A 1.740 ATORY QUESTIONS\ completion

1.70gram

sample of silver was burnt in an atmosphere of sulphur gas. Upon experimental the reaction 2.000 grams of silver sulphide was obtained. Determine the Burnt simpirical formula based upon this data.\ Sulfide silver

=1.740g

\

{(: ebtained =2.00g):}\ {(:=2.000g-1.740g=0.260g):}\ Mass Sulfur \ molar mass sulfur \ 2Ag+S->A_(g)S\ sulfur (0.260)/(32(g)/(m)ol)=0.0081mol\ silver =1.740(9)/(108gmol)=0.016m^(3)l

\ Write a balanced equation for the reaction between silver and sulphur as determined in question #1.

RY QUESTIONS experiment of the reaction 2.000 grams of silver sulphide was obtained. Determine the Burnt sinpirical formula based upon this data. Sulfide silver =1.740g Sulfideobtained=2.00g=2.000g1.740g=0.260g2Ag+Sg molarmasssulfurMasssulfur sulfur 32g/mol0.260=0.0081mol silver =1.740108gmm19=0.016m 2. Write a balanced equation for the reaction between silver and sulphur as determined in question \#1. RY QUESTIONS experiment of the reaction 2.000 grams of silver sulphide was obtained. Determine the Burnt sinpirical formula based upon this data. Sulfide silver =1.740g Sulfideobtained=2.00g=2.000g1.740g=0.260g2Ag+Sg molarmasssulfurMasssulfur sulfur 32g/mol0.260=0.0081mol silver =1.740108gmm19=0.016m 2. Write a balanced equation for the reaction between silver and sulphur as determined in question \#1