given the equation Mg +2HCL --> MgCL2+H2, how many moles of hydrochloric acid are needed to react with O.50 mol of magnesium ?
(1)0.5
(2)1.0
(3)2.0
(4)4.0
is it 3 ?
To determine the moles of hydrochloric acid needed to react with 0.50 mol of magnesium, we need to refer to the balanced equation:
Mg + 2HCl → MgCl2 + H2
According to the stoichiometry of the equation, we can see that 1 mol of magnesium reacts with 2 moles of hydrochloric acid. Therefore, to determine the moles of hydrochloric acid needed to react with 0.50 mol of magnesium, we multiply the mole ratio by the number of moles of magnesium:
0.50 mol Mg × 2 mol HCl / 1 mol Mg = 1.0 mol HCl
So, the correct answer is (2) 1.0.
To determine the number of moles of hydrochloric acid needed to react with 0.50 mol of magnesium, we need to use the balanced chemical equation and stoichiometry.
The balanced chemical equation is:
Mg + 2HCl → MgCl2 + H2
From the balanced equation, we can see that 1 mole of magnesium reacts with 2 moles of hydrochloric acid.
Since we have 0.50 mol of magnesium, we need to determine how many moles of hydrochloric acid are required:
0.50 mol Mg × (2 mol HCl / 1 mol Mg) = 1.0 mol HCl
Therefore, 1.0 mole of hydrochloric acid is needed to react with 0.50 mole of magnesium.
The correct answer is option (2) 1.0.
It helps us help you if you don't change your screen name, especially when asking the same type question. Look back at the problem I worked with the NH3 and O2 problem? This one would be
??moles HCl = moles Mg x (moles HCl/moles Mg) = 0.50 mole Mg x (2 mol HCl/1 mol Mg) = ??. Is that 3?
Note again: You want the answer to be in units of HCl; therefore, note the mols Mg cancel and leaves units of HCl.