In the reaction of 2.75 g of magnesium metal with excess hydrochloric acid, what volume of hydrogen gas will be produced by the reaction if the lab occurs at 25.0oC and 765 torr? (Hint: write a balanced chemical reaction first and do stoichiometry, then use the ideal gas law)

Answer 1

What pressure will be exerted by 45.0 grams of CO2 at a temperature of 25 ˚C and a volume of 630. mL

Answer 2

In the reaction of 2.75 g of magnesium metal with excess hydrochloric acid, what volume of hydrogen gas will be produced by the reaction if the lab occurs at 25.0oC and 765 torr? (Hint: write a balanced chemical reaction first and do stoichiometry, then use the ideal gas law)

Step 1. Write and balance the equation.
Mg + 2HCl ==> MgCl2 + H2
Step 2. Convert g Mg to mols Mg = 2.75 g/atomic mass Mg = ?
Step 3. Convert mols Mg to mols H2 produced using the coefficients in the balanced equation. ?mols Mg from step 2 x (1 mols H2/1 mol Mg) = ?
Then use PV = nRT and plug mols Mg in for n. Solve for V in L. Remember to use T in kelvin. If you use R as 0.08206 then convert pressure to atm.
Post your work if you get stuck.