Asked by Katie
Please help me.
1. A chemist adds 25.0 mL of a 43.4 g/dL iron (ii) bromide (FeBr2) solution to a flask. Calculate the mas in gram of iron (ii) bromise the chemist has added to the flask.
2. A certain substance X has a normal boiling point of 100.3 C and molal boiling point elevation constant, kb=0.87 C*kg*mol. Calculate the boiling point of a solution made of 26.96 g of urea (NH2)2CO) dissolved in 550 g of X.
1. A chemist adds 25.0 mL of a 43.4 g/dL iron (ii) bromide (FeBr2) solution to a flask. Calculate the mas in gram of iron (ii) bromise the chemist has added to the flask.
2. A certain substance X has a normal boiling point of 100.3 C and molal boiling point elevation constant, kb=0.87 C*kg*mol. Calculate the boiling point of a solution made of 26.96 g of urea (NH2)2CO) dissolved in 550 g of X.
Answers
Answered by
DrBob222
43.4 g/dL x (10 mL/dL) = ? g/mL then that times 25.0 mL = ? g
delta T = Kb*molality
m = mols/kg solvent and
mols = grams/molar mass. Solver for mols, then solver for m, then for delta T.
Add delta T to 100.3 = boiling point of new solution
Post your work if you get stuck.
delta T = Kb*molality
m = mols/kg solvent and
mols = grams/molar mass. Solver for mols, then solver for m, then for delta T.
Add delta T to 100.3 = boiling point of new solution
Post your work if you get stuck.
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