When carbon is burned in air, it reacts with oxygen to form carbon dioxide. when 27.6 g of carbon were burned in the presence of 89.6 g of oxygen, 16.0 g of oxygen remained unreacted. what mass of carbon dioxide was produced?

101.2 g of carbon dioxide was produce.

Explanation:

Given data:

mass of mass of carbon = 27.6 g

mass of oxygen = 89.6 g

mass of unreacted oxygen = 16 g

mass of carbon dioxide produced = ?

Solution:

To solve this problem first of all we will calculate the mass of oxygen that reacted.

mass of reacted oxygen = total mass - unreacted mass

mass of oxygen= 89.6 g - 16 g

mass of oxygen= 73.6 g

mass of carbon dioxide produced = mass of oxygen + mass of carbon

mass of carbon dioxide produced = 73.6 g + 27.6 g

mass of carbon dioxide produced = 101.2 g

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.