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lilavasa [31]
2 years ago
5

How many moles of HCI can be formed when 2 mol of hydrogen gas react with chlorine

Chemistry
1 answer:
miss Akunina [59]2 years ago
4 0

So the molar ratio of H2 to HCl is 1:2, so you can make 2mol x 2 = 4 moles of HCl.

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The following reaction does not proceed to form a product: H2O + Au---> no reaction. Why is that?. . A. Gold has a higher act
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5 0
3 years ago
4.0 g Mg and 4.0 g O2 are placed in a container and magnesium oxide, MgO, forms. The Mg is totally consumed but 1.4 g O2 remains
goldfiish [28.3K]

Answer:

The correct answer is: 6.6 g MgO

Explanation:

First we have to write and balance the chemical reaction as follows:

2Mg(s) + O₂(g) → 2MgO(s)

That means that 2 moles of Mg(s) react with 1 mol of O₂(g) to give 2 moles of MgO(s). If Mg is totally consumed and a mass of O₂ remains unaltered after reaction, t<em>he limiting reactant is Mg</em>. We use the limiting reactant to calculate the mass of product.

According to the balanced chemical equation, 2 moles of Mg(s) produce 2 moles of MgO(s).

2 moles Mg = 2 mol x molar mas Mg= 2 mol  x 24.3 g/mol = 48.6 g Mg

2 moles MgO= 2 mol x (molar mass Mg + molar mass O) = 2 mol x (24.3 g/mol + 16 g/mol) = 80.6 g MgO

The stoichiometric ratio is 80.6 g MgO/48.6 g Mg. So, we multiply this ratio by the mass of consumed Mg (4.0 g) in order to obtain the produced mass of MgO:

4.0 g Mg x 80.6 g MgO/48.6 g Mg = 6.63 g MgO

6.6 grams of magnesium oxide are formed.

5 0
3 years ago
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