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11 Dec 2019

A number of chemical reactions have been proposed for the formation of organic (chemicals of life) compounds from inorganic precursors. Here is one of them: H2S(g) + FeS(s) + CO2(g) → FeS2(s) + HCO2H(l)

a) identify the ions and charges in FeS and FeS2 and name the compounds

b) How much HCO2H is obtained by reacting 1.10 g of FeS with 0.500 g H2S and 0.500 g of CO2 if the reaction produces a yield of 50%?  

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Patrina Schowalter
Patrina SchowalterLv2
13 Dec 2019

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Related questions

A number of chemical reactions have been proposed for the formation of organic compounds form inorganic precursors. Here is one of them:

H2S +FeS +CO2 -> FeS2 +HCO2H

(a) Supply the correct formula and charge for the ions in FeS. Give the correct name for the compound.

(b) How much HCO2H is obtained by reacting 4.00g of FeS, 2.00g of H2S, and 2.00g of CO2 if the reaction results in a 48.0% yield?

(2) Citric acid (H3C6H5O7) occurs in plants. The acid is added to beverages and candy. An aqueous solution is 0.710 m in citric acid. The density is 1.049 g/mL. Calculate the concentration of this solution as: (w/w %) (w/v %) M Mole Fraction (citric acid) 2

(3) When 75.0 mL of a 0.100 M lead (II) nitrate solution is mixed with 100.0 mL of a 0.190 M potassium iodide solution, a yellow-orange precipitate of lead (II) iodide is formed. a. Write the balanced molecular and net-ionic equation. b. Assuming 100% yield calculate the mass of lead (II) iodide formed. c. Determine the molarities of ions left in solution after the reaction.

(4) A 15.00 mL solution of KNO3 was diluted to 125.0 mL and 25.00 mL of this solution was then diluted to 1000. mL. The concentration of KNO3 in the 1000. mL is 0.00383 M. What was the M of KNO3 in the original solution? 3

(5) How many grams of pure H2SO4 can be obtained from 250 g of iron ore if the ore is 82.0 % (w/w %) FeS2. The reactions involved are given below: 4FeS2 + 11O2 → 2Fe2O3 + 8SO2 (95.0% efficient) 2SO2 + O2 → 2SO3 (90.0 % efficient) SO3 + H2O → H2SO4 (90.0 % efficient)

(6) 30.0 mL of 0.512 M sulfuric acid was added to 25.0 mL of 0.666 M sodium hydroxide. a. Write the balanced chemical equation. b. Determine the molarity of either acid or base remaining after the reaction. c. Find the molarity if a 50.00 mL aliquot of this solution is diluted to 250. mL.

(8) Oxygen is produced by the reaction: 2KClO3 (s) →2KCl (s) + 3O2 (g)  The oxygen produced was collected over water. A sample of KClO3 produced 705 mL of oxygen saturated with water vapor at 20.0 °C where the vapor pressure of water is 17.54 mm Hg. The total gas pressure was 1.104 atm. What mass of KClO3 decomposed?

(9) How many grams of C2H2 must burn according to the equation below in order to heat 2.34 × 104 g of H2O from 25.0 °C to 35.0 °C? C2H2 (g) + O2 (g) →H2O (l) + CO2 (g), Δ = – 1212 kJ

1- The molar heat capacity of silver is 25.35 J/mol⋠∘C. How much energy would it take to raise the temperature of 8.20 g of silver by 14.5 ∘C?

Express your answer with the appropriate units.

_____________

Part A

Calculate the enthalpy of the reaction

2NO(g)+O2(g)→2NO2(g)

given the following reactions and enthalpies of formation:

12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ

12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ

Express your answer with the appropriate units.

2- A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 196 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 ∘C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water.

Enter your answer in kilojoules per mole of compound to three significant figures.

_________

3- A volume of 110. mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘Cis placed in the water. If the final temperature of the system is 21.00 ∘C , what is the mass of the steel bar?

Use the following values:

specific heat of water = 4.18 J/(g⋠∘C)

specific heat of steel = 0.452 J/(g⋠∘C)

Express your answer to three significant figures and include the appropriate units.

Part B

The specific heat of water is 4.18 J/(g⋠∘C). Calculate the molar heat capacity of water.

Express your answer to three significant figures and include the appropriate units.

______-

4- What is the enthalpy for the following reaction?

overall: N2O4→2NO2

Express your answer numerically in kilojoules per mole.

____________

Part B

Calculate the enthalpy of the reaction

4B(s)+3O2(g)→2B2O3(s)

given the following pertinent information:

B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ

2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ

H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ

H2O(l)→H2O(g), ΔH∘D=+44 kJ

Express your answer with the appropriate units.

_____________

5- What is the balanced chemical equation for the reaction used to calculate ΔH∘f of MgCO3(s)?

If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution.

Express your answer as a chemical equation.

__________

6- Part A

Determine the enthalpy for this reaction:

Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l)

Express your answer in kilojoules per mole to one decimal place.

_______

Part B

Consider the reaction

Ca(OH)2(s)→CaO(s)+H2O(l)

with enthalpy of reaction

ΔHrxn∘=65.2kJ/mol

What is the enthalpy of formation of CaO(s)?

Express your answer in kilojoules per mole to one decimal place.

________

7- Part A

Write a balanced chemical equation depicting the formation of one mole of H2O2(g) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part B

For H2O2(g), find the value of ΔH∘f. (Use Appendix C)

Express your answer using five significant figures.

_____

PART C: Write a balanced chemical equation depicting the formation of one mole of CaCO3(s) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part D

For CaCO3(s), find the value of ΔH∘f. (Use Appendix C)

Express your answer using five significant figures.

_____

Part E

Write a balanced chemical equation depicting the formation of one mole of POCl3(l) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

____

Part F

For POCl3(l), find the value of ΔH∘f. (Use Appendix C)

Express your answer using four significant figures.

_____

Part G

Write a balanced chemical equation depicting the formation of one mole of C2H5OH(l) from its elements in their standard states.

Express your answer as a chemical equation. Identify all of the phases in your answer.

_____

Part H

For C2H5OH(l), find the value of ΔH∘f. (Use Appendix C)

Express your answer using four significant figures.

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