For the following Reaction:
2AgNO3 + CaBr2 = 2AgBr + CaN2O6
If a chemist starts with 12.0g AgNO3, how many grams of CaBr2 must be added to use up all of the AgNO3?
See the post just above. Same procedure.
To find out how many grams of CaBr2 must be added to use up all of the AgNO3, we need to determine the stoichiometry of the reaction.
Stoichiometry is the relationship between the amounts of reactants and products in a chemical reaction. It is based on the balanced chemical equation, which shows the ratios of reactants and products.
In this case, the balanced chemical equation is:
2AgNO3 + CaBr2 → 2AgBr + Ca(N2O6)
From the balanced equation, we can see that the ratio between AgNO3 and CaBr2 is 2:1, meaning that for every 2 moles of AgNO3, we need 1 mole of CaBr2 to fully react.
To determine the number of moles of AgNO3, we can use the molar mass of AgNO3, which is 169.87 g/mol.
Moles of AgNO3 = mass (g) / molar mass (g/mol)
Moles of AgNO3 = 12.0 g / 169.87 g/mol
Now, since we know the stoichiometric ratio between AgNO3 and CaBr2 is 2:1, we can find the number of moles of CaBr2 needed using the moles of AgNO3.
Moles of CaBr2 = (moles of AgNO3) / 2
Finally, we can convert the moles of CaBr2 to grams using the molar mass of CaBr2, which is 199.89 g/mol.
Mass of CaBr2 = moles of CaBr2 × molar mass of CaBr2
Now you can substitute the value you calculated to find the mass of CaBr2 needed to use up all of the AgNO3.