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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: KurzickMushroom on February 19, 2009, 11:28:29 PM

Title: Limiting Reagent and Percentage Yield Problem
Post by: KurzickMushroom on February 19, 2009, 11:28:29 PM

Hello again, I have another problem that I have no idea how to do. Please help :)

A solution of 2.63 g of Triphenal Phosphine dissolves in 20 ml of the organic solvent which is CH2Cl2 is added to a solution of 3.5 ml of liquid SbCl5 dissolved in 10 ml of CH2Cl2. After cooling and adding ethers, a precipitate of [(C6H5)3PCL][SbCl6] is formed. The precipitate weighs 5.314 grams.

This is the only equation my teacher gave to me. I don't think it's enough to solve the question.

(C6H5)3P+ 2 SbCl5 --> [(C6H5)3PCL][SbCl6] + SbCl6

Questions:
1. If the density of SbCl5 is 2.33 g/ml which is limiting? ---I don't understand this since I thought it should be 2.33 g/mol not g/ml

2. Calculate percentage yield.

Thanks in advance.

Title: Re: Limiting Reagent and Percentage Yield Problem
Post by: macman104 on February 19, 2009, 11:59:05 PM

No, SbCl5 is a liquid.  So before you can convert to moles, you need grams, and to get grams, you need density.