Search

HNO3 + Be = H2O + NH4NO3 + Be(NO3)2

Input interpretation

HNO_3 nitric acid + Be beryllium ⟶ H_2O water + NH_4NO_3 ammonium nitrate + Be(NO_3)_2 beryllium nitrate
HNO_3 nitric acid + Be beryllium ⟶ H_2O water + NH_4NO_3 ammonium nitrate + Be(NO_3)_2 beryllium nitrate

Balanced equation

Balance the chemical equation algebraically: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Be ⟶ c_3 H_2O + c_4 NH_4NO_3 + c_5 Be(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Be: H: | c_1 = 2 c_3 + 4 c_4 N: | c_1 = 2 c_4 + 2 c_5 O: | 3 c_1 = c_3 + 3 c_4 + 6 c_5 Be: | c_2 = c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 4 c_3 = 3 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2
Balance the chemical equation algebraically: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Be ⟶ c_3 H_2O + c_4 NH_4NO_3 + c_5 Be(NO_3)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Be: H: | c_1 = 2 c_3 + 4 c_4 N: | c_1 = 2 c_4 + 2 c_5 O: | 3 c_1 = c_3 + 3 c_4 + 6 c_5 Be: | c_2 = c_5 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 10 c_2 = 4 c_3 = 3 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + beryllium ⟶ water + ammonium nitrate + beryllium nitrate
nitric acid + beryllium ⟶ water + ammonium nitrate + beryllium nitrate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 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: 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2 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 HNO_3 | 10 | -10 Be | 4 | -4 H_2O | 3 | 3 NH_4NO_3 | 1 | 1 Be(NO_3)_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) Be | 4 | -4 | ([Be])^(-4) H_2O | 3 | 3 | ([H2O])^3 NH_4NO_3 | 1 | 1 | [NH4NO3] Be(NO_3)_2 | 4 | 4 | ([Be(NO3)2])^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 = ([HNO3])^(-10) ([Be])^(-4) ([H2O])^3 [NH4NO3] ([Be(NO3)2])^4 = (([H2O])^3 [NH4NO3] ([Be(NO3)2])^4)/(([HNO3])^10 ([Be])^4)
Construct the equilibrium constant, K, expression for: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 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: 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2 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 HNO_3 | 10 | -10 Be | 4 | -4 H_2O | 3 | 3 NH_4NO_3 | 1 | 1 Be(NO_3)_2 | 4 | 4 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 10 | -10 | ([HNO3])^(-10) Be | 4 | -4 | ([Be])^(-4) H_2O | 3 | 3 | ([H2O])^3 NH_4NO_3 | 1 | 1 | [NH4NO3] Be(NO_3)_2 | 4 | 4 | ([Be(NO3)2])^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 = ([HNO3])^(-10) ([Be])^(-4) ([H2O])^3 [NH4NO3] ([Be(NO3)2])^4 = (([H2O])^3 [NH4NO3] ([Be(NO3)2])^4)/(([HNO3])^10 ([Be])^4)

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 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: 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2 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 HNO_3 | 10 | -10 Be | 4 | -4 H_2O | 3 | 3 NH_4NO_3 | 1 | 1 Be(NO_3)_2 | 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 HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) Be | 4 | -4 | -1/4 (Δ[Be])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NH_4NO_3 | 1 | 1 | (Δ[NH4NO3])/(Δt) Be(NO_3)_2 | 4 | 4 | 1/4 (Δ[Be(NO3)2])/(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 = -1/10 (Δ[HNO3])/(Δt) = -1/4 (Δ[Be])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NH4NO3])/(Δt) = 1/4 (Δ[Be(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + Be ⟶ H_2O + NH_4NO_3 + Be(NO_3)_2 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: 10 HNO_3 + 4 Be ⟶ 3 H_2O + NH_4NO_3 + 4 Be(NO_3)_2 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 HNO_3 | 10 | -10 Be | 4 | -4 H_2O | 3 | 3 NH_4NO_3 | 1 | 1 Be(NO_3)_2 | 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 HNO_3 | 10 | -10 | -1/10 (Δ[HNO3])/(Δt) Be | 4 | -4 | -1/4 (Δ[Be])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) NH_4NO_3 | 1 | 1 | (Δ[NH4NO3])/(Δt) Be(NO_3)_2 | 4 | 4 | 1/4 (Δ[Be(NO3)2])/(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 = -1/10 (Δ[HNO3])/(Δt) = -1/4 (Δ[Be])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[NH4NO3])/(Δt) = 1/4 (Δ[Be(NO3)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate formula | HNO_3 | Be | H_2O | NH_4NO_3 | Be(NO_3)_2 Hill formula | HNO_3 | Be | H_2O | H_4N_2O_3 | BeN_2O_6 name | nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate IUPAC name | nitric acid | beryllium | water | | beryllium dinitrate
| nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate formula | HNO_3 | Be | H_2O | NH_4NO_3 | Be(NO_3)_2 Hill formula | HNO_3 | Be | H_2O | H_4N_2O_3 | BeN_2O_6 name | nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate IUPAC name | nitric acid | beryllium | water | | beryllium dinitrate

Substance properties

| nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate molar mass | 63.012 g/mol | 9.0121831 g/mol | 18.015 g/mol | 80.04 g/mol | 133.02 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | -41.6 °C | 1278 °C | 0 °C | 169 °C | 1287.2 °C boiling point | 83 °C | 2970 °C | 99.9839 °C | 210 °C | density | 1.5129 g/cm^3 | 1.85 g/cm^3 | 1 g/cm^3 | 1.73 g/cm^3 | 1.2 g/cm^3 solubility in water | miscible | insoluble | | | very soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |
| nitric acid | beryllium | water | ammonium nitrate | beryllium nitrate molar mass | 63.012 g/mol | 9.0121831 g/mol | 18.015 g/mol | 80.04 g/mol | 133.02 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | -41.6 °C | 1278 °C | 0 °C | 169 °C | 1287.2 °C boiling point | 83 °C | 2970 °C | 99.9839 °C | 210 °C | density | 1.5129 g/cm^3 | 1.85 g/cm^3 | 1 g/cm^3 | 1.73 g/cm^3 | 1.2 g/cm^3 solubility in water | miscible | insoluble | | | very soluble surface tension | | | 0.0728 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |

Units

Random Queries

electron configuration titanium
formula of sulfonium ylide functional group vs sulfoxonium ylide functional group
HClO + MnS = HCl + MnSO4
CAS number of carbon vs nitrogen
ion class of orthovanadate anion
chemical types of lanthanum hexaboride
lead(IV) ions
alternate names of buckminsterfullerene vs vanadium
selenious acid vs potassium persulfate
density of kadyrelite vs rorisite