(adsbygoogle = window.adsbygoogle || []).push({}); Calculating Molal Boiling point elevation constant!! HELP!

So here's how I did my problem, but the answer I arrived with is wrong. I need help with this....

Carbon disulfide (CS2) boils at 46.30°C and has a density of 1.261g/mL.

When 0.250 mol of a nondissociating solute is dissolved in 400.0 mL of CS2, the solution boils at 47.46°C. What is the molal boiling point elevation constant for CS2?

1. The problem statement, all variables and given/known data

Normal Boiling Point: 46.3°C

0.250mol of solute

400.0mL of CS2 (solvent)

2. Relevant equations

ΔT[itex]_{b}[/itex]=k[itex]_{b}[/itex](molality)

3. The attempt at a solution

ΔT[itex]_{b}[/itex]=47.46-46.30=1.16°C

molality = 0.250mol/0.400kg = 0.625m

k[itex]_{b}[/itex]= ΔT[itex]_{b}[/itex]/molality.

k[itex]_{b}[/itex]=1.16°C/0.625=1.856.

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# Homework Help: Calculating Molal Boiling point elevation constant HELP!

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