A50.51g sample of a compound made from phosphorus and chlorine is decomposed. analysis of the products showed that 11.39 g of phosphorus atoms were produced. answer using three significant figures. what is the percent by mass of phosphorus? % what is the percent by mass of chlorine? %

mass of phosphorus (P) = 11.39g

mass of chlorine (CL)  =  mass of compound - mass of phosphorus

                                         50.51 - 11.39 = 39.12g

atomic mass of P : CL  =    ( 11.39 / 31 ) :  (39.12 / 35.5)  =  1  :   3

mass of p%  =   11.39/31 * 100 =    36.7 %

mass of CL%  =   39.12 / 35.5 * 100=  110 %

empirical formula :-  PCl3

The percent by mass of phosphorus is 22.5%.

The percent by mass of chlorine is 77.5%.

Explanation:

Amount of compound made from phosphorus and chlorine, M = 50.51 g

Amount of  phosphorus atoms were produced,x = 11.39 g

The percent by mass of phosphorus:

The percent by mass of chlorine:

= 100% - (percent by mass of phosphorus)%=100 % -22.5% = 77.8 %

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error