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When aqueous solutions of (NH4)2CrO4 and Ba(NO3 )2 are combined, BaCrO4 precipitates. Calculate the mass, in grams, of the BaCrO4 produced when 2.76 mL of 0.19 M Ba(NO3 )2 and 3.86 mL of 0.716 M (NH4)2CrO4 are mixed. Calculate the mass to 3 significant figures

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Oseni

The mass, in grams of BaCrO4 that will be produced, according to the illustration, would be 0.1329 grams

Stoichiometric calculations

From the equation of the reaction:

Ba(NO3)2 + (NH4)2CrO4 → BaCrO4 + 2(NH4)NO3

The mole ratio of the reactants is 1:1.

Mole of (NH4)2CrO4 = 3.86/1000 x 0.716

                                       = 0.0028 moles

Mole of Ba(NO3 )2 = 2.76/1000 x 0.19

                               = 0.0005 moles

Thus, Ba(NO3 )2 is limiting in availability.

Mole ratio of Ba(NO3 )2 and BaCrO4  = 1:1

Mole equivalent of BaCrO4  = 0.0005 moles

Mass of 0.0005 moles BaCrO4  = 0.0005 x 253.37

                                                        = 0.1329 grams

More on stoichiometric calculations can be found here: https://brainly.com/question/8062886

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