Search

H2S + Ni(NO3)2 = HNO3 + NiS

Input interpretation

H_2S hydrogen sulfide + Ni(NO_3)_2 nickel(II) nitrate ⟶ HNO_3 nitric acid + SNi nickel(II) sulfide
H_2S hydrogen sulfide + Ni(NO_3)_2 nickel(II) nitrate ⟶ HNO_3 nitric acid + SNi nickel(II) sulfide

Balanced equation

Balance the chemical equation algebraically: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 Ni(NO_3)_2 ⟶ c_3 HNO_3 + c_4 SNi Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, N, Ni and O: H: | 2 c_1 = c_3 S: | c_1 = c_4 N: | 2 c_2 = c_3 Ni: | c_2 = c_4 O: | 6 c_2 = 3 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 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi
Balance the chemical equation algebraically: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2S + c_2 Ni(NO_3)_2 ⟶ c_3 HNO_3 + c_4 SNi Set the number of atoms in the reactants equal to the number of atoms in the products for H, S, N, Ni and O: H: | 2 c_1 = c_3 S: | c_1 = c_4 N: | 2 c_2 = c_3 Ni: | c_2 = c_4 O: | 6 c_2 = 3 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 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen sulfide + nickel(II) nitrate ⟶ nitric acid + nickel(II) sulfide
hydrogen sulfide + nickel(II) nitrate ⟶ nitric acid + nickel(II) sulfide

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi 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: H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi 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_2S | 1 | -1 Ni(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 SNi | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 1 | -1 | ([H2S])^(-1) Ni(NO_3)_2 | 1 | -1 | ([Ni(NO3)2])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 SNi | 1 | 1 | [S1Ni1] 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 = ([H2S])^(-1) ([Ni(NO3)2])^(-1) ([HNO3])^2 [S1Ni1] = (([HNO3])^2 [S1Ni1])/([H2S] [Ni(NO3)2])
Construct the equilibrium constant, K, expression for: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi 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: H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi 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_2S | 1 | -1 Ni(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 SNi | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2S | 1 | -1 | ([H2S])^(-1) Ni(NO_3)_2 | 1 | -1 | ([Ni(NO3)2])^(-1) HNO_3 | 2 | 2 | ([HNO3])^2 SNi | 1 | 1 | [S1Ni1] 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 = ([H2S])^(-1) ([Ni(NO3)2])^(-1) ([HNO3])^2 [S1Ni1] = (([HNO3])^2 [S1Ni1])/([H2S] [Ni(NO3)2])

Rate of reaction

Construct the rate of reaction expression for: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi 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: H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi 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_2S | 1 | -1 Ni(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 SNi | 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 H_2S | 1 | -1 | -(Δ[H2S])/(Δt) Ni(NO_3)_2 | 1 | -1 | -(Δ[Ni(NO3)2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) SNi | 1 | 1 | (Δ[S1Ni1])/(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[H2S])/(Δt) = -(Δ[Ni(NO3)2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[S1Ni1])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_2S + Ni(NO_3)_2 ⟶ HNO_3 + SNi 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: H_2S + Ni(NO_3)_2 ⟶ 2 HNO_3 + SNi 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_2S | 1 | -1 Ni(NO_3)_2 | 1 | -1 HNO_3 | 2 | 2 SNi | 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 H_2S | 1 | -1 | -(Δ[H2S])/(Δt) Ni(NO_3)_2 | 1 | -1 | -(Δ[Ni(NO3)2])/(Δt) HNO_3 | 2 | 2 | 1/2 (Δ[HNO3])/(Δt) SNi | 1 | 1 | (Δ[S1Ni1])/(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[H2S])/(Δt) = -(Δ[Ni(NO3)2])/(Δt) = 1/2 (Δ[HNO3])/(Δt) = (Δ[S1Ni1])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide formula | H_2S | Ni(NO_3)_2 | HNO_3 | SNi Hill formula | H_2S | N_2NiO_6 | HNO_3 | NiS name | hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide IUPAC name | hydrogen sulfide | nickel(+2) dinitrate | nitric acid | sulfanylidenenickel
| hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide formula | H_2S | Ni(NO_3)_2 | HNO_3 | SNi Hill formula | H_2S | N_2NiO_6 | HNO_3 | NiS name | hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide IUPAC name | hydrogen sulfide | nickel(+2) dinitrate | nitric acid | sulfanylidenenickel

Substance properties

| hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide molar mass | 34.08 g/mol | 182.7 g/mol | 63.012 g/mol | 90.75 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | melting point | -85 °C | 57 °C | -41.6 °C | boiling point | -60 °C | 137 °C | 83 °C | density | 0.001393 g/cm^3 (at 25 °C) | 1.77 g/cm^3 | 1.5129 g/cm^3 | solubility in water | | | miscible | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 7.6×10^-4 Pa s (at 25 °C) |
| hydrogen sulfide | nickel(II) nitrate | nitric acid | nickel(II) sulfide molar mass | 34.08 g/mol | 182.7 g/mol | 63.012 g/mol | 90.75 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | melting point | -85 °C | 57 °C | -41.6 °C | boiling point | -60 °C | 137 °C | 83 °C | density | 0.001393 g/cm^3 (at 25 °C) | 1.77 g/cm^3 | 1.5129 g/cm^3 | solubility in water | | | miscible | dynamic viscosity | 1.239×10^-5 Pa s (at 25 °C) | | 7.6×10^-4 Pa s (at 25 °C) |

Units

Random Queries

freezing point of 5-chloro-7-iodo-8-quinolinol
lethal dosage of non-polar solvents
NFPA reactivity rating of 1-bromo-3-methyl-2-butene
handwritten style what solvents are miscible in acetone
atomic radius of non-metallic elements
phase of rubidium hydroxide vs potassium hydroxide
formula of erythorbic acid vs (4 S-trans)-2,2-dimethyl-α,α,α',α'-tetra(2-naphthyl)-1,3-dioxolane-4,5-dimethanol
melting point of neodymium(II) chloride
net ionic charge of hydrogen carbonate anion vs permanganate anion
ion class of chromium(III) cation