Oxygen and carbon monoxide react to form carbon dioxide as shown in the following reaction
O2 (g) + 2CO (g) - 2CO2 (g)
If a sample of 70.0 g of carbon monoxide was reacted with
32.0 g of oxygen, how many moles of carbon dioxide would be
produced?
moles

The number of moles of carbon dioxide that would be produced is 2 moles

Explanation:

The given reaction is presented as follows;

O₂ (g) + 2CO (g) → 2CO₂ (g)

The parameters given are;

The mass of the carbon monoxide, m₁ = 70.0 g

The mass of the oxygen, m₂ = 32.0 g

The molar mass of carbon monoxide = 28.01 g/mol

The molar mass of oxygen gas O₂ = 32.0 g/mol

The number of moles, n = (The mass)/(The Molar Mass)

The number of moles of carbon monoxide in the reaction = 70.0 g/(28.01 g/mol) = 2.49910746 moles ≈ 2.5 moles

The number of moles of oxygen in the reaction = 32.0 g/(32.0 g/mol) = 1 moles

Therefore, from the chemical reaction, we have;

One mole of O₂ reacts with two moles of  CO  to produce two moles of CO₂ (g)

1 mole of oxygen produces 2 moles of carbon dioxide

Therefore, given that the number of moles of oxygen in the reaction is 1  mole, we have that the number of moles of carbon dioxide that would be produced = 2 moles.

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6