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3 years ago

Why does SO2 and water make H2SO3 and NOT H2SO4?

2 answers:

3 0

SO₂ is a polar molecule and dissolves in water to form H₂SO₃; however, it does not have the ability to break the H-O bond in water and isolate an Oxygen atom to form H₂SO₄. This is why in the production of Sulfuric acid via the contact process, SO₂ is converted into SO₃ first.

Anna71 [15]3 years ago

3 0

SO2+H2O = H2SO3

To get H2SO4,
SO2 must be oxidized to form SO3, Sulfur tri-oxide
2SO2+ O2= 2SO3 SO3 can the dissolve in water to form acid rain:

SO3 + H2O = H2SO4

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If 10.0g of powdered iron is heated with 10.0g of sulfur in an open crucible, what is the mass of iron (II) sulfide that is form

Ugo [173]

Answer:

See Explanation

Explanation:

8Fe + S₈ => 8FeS

Given: 10g 10g

moles 10g/56g/mol 10g/256g/mol

= 0.179mol Fe = 0.039mol S₈

Reduce => divide mole values by respective coefficients; smaller value is Limiting Reactant.

0.179/8 = 0.022 0.039/1 = 0.039

=> Fe is limiting reactant

8Fe + S₈ => 8FeS

Given: 10g/56g/mol 10g/256g/mol

= 0.179mol = 0.039 mol 0.179mol FeS produced

1/8(0.179)mol S₈ used (coefficients are equal,

= 0.022 mol S₈ used => moles Fe = moles FeS)

= (0.039 - 0.022)mol S₈ = 0.179mol FeS

remains in excess =(0.179mol)(88g/mol)

= 0.0166 mol S₈ (excess) = 15.8 g FeS

= (0.0166mol)(256g/mol) (Theoretical Yield)

= 4.26g S₈ in excess

7 0

3 years ago

Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas well

Harlamova29_29 [7]

Answer: Rate of production of Sulfur dioxide is 0.15kg/s to 2 significant digits

Note: The question is incomplete. The complete question is as follows:

Most of the used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 198. liters per second of dioxygen are consumed when the reaction is run at 186. °C and 0.69 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.

Explanation:

The balanced equation of the reaction between hydrogen sulfide gas and dioxygen gas to produce sulfur dioxide and water is as follows:

2H₂S(g) + 3O₂(g) ---> 2SO₂(g) + 2H₂O(g)

From the equation above, 3 moles of dioxide yields 2 moles of sulfur dioxide.

Using the ideal gas equation to determine the number of moles of dioxygen present in 198 litres of the gas at 186. °C and 0.69 atm;

PV = nRT,

where P = 0.69atm, V = 198Litres, R (molar gas constant) = 0.082atmLK⁻¹mol⁻¹, T = 186. °C = 459K

n = PV/RT

n = 0.69*198*/(0.082*459)

n = 3.63moles of dioxygen

Therefore, 3.63 moles of dioxygen are consumed per second

Using the mole ratio from the equation of reaction,

number of moles of sulfur dioxide produced will be 3.63moles * 2/3 = 2.42moles

Therefore, the number of moles of sulfur dioxide consumed is 2.42 moles per second.

Converting to kilograms per second,

1 mole of sulfur dioxide weighs 64g (molar mass of sulfur dioxide)

2.42 moles weighs 2.42*64g =154.88g or 0.15488Kg which is approximately 0.15Kg

Therefore, rate of production of Sulfur dioxide is 0.15kg/s to 2 significant digits

8 0

3 years ago

Suppose of nickel(II) chloride is dissolved in of a aqueous solution of potassium carbonate. Calculate the final molarity of chl

stich3 [128]

Answer: Molarity of chloride anion = 0.32 M

Note: the question is missing some values. The full question is given below;

Suppose 7.26 g of nickel(II) chloride is dissolved in 350 mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

Explanation:

Molarity or molar concentration is the number of moles (mol) of component per volume (liters) concentration of solution in mol/L or M

The mass of nickel (II) chloride is 7.26 g.

The volume of potassium carbonate is 350 mL = 0.35 L

The molarity of potassium carbonate solution is 0.50 M

The reaction of nickel (II) chloride and potassium carbonate is given below.

NiCl₂(aq) + KCO₃(aq) --------> KCl(aq) +NiCO₃(s)

The dissociation of nickel (II) chloride is given below.

NiCl₂ -----> Ni²⁺ + 2Cl⁻

The molar mass of nickel (II) chloride is 129.6 g/mol

The moles of nickel (II) chloride can be calculated by the formula given below;

No of moles = mass(g) / molar mass (g/mol)

No of moles = 7.26 / 129.6 = 0.056 moles

Therefore, molarity of NiCl₂ = 0.056 moles/ 0.35 L = 0.16 M

The molarity of 1 mole nickel (ii) chloride is 0.16 m and according to dissociation of nickel (II) chloride, 1 mole of nickel (II) chloride gives 2 moles of chloride anion.

Therefore, the molarity of chloride anion = 0.16 * 2 = 0.32 M

3 0

3 years ago

An experiment was conducted in order to determine the enthalpy change that occurs when 1.0 mole of ice at 0 degrees Celsius melt

Mashutka [201]

Answer: 1

Explanation:

6 0

3 years ago

A mixture of gases at a total pressure of 95 kPa contains N₂, CO₂, and O₂. The partial pressure of the CO₂ is 24 kPa and the par

Zinaida [17]

Answer:

23 kPa = Partial pressure O₂

Explanation:

In a mixture of gases, the sum of partial pressure of each gas that contains the mixture = Total pressure

Total pressure = Partial pressure N₂ + Partial pressure CO₂ + Partial pressure O₂

95 kPa = 48 kPa + 24 kPa + Partial pressure O₂

95 kPa - 48 kPa - 24 kPa = Partial pressure O₂

23 kPa = Partial pressure O₂

7 0

3 years ago