Al + CuSO4 ⟶ Cu + Al2(SO4)3
How many grams of copper will be produced when 1.87 grams of Al is used?

Question

person321 · Answer

please help ^^

jhonyy9 · Answer

like a first step you need balance this reaction - hope you know the way

person321 · Answer

2Al + 3CuSO4 ⟶ 3Cu Al2(SO4)3

there's the balanced equation

person321 · Answer

um, could someone help?

AZ · Answer

Good! You correctly balanced the equation. $\text{2 Al + 3 CuSO}_4 \to \text{3 Cu + Al}_2\text{(SO}_4)_3$ We are told that 1.87 grams of aluminum are used. This means that Al is our limiting reagent and we have plenty of $\text{CuSO}_4$ The most important thing you have to remember is that the chemical equation gives us the molar ratios. This means that the ratio between the reactants and products is in moles. We cannot use grams. We have to use moles which requires us to first convert grams to moles. This image should help you remember how to convert between grams, moles, and molecules https://chemistrylearningbydoing.org/wp-content/uploads/2019/06/chapter5_fig2.png

AZ · Answer

From our balanced chemical equation, we know that 2 moles of aluminum will form 3 moles of copper. But first, let's convert 1.87 g of Al to moles. Do you know how to find the molar mass of aluminum? We have to use the periodic table https://thisperiodictable.com/ The number under the element is the molar mass. For example: oxygen's molar mass is 15.999 This means that 15.999 grams of oxygen is 1 mole of oxygen So what is the molar mass of aluminum? And can you use that to calculate how many moles of aluminum we have?