 LiHCOO 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_2O | 2 | -2 Li2SO3 | 3 | -3 Cu(HCOO)2 | 2 | -2 LiHSO3 | 2 | 2 (CuOH)2SO3 | 1 | 1 LiHCOO | 4 | 4 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_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Li2SO3 | 3 | -3 | -1/3 (Δ[Li2SO3])/(Δt) Cu(HCOO)2 | 2 | -2 | -1/2 (Δ[Cu(HCOO)2])/(Δt) LiHSO3 | 2 | 2 | 1/2 (Δ[LiHSO3])/(Δt) (CuOH)2SO3 | 1 | 1 | (Δ[(CuOH)2SO3])/(Δt) LiHCOO | 4 | 4 | 1/4 (Δ[LiHCOO])/(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[H2O])/(Δt) = -1/3 (Δ[Li2SO3])/(Δt) = -1/2 (Δ[Cu(HCOO)2])/(Δt) = 1/2 (Δ[LiHSO3])/(Δt) = (Δ[(CuOH)2SO3])/(Δt) = 1/4 (Δ[LiHCOO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| water | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO formula | H_2O | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO Hill formula | H_2O | Li2O3S | C2H2CuO4 | HLiO3S | H2Cu2O5S | CHLiO2 name | water | | | | |
| water | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO formula | H_2O | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO Hill formula | H_2O | Li2O3S | C2H2CuO4 | HLiO3S | H2Cu2O5S | CHLiO2 name | water | | | | |

Substance properties

| water | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO molar mass | 18.015 g/mol | 93.9 g/mol | 153.58 g/mol | 88 g/mol | 241.16 g/mol | 51.96 g/mol phase | liquid (at STP) | | | | | melting point | 0 °C | | | | | boiling point | 99.9839 °C | | | | | density | 1 g/cm^3 | | | | | surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | | odor | odorless | | | | |
| water | Li2SO3 | Cu(HCOO)2 | LiHSO3 | (CuOH)2SO3 | LiHCOO molar mass | 18.015 g/mol | 93.9 g/mol | 153.58 g/mol | 88 g/mol | 241.16 g/mol | 51.96 g/mol phase | liquid (at STP) | | | | | melting point | 0 °C | | | | | boiling point | 99.9839 °C | | | | | density | 1 g/cm^3 | | | | | surface tension | 0.0728 N/m | | | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | | | | odor | odorless | | | | |

Units

Random Queries

phase of [bis(trifluoroacetoxy)iodo]benzene vs calcium iodide
CAS number of heavy molecules
name of krypton(II) cation vs xenon(VIII) cation
empirical formula of sodium hypochlorite vs vanadium(V) fluoride
d-spacing of minguzzite
volume of 12 kg of potassium
alternate names of antimony vs indium
oxygen vs hydrogen
isopropyllithium
chemical uses of rifaximin vs 3-hydroxy-3-methylglutaric acid