Mg reacts with 150 mL of 6.00M Hcl through single replacement to produce hydrogen gas. How many liters of hydrogen gas are produced? (tell me how you got it please)
I assume this is for STP.
Write and balance the equation.
Mg + 2HCl ==> H2 + MgCl2
How many moles HCl did you use? M x L = moles.
Using the coefficients in the balanced equation, convert moles HCl to moles H2.
Now convert moles H2 to liters knowing that 1 mole H2 gas occupies 22.4 L at STP.
Post your work if you get stuck.
To determine the number of liters of hydrogen gas produced, we need to use the given information about the reactants and stoichiometry.
First, we can write the balanced chemical equation for the reaction:
Mg + 2HCl → MgCl2 + H2
From the balanced equation, we know that one mole of magnesium (Mg) reacts with two moles of hydrochloric acid (HCl) to produce one mole of hydrogen gas (H2).
We are given the concentration of HCl as 6.00M, which means there are 6.00 moles of HCl in 1 liter of the solution. However, we have 150 mL of the HCl solution, which is equivalent to 0.150 liters.
To calculate the number of moles of HCl used, we multiply the volume (in liters) by the concentration:
0.150 L × 6.00 mol/L = 0.900 mol HCl
Since the ratio of Mg to H2 in the balanced equation is 1:1, this tells us that 0.900 moles of magnesium will produce 0.900 moles of hydrogen gas.
Finally, we convert moles of hydrogen gas to liters using the ideal gas law. At standard temperature and pressure (STP), one mole of any gas occupies 22.4 liters.
0.900 mol H2 × 22.4 L/mol = 20.16 L
Therefore, approximately 20.16 liters of hydrogen gas are produced when Mg reacts with 150 mL of 6.00M HCl.