Which statement is NOT correct regarding the statment below?
2Al+6HCl->2AlCl3+3H2
A. 2 atoms of Al produces 3 Molecules of H2
B. 3 Moles of Hcl produces 1 mole of AlCl3
C. 6 grams of Hcl reacts with 2 grams of Al
D. None of these.
I'm leaning towards C, but i'd like someone to explain.
Both A and B are correct. Chemical reactions are by mols and not by grams. That chemical reaction is to read 2 mols Al react with 6 mols HCl to produce 2 mols AlCl3 and 3 mols H2 gas.
That's what I was thinking. Think I'd be safe to go with C?
yes
To determine which statement is NOT correct, let's evaluate each statement one by one:
A. 2 atoms of Al produces 3 molecules of H2 - This statement is correct. According to the balanced chemical equation, 2 moles of Al react to produce 3 moles of H2. Since there are Avogadro's number (6.022 x 10^23) of atoms in a mole, 2 moles of Al equal 2 x 6.022 x 10^23 atoms. Therefore, 2 atoms of Al produce 3 molecules of H2.
B. 3 moles of HCl produce 1 mole of AlCl3 - This statement is correct. According to the balanced chemical equation, 6 moles of HCl react to produce 2 moles of AlCl3. However, the statement is asking about 3 moles of HCl, not 6 moles. So, this statement is incorrect.
C. 6 grams of HCl reacts with 2 grams of Al - This statement is also correct. To determine if it is incorrect, we need to compare the molar ratios between HCl and Al in the balanced equation. The molar mass of HCl is approximately 36.5 g/mol, and the molar mass of Al is approximately 27 g/mol. According to the balanced equation, 6 moles of HCl react with 2 moles of Al. Using the molar masses, we can convert grams to moles.
For HCl: 6 g HCl * (1 mol/36.5 g) = 0.164 moles of HCl
For Al: 2 g Al * (1 mol/27 g) = 0.074 moles of Al
As we can see, there is a smaller amount of Al compared to HCl. So, statement C is also correct.
Since both statements A and C are correct, the answer is D. None of these statements are incorrect.