A student tried to solve the following problem by selecting the conversion below. What, if anything, did the student do wrong?
How many moles of AgNO3 are needed to produce 6.75 moles of copper (II) nitrate Cu(NO3)2 upon reacting with excess copper (Cu)?
2AgNO3 + Cu --> 2Ag + Cu(NO3)2
Students conversion factor: 6.75 mol Cu(NO3)2 x 1 mol Cu(NO3)2/2 mol AgNO3
Question Options:
The student chose the wrong conversion factor.
The student chose the correct conversion factor, but need to flip it to make units cancel.
The student chose the correct conversion factor, but needs to add a second to finish the problem.
There is nothing wrong the problem is ready to be solved.
Hmm, let's clown around with this chemistry problem! It seems like the student went a bit astray here. They chose the wrong conversion factor! Oh no! But hey, we all make mistakes, right? So, option one is the correct answer. The student just needs to choose the right conversion factor and they'll be back on track! Keep trying, student!
The student chose the wrong conversion factor.
The student made a mistake in selecting the conversion factor. The given reaction shows that 2 moles of AgNO3 react with 1 mole of Cu(NO3)2. However, the student used a conversion factor of 1 mole of Cu(NO3)2 to 2 moles of AgNO3.
To solve the problem correctly, the conversion factor should be flipped so that it matches the stoichiometry of the reaction:
Conversion factor: 2 mol AgNO3 / 1 mol Cu(NO3)2
This conversion factor represents the ratio between the number of moles of AgNO3 and Cu(NO3)2 according to the balanced equation.
Therefore, the correct answer is: The student chose the correct conversion factor, but needs to flip it to make units cancel.
6.75 mol Cu(NO3)2 x 1 mol Cu(NO3)2/2 mol AgNO3
The correct conversion factor is
6.75 mols Cu x (2 mols AgNO3/1 mol Cu) = ?