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Chemistry
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1. What theoretical quantity of Ag2S can be obtained from thereaction of 10.5 g of Ag with 7.5 g of S in the followingreaction?


2Ag+S=Ag2S


2. What is the percentyield if a chemist actually obtains 9.8 g of Ag2S in thelaboratory?

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Nestor Rutherford
Nestor RutherfordLv2
21 Apr 2019
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Related questions

silver tarnish is the result of slver metal reacting with sulfurcompounds, such as H2S, in the air. the tarnish on silverware(Ag2S) can be removed by soaking in a solution of NaHCO3(bakingsoda) in a basin lined with aluminum foil.


1/ write a balanced equation for the tarnishing of Ag2S. do notinclude phases


2/ how many electrons are transferred per mole of silver ??


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a. How many moles of Ag2S are needed to produce6.50 moles of Al2S3 in the above equation ?

b. How many grams of Al2S3 can be produced from4.00 moles of Al in the above equation?

2. Find the molarity of a solution that contains 17g of NH3 in0.50 L of solution ?

3. What volume of a 2.00 M KCl solution is required to prepare500. ml of a 0.100 M KCl ?

64. As long as Keq > 1, all reactants will eventually be consumed and leave us exclusively with product molecules. (T?F)

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A. 0.10

B. 0.015

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