Input interpretation
![H_2CO_3 carbonic acid ⟶ H_2CO_3 carbonic acid](../image_source/3a3a504c4d845f8e1d7f6ca62e648927.png)
H_2CO_3 carbonic acid ⟶ H_2CO_3 carbonic acid
Balanced equation
![Balance the chemical equation algebraically: H_2CO_3 ⟶ H_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2CO_3 ⟶ c_2 H_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H and O: C: | c_1 = c_2 H: | 2 c_1 = 2 c_2 O: | 3 c_1 = 3 c_2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2CO_3 ⟶ H_2CO_3](../image_source/ffe0a1d8afdf285d13d5d29ed0e27556.png)
Balance the chemical equation algebraically: H_2CO_3 ⟶ H_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2CO_3 ⟶ c_2 H_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for C, H and O: C: | c_1 = c_2 H: | 2 c_1 = 2 c_2 O: | 3 c_1 = 3 c_2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2CO_3 ⟶ H_2CO_3
Structures
![⟶](../image_source/e842d860c8874714fd8a68ef742f218a.png)
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Names
![carbonic acid ⟶ carbonic acid](../image_source/1a1f4cfbaf741ea041cd902b31c2ce23.png)
carbonic acid ⟶ carbonic acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2CO_3 ⟶ H_2CO_3 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: H_2CO_3 ⟶ H_2CO_3 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_2CO_3 | 1 | -1 H_2CO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) H_2CO_3 | 1 | 1 | [H2CO3] 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 = ([H2CO3])^(-1) [H2CO3] = ([H2CO3])/([H2CO3])](../image_source/7da7aada4d0477891842bf7fedf248ce.png)
Construct the equilibrium constant, K, expression for: H_2CO_3 ⟶ H_2CO_3 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: H_2CO_3 ⟶ H_2CO_3 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_2CO_3 | 1 | -1 H_2CO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2CO_3 | 1 | -1 | ([H2CO3])^(-1) H_2CO_3 | 1 | 1 | [H2CO3] 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 = ([H2CO3])^(-1) [H2CO3] = ([H2CO3])/([H2CO3])
Rate of reaction
![Construct the rate of reaction expression for: H_2CO_3 ⟶ H_2CO_3 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: H_2CO_3 ⟶ H_2CO_3 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_2CO_3 | 1 | -1 H_2CO_3 | 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 H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) H_2CO_3 | 1 | 1 | (Δ[H2CO3])/(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 = -(Δ[H2CO3])/(Δt) = (Δ[H2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/27bec00529ad1081c7c81a1bbf86dca0.png)
Construct the rate of reaction expression for: H_2CO_3 ⟶ H_2CO_3 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: H_2CO_3 ⟶ H_2CO_3 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_2CO_3 | 1 | -1 H_2CO_3 | 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 H_2CO_3 | 1 | -1 | -(Δ[H2CO3])/(Δt) H_2CO_3 | 1 | 1 | (Δ[H2CO3])/(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 = -(Δ[H2CO3])/(Δt) = (Δ[H2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| carbonic acid | carbonic acid formula | H_2CO_3 | H_2CO_3 Hill formula | CH_2O_3 | CH_2O_3 name | carbonic acid | carbonic acid](../image_source/3d72993dc3aecdffd2bb69c4b06489a1.png)
| carbonic acid | carbonic acid formula | H_2CO_3 | H_2CO_3 Hill formula | CH_2O_3 | CH_2O_3 name | carbonic acid | carbonic acid
Substance properties
![| carbonic acid | carbonic acid molar mass | 62.024 g/mol | 62.024 g/mol](../image_source/4bfb8613e2596038a06f8f6f691eba71.png)
| carbonic acid | carbonic acid molar mass | 62.024 g/mol | 62.024 g/mol
Units