Question

At 1023 K and 1 atm, a 3.00 gram sample of Snoz(s) (gram-formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and water, as
shown in the balanced equation below:
SnO2 (s) + 2H2(g) + Sn(l) + 2H2O(g)
Determine the number
of moles of sn(l)
produced when 4.0
Moles of H2(g) is completely consumed

Answer 1

Answer:

2 moles of Sn are produced when 4 moles of H2(g) are consumed completely

Explanation:

to determine the number of moles of sn (l) produced when 4.0 moles of H2 (g) is consumed completely.

First, find the number of moles of H2 consumed by taking this as limiting reagent.

                                           $n = \frac{g}{M.W (g/mol)}$

Then find the moles of Sn (l) taking into account the stoichiometric relationship between H2(g) and Sn(l). 2:1

                          $SnO_{2}$ (s) + 2$H_{2}$(g)  ⇒  Sn(l) + 2$H_{2}O$(g)

                              $mol Sn(l) = \frac{1mol Sn}{2mol H_{2} } . 4 mol H_{2} = 2 mol$

∴2 moles of Sn are produced when 4 moles of H2(g) are consumed completely.