Calcium hydroxide (“slaked lime”) and sulfuric acid react to produce calcium sulfate and water according to the following balanced equation:
Ca(OH)2 (aq) + H2SO4 (aq) -> CaSO4 (s) + 2 H2O (l)
Our H2SO4 solution is 0.5 M and we end up titrating (adding) 50 mL to an excess amount of Ca(OH)2 in H2O. Using the molarity and volume, how much CaSO4 do we end up producing in grams?
Answers: 2
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From the options provided for each element below, choose the properties that it may have based on its location in the periodic table fluorine (f): highly reactive nonmetal shiny a conductor
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Consider the reaction of a(g) + b(g) + c(g) => d(g) for which the following data were obtained: experiment initial [a], mol/l initial [b], mol/l initial [c], mol/l initial rate, mol/l. s 1 0.0500 0.0500 0.0100 6.25 x 10^-3 2 0.100 0.0500 0.0100 2.50 x 10^-2 3 0.100 0.100 0.0100 1.00 x 10^-1 4 0.0500 0.0500 0.0200 6.25 x 10^-3 what is the rate law for the reaction?
Answers: 3
Calcium hydroxide (“slaked lime”) and sulfuric acid react to produce calcium sulfate and water accor...
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