If you mix 40.0 mL of a 0.200 M solution of K2CrO4 is reacted with 40.0 mL of a 0.200 M solution of AgNO3, what mass of solid forms?
Group of answer choices
1.79 g
2.65 g
0.896 g
1.33 g
none of these
To determine the mass of solid formed, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between K2CrO4 and AgNO3:
2 K2CrO4 + 3 AgNO3 -> Ag2CrO4 + 2 KNO3
From the balanced equation, we can see that for every 2 moles of K2CrO4, we produce 1 mole of Ag2CrO4.
First, let's calculate the number of moles of K2CrO4 and AgNO3 in the given solutions:
Number of moles of K2CrO4 = (volume of solution in L) * (molarity of solution in mol/L)
= (40.0 mL / 1000 mL/L) * 0.200 mol/L
= 0.008 mol
Number of moles of AgNO3 = (volume of solution in L) * (molarity of solution in mol/L)
= (40.0 mL / 1000 mL/L) * 0.200 mol/L
= 0.008 mol
From the stoichiometry of the balanced equation, we know that the number of moles of Ag2CrO4 formed is half the number of moles of K2CrO4 used:
Number of moles of Ag2CrO4 formed = 0.008 mol / 2
= 0.004 mol
To find the mass of Ag2CrO4 formed, we need to convert the number of moles to grams using the molar mass of Ag2CrO4:
Molar mass of Ag2CrO4 = (2 * atomic mass of Ag) + atomic mass of Cr + (4 * atomic mass of O)
= (2 * 107.87 g/mol) + 52.00 g/mol + (4 * 16.00 g/mol)
= 331.74 g/mol
Mass of Ag2CrO4 formed = (number of moles of Ag2CrO4) * (molar mass of Ag2CrO4)
= 0.004 mol * 331.74 g/mol
= 1.327 g
Therefore, the mass of solid formed is 1.327 g. None of the provided answer choices match this result, so the correct answer cannot be determined from the given options.