Answer: Correct answer is approximately 120 grams of oxygen will be needed to produce 2.5 moles of water in this reaction.
Explanation: Certainly! Let’s break down the given reaction:
[ B_2H_6 + O_2 \rightarrow HBO_2 + H_2O ]
From the balanced equation, we can see that 1 mole of B2H6 reacts with 3 moles of O2 to produce 2 moles of H2O.
Given that you want to produce 2.5 moles of water, we can set up a proportion:
(\frac{{2.5 , \text{{moles of H2O}}}}{{2 , \text{{moles of B2H6}}}} = \frac{{x , \text{{moles of O2}}}}{{3 , \text{{moles of O2}}}})
Solving for (x):
[ x = \frac{{2.5 \times 3}}{{2}} = 3.75 , \text{{moles of O2}} ]
Now let’s convert moles of oxygen to grams. The molar mass of oxygen (O2) is approximately 32 g/mol:
[ \text{{Mass of O2}} = 3.75 , \text{{moles of O2}} \times 32 , \text{{g/mol}} = 120 , \text{{grams of O2}} ]
Therefore, approximately 120 grams of oxygen will be needed to produce 2.5 moles of water in this reaction
