Input interpretation
![NH4ClNaOH ⟶ NH3H2ONaCl](../image_source/c0c84ab09185caeb241fcc114e878cb7.png)
NH4ClNaOH ⟶ NH3H2ONaCl
Balanced equation
![Balance the chemical equation algebraically: NH4ClNaOH ⟶ NH3H2ONaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH4ClNaOH ⟶ c_2 NH3H2ONaCl Set the number of atoms in the reactants equal to the number of atoms in the products for N, H, Cl, Na and O: N: | c_1 = c_2 H: | 5 c_1 = 5 c_2 Cl: | c_1 = c_2 Na: | c_1 = c_2 O: | c_1 = 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: | | NH4ClNaOH ⟶ NH3H2ONaCl](../image_source/b91a9615b894fc86e0ca70bc1dbb0608.png)
Balance the chemical equation algebraically: NH4ClNaOH ⟶ NH3H2ONaCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH4ClNaOH ⟶ c_2 NH3H2ONaCl Set the number of atoms in the reactants equal to the number of atoms in the products for N, H, Cl, Na and O: N: | c_1 = c_2 H: | 5 c_1 = 5 c_2 Cl: | c_1 = c_2 Na: | c_1 = c_2 O: | c_1 = 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: | | NH4ClNaOH ⟶ NH3H2ONaCl
Structures
![NH4ClNaOH ⟶ NH3H2ONaCl](../image_source/75f3da090a794c7d53a2fbb86ce43cdc.png)
NH4ClNaOH ⟶ NH3H2ONaCl
Names
![NH4ClNaOH ⟶ NH3H2ONaCl](../image_source/95035bbc1dcd07ecca483f4af0d12c46.png)
NH4ClNaOH ⟶ NH3H2ONaCl
Equilibrium constant
![Construct the equilibrium constant, K, expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH4ClNaOH | 1 | -1 | ([NH4ClNaOH])^(-1) NH3H2ONaCl | 1 | 1 | [NH3H2ONaCl] 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 = ([NH4ClNaOH])^(-1) [NH3H2ONaCl] = ([NH3H2ONaCl])/([NH4ClNaOH])](../image_source/0258487d1f798c7f77cf04166ba68429.png)
Construct the equilibrium constant, K, expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NH4ClNaOH | 1 | -1 | ([NH4ClNaOH])^(-1) NH3H2ONaCl | 1 | 1 | [NH3H2ONaCl] 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 = ([NH4ClNaOH])^(-1) [NH3H2ONaCl] = ([NH3H2ONaCl])/([NH4ClNaOH])
Rate of reaction
![Construct the rate of reaction expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 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 NH4ClNaOH | 1 | -1 | -(Δ[NH4ClNaOH])/(Δt) NH3H2ONaCl | 1 | 1 | (Δ[NH3H2ONaCl])/(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[NH4ClNaOH])/(Δt) = (Δ[NH3H2ONaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/8a6550541ca08801e032e596c9147ccc.png)
Construct the rate of reaction expression for: NH4ClNaOH ⟶ NH3H2ONaCl 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: NH4ClNaOH ⟶ NH3H2ONaCl 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 NH4ClNaOH | 1 | -1 NH3H2ONaCl | 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 NH4ClNaOH | 1 | -1 | -(Δ[NH4ClNaOH])/(Δt) NH3H2ONaCl | 1 | 1 | (Δ[NH3H2ONaCl])/(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[NH4ClNaOH])/(Δt) = (Δ[NH3H2ONaCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| NH4ClNaOH | NH3H2ONaCl formula | NH4ClNaOH | NH3H2ONaCl Hill formula | H5ClNNaO | H5ClNNaO](../image_source/3b13e1934069d0ef56b5081b3b13fbcc.png)
| NH4ClNaOH | NH3H2ONaCl formula | NH4ClNaOH | NH3H2ONaCl Hill formula | H5ClNNaO | H5ClNNaO
Substance properties
![| NH4ClNaOH | NH3H2ONaCl molar mass | 93.49 g/mol | 93.49 g/mol](../image_source/84bc49d7661e92b641e0b1949977fb90.png)
| NH4ClNaOH | NH3H2ONaCl molar mass | 93.49 g/mol | 93.49 g/mol
Units