Input interpretation
![Cl_2 chlorine + Sr strontium ⟶ SrCl](../image_source/86b610524006ac7347254c4dbb4b4494.png)
Cl_2 chlorine + Sr strontium ⟶ SrCl
Balanced equation
![Balance the chemical equation algebraically: Cl_2 + Sr ⟶ SrCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Sr ⟶ c_3 SrCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Sr: Cl: | 2 c_1 = c_3 Sr: | c_2 = c_3 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 = 2 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 Sr ⟶ 2 SrCl](../image_source/b4be03a0786e7a9639cfb691d75983b4.png)
Balance the chemical equation algebraically: Cl_2 + Sr ⟶ SrCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Cl_2 + c_2 Sr ⟶ c_3 SrCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl and Sr: Cl: | 2 c_1 = c_3 Sr: | c_2 = c_3 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 = 2 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Cl_2 + 2 Sr ⟶ 2 SrCl
Structures
![+ ⟶ SrCl](../image_source/a10c4b3a674a590254ad8f16341ffcf0.png)
+ ⟶ SrCl
Names
![chlorine + strontium ⟶ SrCl](../image_source/a7255289e949736f78b1bd4738f7e6fc.png)
chlorine + strontium ⟶ SrCl
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Cl_2 + Sr ⟶ SrCl 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: Cl_2 + 2 Sr ⟶ 2 SrCl 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 Cl_2 | 1 | -1 Sr | 2 | -2 SrCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) Sr | 2 | -2 | ([Sr])^(-2) SrCl | 2 | 2 | ([SrCl])^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 = ([Cl2])^(-1) ([Sr])^(-2) ([SrCl])^2 = ([SrCl])^2/([Cl2] ([Sr])^2)](../image_source/9f604a31373a3f11a1f0d4df252d2dcb.png)
Construct the equilibrium constant, K, expression for: Cl_2 + Sr ⟶ SrCl 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: Cl_2 + 2 Sr ⟶ 2 SrCl 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 Cl_2 | 1 | -1 Sr | 2 | -2 SrCl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Cl_2 | 1 | -1 | ([Cl2])^(-1) Sr | 2 | -2 | ([Sr])^(-2) SrCl | 2 | 2 | ([SrCl])^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 = ([Cl2])^(-1) ([Sr])^(-2) ([SrCl])^2 = ([SrCl])^2/([Cl2] ([Sr])^2)
Rate of reaction
![Construct the rate of reaction expression for: Cl_2 + Sr ⟶ SrCl 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: Cl_2 + 2 Sr ⟶ 2 SrCl 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 Cl_2 | 1 | -1 Sr | 2 | -2 SrCl | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Sr | 2 | -2 | -1/2 (Δ[Sr])/(Δt) SrCl | 2 | 2 | 1/2 (Δ[SrCl])/(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[Cl2])/(Δt) = -1/2 (Δ[Sr])/(Δt) = 1/2 (Δ[SrCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/9a5df1d13fff331c471f6eebcfe81023.png)
Construct the rate of reaction expression for: Cl_2 + Sr ⟶ SrCl 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: Cl_2 + 2 Sr ⟶ 2 SrCl 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 Cl_2 | 1 | -1 Sr | 2 | -2 SrCl | 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 Cl_2 | 1 | -1 | -(Δ[Cl2])/(Δt) Sr | 2 | -2 | -1/2 (Δ[Sr])/(Δt) SrCl | 2 | 2 | 1/2 (Δ[SrCl])/(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[Cl2])/(Δt) = -1/2 (Δ[Sr])/(Δt) = 1/2 (Δ[SrCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| chlorine | strontium | SrCl formula | Cl_2 | Sr | SrCl Hill formula | Cl_2 | Sr | ClSr name | chlorine | strontium | IUPAC name | molecular chlorine | strontium |](../image_source/e4b33f88c593eac737d0b61a5bf4ab08.png)
| chlorine | strontium | SrCl formula | Cl_2 | Sr | SrCl Hill formula | Cl_2 | Sr | ClSr name | chlorine | strontium | IUPAC name | molecular chlorine | strontium |
Substance properties
![| chlorine | strontium | SrCl molar mass | 7.09×10^1 g/mol | 8.762×10^1 g/mol | 1.231×10^2 g/mol phase | gas (at STP) | solid (at STP) | melting point | -1.01×10^2 °C | 7.57×10^2 °C | boiling point | -3.4×10^1 °C | 1.384×10^3 °C | density | 3.214×10^-3 g/cm^3 (at 0×10^0 °C) | 2.6×10^0 g/cm^3 |](../image_source/a0fda20a6c0c80aefed3e3256039f8d9.png)
| chlorine | strontium | SrCl molar mass | 7.09×10^1 g/mol | 8.762×10^1 g/mol | 1.231×10^2 g/mol phase | gas (at STP) | solid (at STP) | melting point | -1.01×10^2 °C | 7.57×10^2 °C | boiling point | -3.4×10^1 °C | 1.384×10^3 °C | density | 3.214×10^-3 g/cm^3 (at 0×10^0 °C) | 2.6×10^0 g/cm^3 |
Units