Question CI.21: A metal (M) completely reacts with 34.8 mL of a 0.520 M HCl ...
A metal (M) completely reacts with 34.8 mL of a 0.520 M HCl solution to form MCl_3(aq) and H_2 (g). (4.1, 7.2, 7.4, 7.7, 8.6,10.7)
a. Write the balanced chemical equation for the reaction of the metal M(s) and HCl(aq).
b. What volume, in milliliters, of H_2 is produced at STP?
c. How many moles of metal M reacted?
d. If the metal has a mass of 0.420 g, use your results from part c to determine the molar mass of the metal M.
e. What are the name and symbol of metal M in part d?
f. Write the balanced chemical equation using the symbol of the metal from part e.
a. 2 \mathrm{M}(s)+6 \mathrm{HCl}(a q) \longrightarrow 3 \mathrm{H}_2(g)+2 \mathrm{MCl}_3(a q)
b. 203 \mathrm{~mL} of \mathrm{H}_2
c. 6.03 \times 10^{-3} mole of \mathrm{M}
d. 69.7 \mathrm{~g} / \mathrm{mole}
e. gallium; \mathrm{Ga}
f. 2 \mathrm{Ga}(s)+6 \mathrm{HCl}(a q) \longrightarrow 3 \mathrm{H}_2(g)+2 \mathrm{GaCl}_3(a q)