In the reaction
Cu+2AgNO3->2Ag+Cu(NO3)2
what number of grams of silver can be produced from the reaction of 83.7 g of copper?
a. 284 g Ag
b. 142.1 g Ag
c. 71.1 g Ag
d. 98.6 g Ag
e. 1.32 g Ag
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To solve this problem, we need to first determine the molar ratio between copper and silver in the balanced chemical equation. From the equation:
Cu + 2AgNO3 -> 2Ag + Cu(NO3)2
We can see that for every one mole of copper (Cu) that reacts, 2 moles of silver (Ag) are produced. Therefore, the molar ratio between copper and silver is 1:2.
Next, we need to determine the number of moles of copper (Cu) in 83.7 g. To do this, we divide the given mass by the molar mass of copper.
Molar mass of copper (Cu) = 63.55 g/mol
Number of moles of copper (Cu) = 83.7 g / 63.55 g/mol = 1.32 mol
Since the molar ratio between copper and silver is 1:2, this means that for 1.32 moles of copper, we will produce double that amount of silver (2.64 moles).
Finally, we can calculate the mass of silver (Ag) produced by multiplying the number of moles by the molar mass of silver.
Molar mass of silver (Ag) = 107.87 g/mol
Mass of silver (Ag) = 2.64 mol * 107.87 g/mol = 284 g Ag
Therefore, the correct answer is:
a. 284 g Ag
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