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torisob [31]
3 years ago
6

If 5.65 grams of zinc metal react with 21.6 grams of silver nitrate, how many grams of silver metal can be formed and how many g

rams of the excess reactant will be left over when the reaction is complete? Show all of your work.
unbalanced equation: Zn + AgNO3 Zn(NO3)2 + Ag
Chemistry
2 answers:
Igoryamba3 years ago
7 0
The balanced chemical reaction is:

Zn + 2AgNO3 =  Zn(NO3)2 + 2Ag

To determine the amount of the reactant left, we have to determine which is the limiting and the excess reactant. We do as follows:

5.65 g Zn ( 1 mol / 65.38 g) = 0.09 mol Zn
21.6 g AgNO3 (1 mol / 169.87 g) = 0.13 mol AgNO3

The limiting reactant would be silver nitrate since it is consumed completely in the reaction. The excess reactant would be zinc. 

Excess Zinc = 0.09 mol Zn - (0.13 / 2) mol Zn = 0.025 mol Zn left
STALIN [3.7K]3 years ago
5 0

Answer:

1.3710 grams of silver metal can be formed.

0.4158 grams of the excess reactant will be left over when the reaction is complete

Explanation:

Zn+2AgNO_3\rightarrow Zn(NO_3)_2+2Ag

Moles of zinc metal =\frac{5.65 g}{65.38 g/mol}=0.0864 mol

Moles of silver nitrate = \frac{21.6}{169.87 g/mol}=0.01271 mol

According to reaction , 1 mole of zinc reacts with 2 mole of silver nitrate.

Then 0.0864 mol of zinc will react with:

2\times 0.0864 mol=0.1728 mol silver nitrate

This means that zinc is in excessive amount.

So, the formation of silver metal will depend on moles of silver nitrate.

According to reaction 2 moles of silver nitrate produces 2 mole of silver metal.

Then 0.01271 moles of silver nitrate will produce:

\frac{2}{2}\times 0.01271 mol=0.01271 mol of silver metal

Mass of 0.01271 mol of silver metal = 0.01271 mol × 107.87 g/mol = 1.3710 g

Moles of excessive reagent left

According to reaction , 1 mole of zinc reacts with 2 mole of silver nitrate.

Then 0.01271 mol of silver nitrate will react with:

\frac{1}{2}\times 0.01271 mol=0.00635 mol of zinc

Moles of an excess reagent = 0.01271 mol - 0.00635 mol = 0.00636 mol

Mass of 0.00636 mol zinc:

0.00636 mol × 65.38 g/mol = 0.4158 g

1.3710 grams of silver metal can be formed.

0.4158 grams of the excess reactant will be left over when the reaction is complete

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The molar concentration will be greater than 0.01 M KIO_{3}.


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A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapour pressure of pure CCl4 is 33
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Explanation:

The given data is as follows.

     Vapour pressure of pure CCl_{4} = 33.85 Torr

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Therefore, calculate the vapor pressure of Br_{2} as follows.      

     Vapour pressure of Br_{2} = mole fraction of Br_{2} x K of Br_{2}

                                    = 0.050 x 122.36 Torr

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So, vapor pressure of Br_{2} is 6.118 Torr .

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     Vapour pressure of CCl_{4} = mole fraction of CCl_{4} x Pressure of CCl_{4}

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So, vapor pressure of CCl_{4} is 32.1575 Torr  .

Hence, the total pressure will be as follows.

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Therefore, composition of CCl_{4} = \frac{32.1575 Torr}{38.2755 Torr}

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Composition of CCl_{4} is 0.8405 .

And, composition of Br_{2} = \frac{6.118 Torr}{38.2755 Torr}

                                                  = 0.1598

Composition of Br_{2} is 0.1598 .

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