Question

6 moles of YCl3 were reacted with BaS.

a) how many moles of BaS were needed?
b) how many moles of BaCl2 were formed?
c) how many g of Y2S3 are formed?

Answer 1

For 6 moles of YCl₃, 6 moles of BaS are needed, and this reaction will produce 6 moles of BaCl₂. The mass of Y₂S₃ can be calculated using the balanced chemical equation and its molar mass.

Step-by-step explanation:

The student asked how many moles of BaS were needed to react with 6 moles of YCl₃, how many moles of BaCl₂ were formed, and the mass of Y₂S₃ formed from the reaction.

1. According to the stoichiometry of the reaction, for each mole of YCl₃, one mole of BaS is required. So, for 6 moles of YCl₃, you will also need 6 moles of BaS.
2. Since there is a 1:1 ratio in the reaction for YCl₃ to BaCl₂, 6 moles of YCl₃ will produce 6 moles of BaCl₂.
3. To find the mass of Y₂S₃ formed, we require balanced chemical equations and molar masses. We would use the molar mass of Y₂S₃ and the stoichiometry from the balanced equation (not provided here) to calculate the mass from the moles of YCl₃ reacted.