What percentage of the earth\'s crust can be attributed to aluminum atoms? 2.Whi

Question

What percentage of the earth's crust can be attributed to aluminum atoms?

2.Which of the following cations is aluminum metal capable of donating electrons to?

D. Zn

What are alums?

D. misspellings of aluminum

4. The conversion of aluminum to a cation of aluminum is an example of

D. cannot be determined without the charge

5. If you start this experiment with 4.20g of Al and have an excess of every other reagent, what is your theoretical yield?

D. 73.8g

6. A 6.0% by mass solution would contain what mass of sodium hypochlorite per 100.0g of solution?

D. 6 g

7. hat is the concentration (in molarity) of a 10.4% by mass solution of sodium chloride (NaCl - this is different from what we're using in this experiment... be sure to do this calculation for NaCl and NOT NaClO)?

D. 5.62

8. What is the molarity of 34.6g of NaClO dissolved in 157.0mL of water?

D. 2.20M

9.

H2 + O2 -> H2O

Given that unbalanced equation, balance it and select the correct statement below

C. 2 moles of H2 react with 1 mole of O2 to produce exactly 2 moles of H2O

d. reaction did not take place

10. Determining reaction stoichiometry by continuous variations is also known as

Explanation / Answer

(1)What percentage of the earth's crust can be attributed to aluminum atoms?

It is about 8% in the earth crust.

(2) Which of the following cations is aluminum metal capable of donating electrons to Zn remaining all are S-block elements so they ready to loose electrons to gat stability

(3)Alums are double salts.For example potash alum, or potassium aluminum sulfate,KAl(SO4)2·12H2O

                                                                                     0        +3

(4) The conversion of aluminum to a cation of aluminum is Al ----> Al3+

Here the oxidation state of Al increases from 0 to +3 so it is an example for oxidation reaction

(5) If you start this experiment with 4.20g of Al and have an excess of every other reagent, what is your theoretical yield?

Question incomplete

(6) A 6.0% by mass solution would contain what mass of sodium hypochlorite per 100.0g of solution?

6.0% by mass solution menas 6.0 g of sodium hypochlorite present in 100.0 g of solution

So the mass is 6.0g

(7) hat is the concentration (in molarity) of a 10.4% by mass solution of sodium chloride (NaCl - this is different from what we're using in this experiment... be sure to do this calculation for NaCl and NOT NaClO)?

Molarity = ( mass of NaCl / Molar mass of NaCl) x ( 1000 / Volume of solution in mL)

            = ( 10.4 g / 58.5(g/mol)) x ( 1000 / 100 mL)

            = 1.78 M

(8) . What is the molarity of 34.6g of NaClO dissolved in 157.0mL of water?

Molarity = ( mass of NaClO / Molar mass of NaClO) x ( 1000 / Volume of solution in mL)

            = ( 34.6 g / 74.5(g/mol)) x ( 1000 / 157.0 mL)

            = 2.96 M

(9)The balanced reaction is 2H2 + O2 ----> 2H2O

So 2 moles of H2 react with 1 mole of O2 to produce exactly 2 mole of H2O

(10) Determining reaction stoichiometry by continuous variations is also known as Job's method

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