Question

According to this chemical reaction, calculate the number of moles of KBr (119.00 g/mol) that will be produced from 272.08 grams of BaBr2 (297.13 g/mol).

BaBr2 + K2SO4 --> 2KBr + BaSO4



Report your answer to the hundredths.

Answer 1

First, we need to find out how many moles of BaBr2 we have. We can do this by dividing the given mass by its molar mass:

Moles of BaBr2 = 272.08 g / 297.13 g/mol = 0.915 moles

From the balanced equation, we know that 1 mole of BaBr2 reacts with 2 moles of KBr. Therefore, we can use stoichiometry to find out how many moles of KBr will be produced:

Moles of KBr = 0.915 moles BaBr2 × (2 moles KBr / 1 mole BaBr2) = 1.83 moles KBr

Finally, we can use the molar mass of KBr to calculate its mass:

Mass of KBr = 1.83 moles × 119.00 g/mol = 217.77 g

Therefore, 272.08 grams of BaBr2 will produce 217.77 grams or 1.83 moles of KBr.