Question

magnesium metal reacts with aqueous hydrochloric acid to form hydrogen gas and aqueous magnesium chloride. Mg(s)+2HCl(aq)=MgCl2(aq)+H2(g)

A student performs this reaction in a laboratory and collects the hydrogen gas over water. The student collects 215.8mL of gas at a pressure of 755.2mmHg and a temperature of 22 degrees C.

(here are some answers I found already correct me if I am wrong)

I found the water pressure at 22 degrees C to be 19.8mmHg

I found the partial pressure of the hydrogen in the tube to be 735.4mmHg or 0.968atm

Using the ideal gas law to calculate moles of hydrogen produced in the reaction I got 0.0086 mol H2.

I need help with these questions.

How many moles of Mg reacted? (assume 100% yield)

What mass of Mg reacted?