Input interpretation
![H_2O water + Cs cesium ⟶ H_2 hydrogen + CsOH cesium hydroxide](../image_source/fa83a7be93d88ef487aa047358832f81.png)
H_2O water + Cs cesium ⟶ H_2 hydrogen + CsOH cesium hydroxide
Balanced equation
![Balance the chemical equation algebraically: H_2O + Cs ⟶ H_2 + CsOH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cs ⟶ c_3 H_2 + c_4 CsOH Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Cs: H: | 2 c_1 = 2 c_3 + c_4 O: | c_1 = c_4 Cs: | c_2 = c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 Cs ⟶ H_2 + 2 CsOH](../image_source/a2d3708224970e6b71c4e1fd46fa10d7.png)
Balance the chemical equation algebraically: H_2O + Cs ⟶ H_2 + CsOH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2O + c_2 Cs ⟶ c_3 H_2 + c_4 CsOH Set the number of atoms in the reactants equal to the number of atoms in the products for H, O and Cs: H: | 2 c_1 = 2 c_3 + c_4 O: | c_1 = c_4 Cs: | c_2 = c_4 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_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_2O + 2 Cs ⟶ H_2 + 2 CsOH
Structures
![+ ⟶ +](../image_source/3f63b7e4520dfed80de03242d3b09354.png)
+ ⟶ +
Names
![water + cesium ⟶ hydrogen + cesium hydroxide](../image_source/2d151ffa3f3c4850c70f841c035d9e76.png)
water + cesium ⟶ hydrogen + cesium hydroxide
Reaction thermodynamics
Enthalpy
![| water | cesium | hydrogen | cesium hydroxide molecular enthalpy | -285.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -416.2 kJ/mol total enthalpy | -571.7 kJ/mol | 0 kJ/mol | 0 kJ/mol | -832.4 kJ/mol | H_initial = -571.7 kJ/mol | | H_final = -832.4 kJ/mol | ΔH_rxn^0 | -832.4 kJ/mol - -571.7 kJ/mol = -260.7 kJ/mol (exothermic) | | |](../image_source/30161a3292fee9ec40d8e68bfdd4cd95.png)
| water | cesium | hydrogen | cesium hydroxide molecular enthalpy | -285.8 kJ/mol | 0 kJ/mol | 0 kJ/mol | -416.2 kJ/mol total enthalpy | -571.7 kJ/mol | 0 kJ/mol | 0 kJ/mol | -832.4 kJ/mol | H_initial = -571.7 kJ/mol | | H_final = -832.4 kJ/mol | ΔH_rxn^0 | -832.4 kJ/mol - -571.7 kJ/mol = -260.7 kJ/mol (exothermic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2O + Cs ⟶ H_2 + CsOH 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 + 2 Cs ⟶ H_2 + 2 CsOH 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 Cs | 2 | -2 H_2 | 1 | 1 CsOH | 2 | 2 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) Cs | 2 | -2 | ([Cs])^(-2) H_2 | 1 | 1 | [H2] CsOH | 2 | 2 | ([CsHO])^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 = ([H2O])^(-2) ([Cs])^(-2) [H2] ([CsHO])^2 = ([H2] ([CsHO])^2)/(([H2O])^2 ([Cs])^2)](../image_source/360e4889156c8aebc3f7e4ed68b35672.png)
Construct the equilibrium constant, K, expression for: H_2O + Cs ⟶ H_2 + CsOH 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 + 2 Cs ⟶ H_2 + 2 CsOH 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 Cs | 2 | -2 H_2 | 1 | 1 CsOH | 2 | 2 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) Cs | 2 | -2 | ([Cs])^(-2) H_2 | 1 | 1 | [H2] CsOH | 2 | 2 | ([CsHO])^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 = ([H2O])^(-2) ([Cs])^(-2) [H2] ([CsHO])^2 = ([H2] ([CsHO])^2)/(([H2O])^2 ([Cs])^2)
Rate of reaction
![Construct the rate of reaction expression for: H_2O + Cs ⟶ H_2 + CsOH 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 + 2 Cs ⟶ H_2 + 2 CsOH 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 Cs | 2 | -2 H_2 | 1 | 1 CsOH | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Cs | 2 | -2 | -1/2 (Δ[Cs])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) CsOH | 2 | 2 | 1/2 (Δ[CsHO])/(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) = -1/2 (Δ[Cs])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[CsHO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/3913df304a2750702e21b6359a660d0a.png)
Construct the rate of reaction expression for: H_2O + Cs ⟶ H_2 + CsOH 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 + 2 Cs ⟶ H_2 + 2 CsOH 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 Cs | 2 | -2 H_2 | 1 | 1 CsOH | 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 H_2O | 2 | -2 | -1/2 (Δ[H2O])/(Δt) Cs | 2 | -2 | -1/2 (Δ[Cs])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) CsOH | 2 | 2 | 1/2 (Δ[CsHO])/(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) = -1/2 (Δ[Cs])/(Δt) = (Δ[H2])/(Δt) = 1/2 (Δ[CsHO])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| water | cesium | hydrogen | cesium hydroxide formula | H_2O | Cs | H_2 | CsOH Hill formula | H_2O | Cs | H_2 | CsHO name | water | cesium | hydrogen | cesium hydroxide IUPAC name | water | cesium | molecular hydrogen | cesium;hydroxide](../image_source/e64ad3db4a15106e6daec1e445e1482e.png)
| water | cesium | hydrogen | cesium hydroxide formula | H_2O | Cs | H_2 | CsOH Hill formula | H_2O | Cs | H_2 | CsHO name | water | cesium | hydrogen | cesium hydroxide IUPAC name | water | cesium | molecular hydrogen | cesium;hydroxide
Substance properties
![| water | cesium | hydrogen | cesium hydroxide molar mass | 18.015 g/mol | 132.90545196 g/mol | 2.016 g/mol | 149.912 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | 28.5 °C | -259.2 °C | 338.85 °C boiling point | 99.9839 °C | 705 °C | -252.8 °C | density | 1 g/cm^3 | 1.873 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.72 g/cm^3 solubility in water | | decomposes | | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | | odorless |](../image_source/799c40909d8635228047e34f06702616.png)
| water | cesium | hydrogen | cesium hydroxide molar mass | 18.015 g/mol | 132.90545196 g/mol | 2.016 g/mol | 149.912 g/mol phase | liquid (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | 0 °C | 28.5 °C | -259.2 °C | 338.85 °C boiling point | 99.9839 °C | 705 °C | -252.8 °C | density | 1 g/cm^3 | 1.873 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 1.72 g/cm^3 solubility in water | | decomposes | | surface tension | 0.0728 N/m | | | dynamic viscosity | 8.9×10^-4 Pa s (at 25 °C) | | 8.9×10^-6 Pa s (at 25 °C) | odor | odorless | | odorless |
Units