All categories

3 years ago

How many grams of aluminum chloride are produced when 6.73 g of aluminum react with an excess of chlorine gas?

Chemistry

1 answer:

sergejj [24]3 years ago

8 0

Answer:

33.3 g AlCl3

Explanation:

First:

You need a balanced chem equation.

2Al + 3Cl2 --->2AlCl3

So now you use this to set up train track method which helps us cancel out the units. Also we dont care about chlorine because it is excess.

6.73g Al x 1mol Al/26.98g Al x 2mol AlCl3/2molAl x 133.34g AlCl3/1molAlCl3

= 33.3 g AlCl3

You might be interested in

Determine the number of molecules in 43.9 g of carbon tetrachloride

ddd [48]

Answer: There are about 0.28 molecules in 43.9 g of carbon tetrachloride. If you are rounding up, it would be 0.3

Explanation:

7 0

2 years ago

Name the two subatomic particles found in the nucleus.

Vesna [10]

i can think of 3 subatomic particles found in a nucleus protons, neutrons, and electrons

6 0

3 years ago

Read 2 more answers

At what step of glycolysis one NADH+ H+ is formed?

ElenaW [278]

Answer:

During Glycolysis, there is one step where NADH + H+ is formed from NAD+ O F-6-P - F- 1,6-BP O PGAL – 1,3-BPGA O 2-PGA - PEP O 3-PGA → 2-PGA.

3 0

2 years ago

Is corrosion of aluminum metal a chemical or physical process

nadya68 [22]

Corrosion of aluminium metal is a chemical process. Corrosion happens when a certain chemical reaction takes place.

8 0

3 years ago

What is the empirical formula? A compound is used to treat iron deficiency in people. It contains 36.76% iron, 21.11% sulfur, an

Mandarinka [93]

Answer: The empirical formula of the compound is $Fe_1S_1O_4$

Explanation:

Empirical formula is defined formula which is simplest integer ratio of number of atoms of different elements present in the compound.

Percentage of iron in a compound = 36.76 %

Percentage of sulfur in a compound = 21.11 %

Percentage of oxygen in a compound = 42.13 %

Consider in 100 g of the compound:

Mass of iron in 100 g of compound = 36.76 g

Mass of iron in 100 g of compound = 21.11 g

Mass of iron in 100 g of compound = 42.13 g

Now calculate the number of moles each element:

Moles of iron= $\frac{36.76 g}{55.84 g/mol}=0.658 mol$

Moles of sulfur= $\frac{21.11 g}{32.06 g/mol}=0.658 mol$

Moles of oxygen= $\frac{42.13 g}{16 g/mol}=2.633 mol$

Divide the moles of each element by the smallest number of moles to calculated the ratio of the elements to each other

For Iron element = $\frac{0.658 mol}{0.658 mol}=1$

For sulfur element = $\frac{0.658 mol}{0.658 mol}=1$

For oxygen element = $\frac{2.633 mol}{0.658 mol}=4.001\approx 4$

So, the empirical formula of the compound is $Fe_1S_1O_4$

4 0

3 years ago

Read 2 more answers