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Dvinal [7]
3 years ago
8

When 8.30 mol Mg react with 13.5 mol HCI, what is the limiting reactant and how many moles of H2 can be formed?

Chemistry
1 answer:
vovikov84 [41]3 years ago
4 0

6.75 moles of H₂

Explanation:

We have the following balanced chemical reaction:

Mg + 2 HCl → MgCl₂ + H₂

From the chemical reaction we deduce that if 1 mole of Mg is reating with 2 moles of HCl then 8.30 moles of Mg is reaction with 16.60 moles of HCl, quantity which is over our available 13.5 moles of HCl. The limiting reactant is HCl.

Knowing this we devise the following reasoning:

if         2 moles of HCl produces 1 mole of  H₂

then    13.5 moles of HCl produces X moles of  H₂

X = (13.5 × 1) / 2 = 6.75 moles of H₂

Learn more about:

balancing chemical equations

brainly.com/question/13898428

#learnwithBrainly

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What is the current theory about the formation of the solar system?
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A method used by the U.S. Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the
baherus [9]

Answer: 1. 9.08\times 10^{-6} moles

2. 90 mg

Explanation:

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According to stoichiometry:

1 mole of ozone is removed by 2 moles of sodium iodide.

Thus 4.54 \times 10^{-6} moles of ozone is removed by =\frac{2}{1}\times 4.54 \times 10^{-6}=9.08\times 10^{-6} moles of sodium iodide.

Thus 9.08\times 10^{-6} moles of sodium iodide are needed to remove 4.54\times 10^{-6} moles of O_3

2. \text{Number of moles of ozone}=\frac{0.01331g}{48g/mol}=0.0003moles

According to stoichiometry:

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Thus 0.0003 moles of ozone is removed by =\frac{2}{1}\times 0.0003=0.0006 moles of sodium iodide.

Mass of sodium iodide= moles\times {\text {molar mass}}=0.0006\times 150g/mol=0.09g=90mg    (1g=1000mg)

Thus 90 mg of sodium iodide are needed to remove 13.31 mg of O_3.

3 0
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