Search

HNO3 + S = H2SO4 + H2 + NO2

Input interpretation

HNO_3 nitric acid + S mixed sulfur ⟶ H_2SO_4 sulfuric acid + H_2 hydrogen + NO_2 nitrogen dioxide
HNO_3 nitric acid + S mixed sulfur ⟶ H_2SO_4 sulfuric acid + H_2 hydrogen + NO_2 nitrogen dioxide

Balanced equation

Balance the chemical equation algebraically: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 S ⟶ c_3 H_2SO_4 + c_4 H_2 + c_5 NO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and S: H: | c_1 = 2 c_3 + 2 c_4 N: | c_1 = c_5 O: | 3 c_1 = 4 c_3 + 2 c_5 S: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_2
Balance the chemical equation algebraically: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 S ⟶ c_3 H_2SO_4 + c_4 H_2 + c_5 NO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and S: H: | c_1 = 2 c_3 + 2 c_4 N: | c_1 = c_5 O: | 3 c_1 = 4 c_3 + 2 c_5 S: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 4 c_2 = 1 c_3 = 1 c_4 = 1 c_5 = 4 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

nitric acid + mixed sulfur ⟶ sulfuric acid + hydrogen + nitrogen dioxide
nitric acid + mixed sulfur ⟶ sulfuric acid + hydrogen + nitrogen dioxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_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: 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_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 | 4 | -4 S | 1 | -1 H_2SO_4 | 1 | 1 H_2 | 1 | 1 NO_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 | 4 | -4 | ([HNO3])^(-4) S | 1 | -1 | ([S])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] H_2 | 1 | 1 | [H2] NO_2 | 4 | 4 | ([NO2])^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])^(-4) ([S])^(-1) [H2SO4] [H2] ([NO2])^4 = ([H2SO4] [H2] ([NO2])^4)/(([HNO3])^4 [S])
Construct the equilibrium constant, K, expression for: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_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: 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_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 | 4 | -4 S | 1 | -1 H_2SO_4 | 1 | 1 H_2 | 1 | 1 NO_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 | 4 | -4 | ([HNO3])^(-4) S | 1 | -1 | ([S])^(-1) H_2SO_4 | 1 | 1 | [H2SO4] H_2 | 1 | 1 | [H2] NO_2 | 4 | 4 | ([NO2])^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])^(-4) ([S])^(-1) [H2SO4] [H2] ([NO2])^4 = ([H2SO4] [H2] ([NO2])^4)/(([HNO3])^4 [S])

Rate of reaction

Construct the rate of reaction expression for: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_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: 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_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 | 4 | -4 S | 1 | -1 H_2SO_4 | 1 | 1 H_2 | 1 | 1 NO_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 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) S | 1 | -1 | -(Δ[S])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) NO_2 | 4 | 4 | 1/4 (Δ[NO2])/(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 = -1/4 (Δ[HNO3])/(Δt) = -(Δ[S])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[H2])/(Δt) = 1/4 (Δ[NO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HNO_3 + S ⟶ H_2SO_4 + H_2 + NO_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: 4 HNO_3 + S ⟶ H_2SO_4 + H_2 + 4 NO_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 | 4 | -4 S | 1 | -1 H_2SO_4 | 1 | 1 H_2 | 1 | 1 NO_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 | 4 | -4 | -1/4 (Δ[HNO3])/(Δt) S | 1 | -1 | -(Δ[S])/(Δt) H_2SO_4 | 1 | 1 | (Δ[H2SO4])/(Δt) H_2 | 1 | 1 | (Δ[H2])/(Δt) NO_2 | 4 | 4 | 1/4 (Δ[NO2])/(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 = -1/4 (Δ[HNO3])/(Δt) = -(Δ[S])/(Δt) = (Δ[H2SO4])/(Δt) = (Δ[H2])/(Δt) = 1/4 (Δ[NO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide formula | HNO_3 | S | H_2SO_4 | H_2 | NO_2 Hill formula | HNO_3 | S | H_2O_4S | H_2 | NO_2 name | nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide IUPAC name | nitric acid | sulfur | sulfuric acid | molecular hydrogen | Nitrogen dioxide
| nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide formula | HNO_3 | S | H_2SO_4 | H_2 | NO_2 Hill formula | HNO_3 | S | H_2O_4S | H_2 | NO_2 name | nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide IUPAC name | nitric acid | sulfur | sulfuric acid | molecular hydrogen | Nitrogen dioxide

Substance properties

| nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide molar mass | 63.012 g/mol | 32.06 g/mol | 98.07 g/mol | 2.016 g/mol | 46.005 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | gas (at STP) melting point | -41.6 °C | 112.8 °C | 10.371 °C | -259.2 °C | -11 °C boiling point | 83 °C | 444.7 °C | 279.6 °C | -252.8 °C | 21 °C density | 1.5129 g/cm^3 | 2.07 g/cm^3 | 1.8305 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 0.00188 g/cm^3 (at 25 °C) solubility in water | miscible | | very soluble | | reacts surface tension | | | 0.0735 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 8.9×10^-6 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) odor | | | odorless | odorless |
| nitric acid | mixed sulfur | sulfuric acid | hydrogen | nitrogen dioxide molar mass | 63.012 g/mol | 32.06 g/mol | 98.07 g/mol | 2.016 g/mol | 46.005 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | gas (at STP) | gas (at STP) melting point | -41.6 °C | 112.8 °C | 10.371 °C | -259.2 °C | -11 °C boiling point | 83 °C | 444.7 °C | 279.6 °C | -252.8 °C | 21 °C density | 1.5129 g/cm^3 | 2.07 g/cm^3 | 1.8305 g/cm^3 | 8.99×10^-5 g/cm^3 (at 0 °C) | 0.00188 g/cm^3 (at 25 °C) solubility in water | miscible | | very soluble | | reacts surface tension | | | 0.0735 N/m | | dynamic viscosity | 7.6×10^-4 Pa s (at 25 °C) | | 0.021 Pa s (at 25 °C) | 8.9×10^-6 Pa s (at 25 °C) | 4.02×10^-4 Pa s (at 25 °C) odor | | | odorless | odorless |

Units

Random Queries

boiling point of 2-(1,3-dioxan-2-yl)ethylzinc bromide
IUPAC name of barium carbonate vs potassium hexachloroplatinate
electronegativity of hydrogen vs beryllium
CAS number of 1,4-bis(trifluoromethyl)benzene-13 C6
CAS number of 2,2-difluoro-5-formylbenzodioxole vs 2-chloro-5-fluoropyridine
atomic mass of sulfur vs bromine
ions of manganese hydroxide vs cobaltous carbonate
molar mass of hexachloroselenate(IV) anion
molar mass of borate anion vs phosphate anion
atomic number of thallium