What is the mass of aluminum metal that reacts to give 1.00 g of hydrogen gas? __Al(s)+ __HCl(aq)→ __AlCl3(aq)+ __H₂(g)

Question

Quizplus · Accepted Answer

To find the mass of aluminum that reacts, we need to use stoichiometry. From the balanced chemical equation, we know that the molar ratio between aluminum and hydrogen is 2:3 (i.e. 2 moles of aluminum react with 3 moles of hydrogen to produce 3 moles of H₂).

Let x be the mass of aluminum that reacts to give 1.00 g of H₂. We can set up the following equation:

(1.00 g H₂) x (1 mol H₂/2 g H₂) x (2 mol Al/3 mol H₂) x (26.98 g Al/1 mol Al) = x

Simplifying this, we get:

x = 8.94 g Al

Therefore, the mass of aluminum that reacts to give 1.00 g of H₂ is 8.94 g, which is closest to option B (8.90 g).

What Is the Mass of Aluminum Metal That Reacts to Give