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blushcicada32Lv1

6 Oct 2020

When copper(II) oxide is heated in hydrogen gas, the following reaction takes place,

. A copper rod coated with copper(II) oxide has a mass of 38.72 g. The rod is heated and made to react with 5.67L of hydrogen gas, whose density is .

(a) How many grams of were converted to ?

(b) What is the mass of copper after all the Hydrogen is consumed? (assume that is converted only to )

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Allen DinoLv9

21 Nov 2020

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Experiment 2

Trial 1

a) Mass of CuSO₄Â·5H₂O (g) 90.000g

b) Moles of CuSO₄Â·5H₂O (mol) _______

c) Moles of copper in CuSO₄Â·5H₂O (mol) _______

d) Mass of copper in CuSO₄Â·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 CuSO₄Â·5H₂O

Moles of copper in CuSO₄Â·5H₂O

Mass of copper in CuSO₄Â·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 didnât heat the solid long enough in Experiment 1.

b) The balance wasnât 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.

answers 6-10

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.