If an experiment with 10.2 g barium chloride produced 14.5 g silver chloride, calculate thr experimental mole ratio of silver chloride to barium chloride

2.06/1

Explanation:

First, we will find the moles of each compound.

The molar mass of BaCl₂ is 208.23 g/mol. The moles corresponding to 10.2 g are:

10.2 g × (1 mol/208.23 g) = 0.0490 mol

The molar mass of AgCl is 143.32 g/mol. The moles corresponding to 14.5 g are:

14.5 g × (1 mol/143.32 g) = 0.101 mol

The experimental mole ratio of AgCl to BaCl₂ is 0.101 mol/0.0490mol = 2.06/1

This is very close to the theoretical mole ratio of AgCl to BaCl₂, according to the following reaction, which is 2/1.

BaCl₂ + 2 Ag⁺ → 2 AgCl + Ba²⁺

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radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.