Week 9 - Yields , atom economy and titration calculations

Last updated over 1 year ago

15 questions

Week 9 - Yields , atom economy and titration calculations

Last updated over 1 year ago

15 questions

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.
2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.
N2 + 3H2 → 2NH3

Copper(I) sulfide, Cu2S, is found in nature as the mineral chalcocite, which is a major component of copper ores. At high temperatures, chalcocite reacts with oxygen to produce copper metal and sulfur dioxide, SO2(g).
a. Formulate the balanced equation for the reaction of copper(I) sulfide with oxygen.
b. Determine the theoretical yield, in kg, of copper metal that could be obtained from 1.00 ton (1000 kg) of an ore that contains 75.3% of chalcocite. Assume that other components of the ore are unreactive.
c. Using your answer to part b, determine the percentage yield of copper metal if its practical yield is 506 kg.

Which of the following statements is most accurate?

Methane reacts with water to form hydrogen (desired product) and carbon monoxide:
CH4 + H2O → 3H2 + CO

a.Calculate the % atom economy for this reaction.

Suggest why the atom economy is so low even though 75% of the molecules produced are the desired product

Outline an issue with the undesired product in this reaction

Dimethyl carbonate, (CH3O)2CO, is a non-toxic and highly efficient “green” solvent.  
The synthesis of dimethyl carbonate is shown in  the following reaction:
4CH3OH(l) + 2CO(g) + O2(g) → 2(CH3O)2CO(l) + 2H2O(l)
Assume that the percentage yield of the reaction is 100%

Calculate the percentage atom economy

Dimethyl carbonate can be used to convert phenylamine, C6H5NH2(l), into N-methylphenylamine, C6H5NHCH3(l).
The by-products of this reaction are methanol, CH3OH(l), and carbon dioxide, CO2(g).

Formulate the balanced equation for this process and calculate its atom economy.

Suggest, by referring to the chemical equation in the previous question, how the atom economy of the synthesis of N-methylphenylamine can be improved.

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

1.25.0 cm3 of arsenic acid, H3AsO4, required 37.5 cm3 of 0.100 mol dm-3 sodium hydroxide for neutralisation.
3NaOH(aq) + H3AsO4(aq) →  Na3AsO4(aq) + 3H2O(l)

Find the concentration of the acid in mol dm-3

Find the concentration of the acid in g dm-3.

A 10.0 cm3 sample of a solution with unknown concentration of barium hydroxide, Ba(OH)2(aq), was titrated with 0.100 mol dm−3 hydrochloric acid, HCl(aq), in the presence of an acid–base indicator.
The colour change was observed when 11.7 cm3 of the standard solution was added.

Week 9 - Yields , atom economy and titration calculations

Week 9 - Yields , atom economy and titration calculations

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.
2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.
N2 + 3H2 → 2NH3

Which of the following statements is most accurate?

a.Calculate the % atom economy for this reaction.

Suggest why the atom economy is so low even though 75% of the molecules produced are the desired product

Outline an issue with the undesired product in this reaction

Calculate the percentage atom economy

Formulate the balanced equation for this process and calculate its atom economy.

Suggest, by referring to the chemical equation in the previous question, how the atom economy of the synthesis of N-methylphenylamine can be improved.

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

Find the concentration of the acid in mol dm-3

Find the concentration of the acid in g dm-3.

a.Formulate the balanced equation for the neutralization if the reaction products are barium chloride, BaCl2(aq), and water.

Determine the concentration, in mol dm−3, of barium hydroxide in the analysed solution.

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.
2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.
N2 + 3H2 → 2NH3

Which of the following statements is most accurate?

a.Calculate the % atom economy for this reaction.

Suggest why the atom economy is so low even though 75% of the molecules produced are the desired product

Outline an issue with the undesired product in this reaction

Calculate the percentage atom economy

Formulate the balanced equation for this process and calculate its atom economy.

Suggest, by referring to the chemical equation in the previous question, how the atom economy of the synthesis of N-methylphenylamine can be improved.

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

Find the concentration of the acid in mol dm-3

Find the concentration of the acid in g dm-3.

a.Formulate the balanced equation for the neutralization if the reaction products are barium chloride, BaCl2(aq), and water.

Determine the concentration, in mol dm−3, of barium hydroxide in the analysed solution.

Week 9 - Yields , atom economy and titration calculations

Week 9 - Yields , atom economy and titration calculations

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.N2 + 3H2 → 2NH3

Which of the following statements is most accurate?

a.Calculate the % atom economy for this reaction.

Suggest why the atom economy is so low even though 75% of the molecules produced are the desired product

Outline an issue with the undesired product in this reaction

Calculate the percentage atom economy

Formulate the balanced equation for this process and calculate its atom economy.

Suggest, by referring to the chemical equation in the previous question, how the atom economy of the synthesis of N-methylphenylamine can be improved.

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

Find the concentration of the acid in mol dm-3

Find the concentration of the acid in g dm-3.

a.Formulate the balanced equation for the neutralization if the reaction products are barium chloride, BaCl2(aq), and water.

Determine the concentration, in mol dm−3, of barium hydroxide in the analysed solution.

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.N2 + 3H2 → 2NH3

Which of the following statements is most accurate?

a.Calculate the % atom economy for this reaction.

Suggest why the atom economy is so low even though 75% of the molecules produced are the desired product

Outline an issue with the undesired product in this reaction

Calculate the percentage atom economy

Formulate the balanced equation for this process and calculate its atom economy.

Suggest, by referring to the chemical equation in the previous question, how the atom economy of the synthesis of N-methylphenylamine can be improved.

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

Find the concentration of the acid in mol dm-3

Find the concentration of the acid in g dm-3.

a.Formulate the balanced equation for the neutralization if the reaction products are barium chloride, BaCl2(aq), and water.

Determine the concentration, in mol dm−3, of barium hydroxide in the analysed solution.

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.
2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.
N2 + 3H2 → 2NH3

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)

1.96.0 g of sulfur dioxide was reacted with an excess of oxygen. In the reaction, only 90.0 g of sulfur trioxide was produced. Calculate the percentage yield of sulfur trioxide.
2SO2 + O2 → 2SO3

90.0 g of hydrogen with an excess of nitrogen. A 30% yield of ammonia was collected. Calculate the mass of ammonia produced.
N2 + 3H2 → 2NH3

25.0 cm3 of 0.0200 mol dm-3sulphuric acid neutralises 18.6 cm3 of barium hydroxide solution. Calculate the molar concentration of the barium hydroxide solution.
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)