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A.) In the Oxygen Lab, we performed a variety of reactions involving oxygen. Please provide the balanced, chemical equation for the reaction between copper and oxygen that produced copper (II) oxide.

B.) In the Oxygen Lab, we performed a variety of reactions involving oxygen. Please provide the two balanced, chemical equations for the two steps involved in the production of phosphoric acid starting from phosphorous and oxygen.

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Related questions

Experiment 2

Trial 1

a) Mass of CuSO4·5H2O (g) 90.000g

b) Moles of CuSO4·5H2O (mol) _______

c) Moles of copper in CuSO4·5H2O (mol) _______

d) Mass of copper in CuSO4·5H2O (g) _______

e) Mass of copper oxide obtained 29.267g

f) Mass of oxygen in copper oxide _______

g) Moles of oxygen in the copper oxide (mol) _______

h) Mole ratio, copper to oxygen (Cu:O) _______

i Average ratio, copper to oxygen (Cu:O) _______

j) Formula of copper oxide _______

Mass of empty beaker 85.000g

Mass of beaker and Copper (II) sulfate pentahydrate 90.000g

Mass of empty test tube 27.400g

Mass of test tube after heating and cooling 29.306g

Using your data from Trial 1, show your work for each of the following:

Moles of CuSO4·5H2O

Moles of copper in CuSO4·5H2O

Mass of copper in CuSO4·5H2O

Mass of oxygen in copper oxide

Moles of oxygen in the copper oxide

Mole ratio, copper to oxygen

Questions

1. How would each of the following affect your experimental determination of your copper/oxygen ratio (too high, too low, or no effect)? In each case, explain your answers.

a) You didn’t heat the solid long enough in Experiment 1.

b) The balance wasn’t properly calibrated in Experiment 1, causing all masses to be too 0.50 g too high.

c) Not all of the copper sulfate was converted to copper hydroxide in Experiment 2.

2. Write a balanced equation for the reaction occurring between copper and oxygen in Experiment 1.

3. Write a balanced equation for the reaction occurring between copper (II) sulfate and NaOH in Experiment 2.

4. Write a balanced equation for the reaction that occurred when the precipitate from Experiment 2 was heated.

Write balanced chemical equations to correspond to each of the following descriptions: (a) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. b) Boron sulfide, B2S3(s), reacts violently with water to form dissolved boric acid, H3BO3, and hydrogen sulfide gas. (c) Phosphine, PH3(g), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide. (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen. (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.

Write balanced equations for the following reactions. a.) Tin (II) oxide reacts with hydrogen gas to produce tin metal and water b.) Potassium hydroxide reacts with sulfuric acid to produce water and potassium sulfate c.) Octane combusts in the presence of oxygen to form carbon dioxide and water d.) Iron (III) chloride reacts with copper (II) sulfate (include the products formed)

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