Given the following equation: H2(g)+F2(g)=2HF(g) How many grams of HF gas are produced as 5 mol of fluorine react?

200grams

Explanation:

The balanced chemical equation for this reaction is given as follows:

H2(g)+F2(g) → 2HF(g)

This equation shows that it takes 1 mol of both hydrogen gas (H2) and fluorine gas (F2) to produce 2 moles of hydrogen fluoride (HF)

Hence, 5 moles of fluorine gas (F2) will produce 5 × 2 = 10 moles of HF.

In order to convert the mole value of HF to gram value, we use the following formula;

Mole = mass/molar mass

Molar mass of HF = 1 + 19 = 20g/mol

mass = mole × molar mass

mass = 10 × 20

mass = 200grams of HF.

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o