Question

The compound KCLO3 decomposes according to the following equation
@KCLO3-- 2KCL + 3O2
a) what is the mole ratio of KCLO3 to O2 in this reaction?
b) How many moles of O2 can be produced by letting 6.0 moles of KCLO3 react based on the above equation?
c) How many molecules of oxygen gas, O2, are produced in question 1b?
2. Magnesium combines with chlorine, Cl2 to form magnesium chloride, MgCl2 during a synthesis reaction.
a) write a balanced chemical equation for the reaction.
b) How many moles of magnesium chloride can be produced with 3 moles of chlorine?

Answer 1

#72437 Chemistry, Other

1. The compound $\mathrm{KClO}_3$ decomposes according to the following equation

$$@\mathrm{KClO}_3 \rightarrow 2\mathrm{KCl} + 3\mathrm{O}_2$$

a) what is the mole ratio of $\mathrm{KClO}_3$ to $\mathrm{O}_2$ in this reaction?

b) How many moles of $\mathrm{O}_2$ can be produced by letting 6.0 moles of $\mathrm{KClO}_3$ react based on the above equation?

c) How many molecules of oxygen gas, $\mathrm{O}_2$, are produced in question 1b?

2. Magnesium combines with chlorine, $\mathrm{Cl}_2$ to form magnesium chloride, $\mathrm{MgCl}_2$ during a synthesis reaction.

a) write a balanced chemical equation for the reaction.

b) How many moles of magnesium chloride can be produced with 3 moles of chlorine?

Answer:

1a. $2\mathrm{KClO}_3 \rightarrow 2\mathrm{KCl} + 3\mathrm{O}_2$

Mole ratio $\mathrm{KClO}_3$ to $\mathrm{O}_2$ is $2:3$

1b. $n(\mathrm{O}_2) = 3/2 \cdot n(\mathrm{KClO}_3) = 3/2 \cdot 6 = 9$ moles

1c. 1 mole = $6.022 \cdot 10^{23}$ molecules

9 moles $\cdot 6.022 \cdot 10^{23}$ molecules = $54.198 \cdot 10^{23}$ molecules

2a. $\mathrm{Mg} + \mathrm{Cl}_2 = \mathrm{MgCl}_2$

$n(\mathrm{MgCl}_2) = n(\mathrm{Cl}_2)$

2b. 3 moles of $\mathrm{Cl}_2$ gives 3 moles of $\mathrm{MgCl}_2$

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