027 (part 1 of 3) 10.0 points
Copper reacts with silver nitrate through single
replacement. If 3.03 g of silver are produced
from the reaction, how much copper(II)
nitrate is also produced?
Answer in units of mol.
028 (part 2 of 3) 10.0 points
How much Cu is required in this reaction?
Answer in units of mol.
029 (part 3 of 3) 10.0 points
Howmuch AgNO3 is required in this reaction?
Answer in units of mol.
Aren't these regular stoichiometry problems?
To answer these questions, we need to use the concept of stoichiometry and the balanced chemical equation for the reaction between copper and silver nitrate.
The balanced chemical equation for the reaction can be written as:
Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag
Now let's answer each part of the question:
027 (part 1 of 3):
To find the amount of copper(II) nitrate produced, we need to determine the number of moles of silver produced. We can use the molar ratio between silver and copper(II) nitrate from the balanced equation:
From the equation, we can see that 1 mole of copper reacts with 2 moles of silver. Therefore, we can write the following proportion:
1 mol of copper / 2 mol of silver = x mol of copper / 3.03 g of silver
To solve for x (the amount of copper(II) nitrate produced), we need to rearrange the proportion and solve for x:
x = (1 mol of copper / 2 mol of silver) * (3.03 g of silver)
x = 1.515 g of copper(II) nitrate
Therefore, the answer is 1.515 mol of copper(II) nitrate.
028 (part 2 of 3):
To find the amount of copper required in this reaction, we can use the same balanced equation and the molar ratio between copper and silver:
From the equation, we can see that 1 mole of copper reacts with 2 moles of silver. Therefore, we can write the following proportion:
1 mol of copper / 2 mol of silver = x mol of copper / y mol of silver
Since there is no information given about the amount of silver, we cannot directly calculate the amount of copper required. We need more information to answer this question.