Based on the following balanced equation,how many moles of SF₆ can form from the combination of 5 moles of S and 18 moles of F₂? S + 3 F₂ $\rightarrow$ SF₆

Question

Quizplus · Accepted Answer

The balanced equation shows that it takes 1 mole of S and 3 moles of F₂ to produce 1 mole of SF₆. Therefore, to determine how many moles of SF₆ can be produced from the given amounts, we need to find the limiting reactant. Using the amount of S (5 moles), we can calculate the amount of F₂ needed to react with all of the S: 5 moles S × (3 moles F₂/1 mole S) = 15 moles F₂ needed However, we are given that there are only 18 moles of F₂ available. This means that F₂ is the limiting reactant and we can only produce as much SF₆ as the amount that would be produced by 18 moles of F₂. Using the ratio from the balanced equation, we can calculate this amount: 18 moles F₂ × (1 mole SF₆/3 moles F₂) = 6 moles SF₆ Therefore, the best choice is B) 5 moles of S can form 6 moles of SF₆.

Based on the Following Balanced Equation,how Many Moles of SF6 →\rightarrow→

Based on the Following Balanced Equation,how Many Moles of SF₆ $\rightarrow$