How do I find the rest of the calculations with results I already have? mass of

ID: 909971 • Letter: H

Question

How do I find the rest of the calculations with results I already have?

mass of coffee cup 3.86 g

mass of coffee cup and water 168.42 g

mass of water 164.55 g

moles of water ?

mass of coffee cup, water and melted ice 189.05 g

mass of ice 20.63 g

moles of ice ?

Initial temperature 21.9 degrees celcius

final temperature 10.6 degrees celcius

delta change of water ?

heat lost by water (qwater) (J) ?

deltaH/mol water (kJ/mol) ?

heat gained by ice (qice) (J) ?

DeltaT of melted Ice ?

heat needed to warm melted ice (qwarming) (J)?

heat needed to melt ice (qmelting) (J) ?

deltaHfusion/mol ice (kJ/mol)?

moles of water = 164.55 /18 = 9.142 mol

moles of ice = 20.63/18 = 1.146 mol

DT of water = 21.9-10.6 = 11.3 c

heat lost by water (qwater) = m*S*DT

m = mass of water = 164.55 g

s = specificheat of water = 4.18 j/g.c

DT = 11.3 C

heat lost by water = 164.55*4.18*11.3 = 7.77 kj

deltaH/mol water (kJ/mol) = 7.77/9.142 = 0.85 kj/mol

heat gained by ice (qice) (J) = 7.77 kj = 1.146*sice*DT

s = specifcheat of ice = 2.03 j/g.c

DeltaT of melted Ice = 7.77/(1.146*2.03) = 3.34c

heat needed to warm melted ice (qwarming) (J)?

7.77*10^3 = qwarming + 1.146*6.01

qwarming = 7.763 kj

heat needed to melt ice (qmelting) (J) = 1.146*6.01 = 6.9 joule

deltaHfusion/mol ice (kJ/mol) = 6.01 kj/mol

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.