Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) What mass of H2(g) is produced from the reaction of 0.75 g Al(s) with excess hydrochloric acid?
Added by Mary O.
Step 1
The molar mass of Al is approximately 26.98 g/mol and the molar mass of H2 is approximately 2.02 g/mol. Show more…
Show all steps
Your feedback will help us improve your experience
Ma Ednelyn Lim and 73 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
When aluminum reacts with concentrated hydrochloric acid, hydrogen gas is produced. 2Al(s) + 6HCl(aq) ⟶ 2AlCl3(aq) + 3H2(g) What mass of Al(s) is required to produce 698.5 mL of H2(g) at STP?
Dr. Satish I.
What mass of hydrogen can be produced by reacting 6.0 moles of aluminum (Al) with enough hydrochloric acid (HCl)? Al + HCl → AlCl3 + H2
Sri K.
Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and $35.8 \mathrm{~mL}$ of hydrogen gas over water at $27^{\circ} \mathrm{C}$ and $751 \mathrm{mmHg} .$ How many grams of aluminum react?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD