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AveGali [126]
2 years ago
12

. For the reaction 2HNO3 + Mg(OH), → Mg(NO3)2 + 2H20, how many grams of magnesium nitrate are produced from 8.00 mol of nitric a

cid, HNO,?​
Chemistry
1 answer:
GREYUIT [131]2 years ago
6 0

Mass of Magnesium nitrate produced : 593.2 g

<h3>Further explanation</h3>

The reaction equation is the chemical formula of reagents and product substances

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

Reaction

2HNO₃ + Mg(OH)₂ → Mg(NO₃)₂ + 2H₂0

mol HNO₃ = 8

From the equation, mol ratio of HNO₃ : Mg(NO₃)₂ = 2 : 1, so mol Mg(NO₃)₂ :

\tt \dfrac{1}{2}\times 8=4~moles

Mass Mg(NO₃)₂(MW=148,3 g/mol) :

\tt mass=mol\times MW\\\\mass=4\times 148,3 g/mol\\\\mass=593.2~g

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When 5.58g H2 react by the following balanced equation, 32.8g H2O are formed. What is the percent yield of the reaction? 2H2(g)+
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<em />

To find percent yield of the reaction we need to find theoretical yield (The yield assuming all hydrogen reacts producing water). With theoretical yield and actual yield (32.8g H₂O) we can determine percent yield as 100 times the ratio between actual yield and theoretical yield.

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5.58g H₂ ₓ (1 mol / 2.016g) = 2.768 moles H₂

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65.7% is percent yield of the reaction

<h3>D) 65.7% </h3>

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