Answer:
For Mass N, Mass H, and Mass O, the mass is 28.0 g N, 4.0 g H, and 48.0 g respectively
Explanation:
The computation of the mass of each element is given below:
As we know that
A1 mole of ammonium nitrate i.e. 2 mol N, 4 mol H, 3 mol
Now we multiply each of above by the molar masses
For N
= 14.0 g/mol × 2
= 28.0 gN
For H
= 1.0 g/mol × 4
= 4.0 gN
ANd, for O
= 16.0 g/mol × 3
= 48.0 gN
Hence, For Mass N, Mass H, and Mass O, the mass is 28.0 g N, 4.0 g H, and 48.0 g respectively
The theoretical yield of silver chloride, AgCl is 5.2109 g
The balanced equation for the reaction is given below:
<h3>3AgNO₃(aq) + AICI₃(aq) —> Al(NO₃)₃ (aq) + 3AgCl (s) </h3>Next, we shall determine the mass of aluminum chloride, AICI₃ that reacted and the mass of silver chloride, AgCl produced from the balanced equation. This is illustrated below:
Molar mass of AICI₃ = 133.34 g/mol
Mass of AICI₃ from the balanced equation = 1 × 133.34 = 133.34 g
Molar mass of AgCl = 143.32 g/mol
Mass of AgCl from the balanced equation = 3 × 143.32 = <em>429.96 g</em>
<h3>SUMMARY</h3>From the balanced equation above,
133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.
Finally, we shall determine the theoretical yield of AgCl by the reaction of 1.616 g of AICI₃ as follow:
From the balanced equation above,
133.34 g of AICI₃ reacted to produce 429.96 g of AgCl.
Therefore,
1.616 g of AICI₃ will react to produce = = 5.2109 g of AgCl.
Thus, the theoretical yield of silver chloride, AgCl is 5.2109 g
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