![]() To do that, use their respective molar masses Your next step will be to determine how many moles of each reactant you get in those #"83.0-g"# samples. ![]() Sulfur dioxide, #"SO"_2#, and hydrogen sulfide, #"H"_2"S"#, will react in a #color(red)(1):color(blue)(2)# mole ratio, which means that the reaction will always consume twice as many moles of hydrogen sulfide as you have moles of sulfur dioxide taking part in the reaction. Start by taking a look at the balanced chemical equation for this reaction ![]() The idea here is that you need to use the mole ratio that exists between the two reactants to determine whether or not you're dealing with a limiting reagent.
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