Study the balanced equation.

3Hg(OH)2 + 2H3PO4 → Hg3(PO4)2 + 6H2O

How many mols of phosphoric acid (H3PO4) reacted to form 3.13 x 101 mol of water (H2O)?

A) 5.22 × 100 mol H3PO4

B) 9.39 × 101 mol H3PO4

C) 6.26 × 101 mol H3PO4

D) 1.04 × 101 mol H3PO4

D) 1.04 × 10¹ mol H₃PO₄

Explanation:

Based on the reaction:

3Hg(OH)₂ + 2H₃PO₄ → Hg₃(PO₄)₂ + 6H₂O

2 moles of phosphoric acid produce 6 moles of water. If there are produced 3.13x10¹ moles of water, the phosphoric acid moles that reacted are:

3.13x10¹ moles of water ₓ (2 moles phosphoric acid / 6 moles of water) =  1.04 × 10¹ mol H₃PO₄

Right answer is:

D) 1.04 × 10¹ mol H₃PO₄

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.