Chemistry, 24.07.2020 19:01 gabbygunshows4530

what mass of calcium nitrate can be prepared by the reaction of 18.9 grams of nitric acid with 7.4 grams of calcium hydroxide

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16.4 grams of calcium nitrate can be prepared by the reaction of 18.9 grams of nitric acid with 7.4 grams of calcium hydroxide

Explanation:

The balanced reaction is:

Ca(OH)₂ + 2 HNO₃ → Ca(NO₃)₂ + 2 H₂O

First, you must determine the limiting reagent. The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

To determine the limiting reagent, it is possible to use the reaction stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction):

Ca(OH)₂: 1 moleHNO₃: 2 molesCa(NO₃)₂: 1 mole H₂O : 2 moles

Being:

Ca: 40 g/moleO: 16 g/moleH: 1 g/moleN: 14 g/mole

Then, the molar mass of the compounds participating in the reaction is:

Ca(OH)₂: 40 g/mole + 2*(16 g/mole + 1 g/mole)= 74 g/moleHNO₃: 1 g/mole + 14 g/mole + 3*16 g/mole= 63 g/moleCa(NO₃)₂: 40 g/mole + 2*(14 g/mole + 3*16 g/mole)= 164 g/moleH₂O : 2*1 g/mole + 16 g/mole= 18 g/mole

Then, by stoichiometry of the reaction the following amounts of reagents and products participate:

Ca(OH)₂: 1 mole* 74 g/mole= 74 gHNO₃: 2 moles* 63 g/mole= 126 gCa(NO₃)₂: 1 mole* 164 g/mole= 164 gH₂O : 2 moles* 18 g/mole= 36 g

Then apply the following rule of three: if 126 grams of nitric acid reacts with 74 grams of calcium hydroxide, 18.9 grams of nitric acid with how much mass of calcium hydroxide does it react?

$mass of calcium hydroxide=\frac{18.9 grams of nitric acid*74 grams of calcium hydroxide}{126 grams of nitric acid}$

mass of calcium hydroxide= 11.1 grams

But 11.1 grams of calcium hydroxide are not available, 7.4 grams are available. Since you have less mass than you need to react with 18.9 grams of nitric acid, calcium hydroxide will be the limiting reagent.

Then, it is possible to determine the amount of mass of calcium nitrate produced by another rule of three: if 164 grams of calcium nitrate are formed by stoichiometry from 74 grams of calcium hydroxide, how much mass of calcium nitrate will form from 7.4 grams of calcium hydroxide?

$mass of calcium nitrate=\frac{7.4 grams of calcium hydroxide*164 grams of calcium nitrate}{74 grams of calcium hydroxide}$

mass of calcium nitrate= 16.4 grams

16.4 grams of calcium nitrate can be prepared by the reaction of 18.9 grams of nitric acid with 7.4 grams of calcium hydroxide

Answer from: Quest

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence, the electronegativity (or the ability to attract electrons) is lessened."

Answer from: Quest

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