Recent content by trying_mybest

Thank you! I caught that mistake earlier, fixed it, and got the correct answer.

m1 = 5 gal * 3.79 L/gal * 1000 g/L = 18,750 g m2 = 50 gal * 3.79 L/gal * 1000 g/L = 187,500 g m1*C*(Tf - T1) = m2*C*(Tf - T2) m1CTf - m1CT1 = m2CTf - m2CT2 m1CTf - m2CTf = m1CT1 - m2CT2 Tf(m1 - m2) = m1T1 - m2T2 Tf = (m1T1 - m2T2) / (m1 - m2) Tf = (18,750*212 - 187,500*50) / (18,750 -...

Final temp should be ˚C. I used m1C∆T1 = m2C∆T2 I keep getting 0 for the final temp when it's supposed to be 18 C

Not really sure how to start this one.

My first attempt, the initial temp was 23.3, but then the second attempt was 25.6. I will make that correction on my calculation. Thank you so much for all the help!

This is what I think it should be: Qheat H2O lost = Qice to reach 0 C + Qmelt ice Qheat H2O lost = mH2O * Cv,H2O * ∆TH2O Qheat H2O lost = [0.25 L * 1000 g/1L] * (4.184 J/g*K) * (0-23.3) = -24,372 J Qice to reach 0 C = mice * Cv,ice * ∆Tice Qice to reach 0 C = (4 * 11) * (2.108 J/g*K) *...

This is the procedure. "Take a large glass or a bowl and fill it with 0.5 liter of water at room temperature, (or let it sit until it is at room temperature) Then estimate how many ice cubes (from your freezer) you think it will take to bring the glass or bowl with 1/2 liter of water down to 0...

Because I don't have a thermometer to measure it accurately, I'm making the assumption that the final temperature is 0˚ C since that's when the ice stopped melting. Also I redid the experiment. The initial temp of the water was 25.6 ˚C. I ended up using 11 ice cubes before the next one was...

The ice does the phase change I believe.

Q1 = m(ice) * Cv * ∆T = amount of heat the ice absorbs Q2 = m(H2O) * Lf = amount of heat the water loses Q1 = (4*8 g) * (2198 J/g*K) * (0-(-15)) = 1.055 * 10^6 J Q1=Q2 Q2 = 1.055 * 10^6 J = m(H2O) * Lf Lf = 1.055 * 10^6 J / m(H2O) = 1.055 * 10^6 J / (0.25 L * 1000 g/1L) = 4220 J/g My answer is...