QUESTION 1 How much energy in kJ is needed to heat 8.36 g of ice from -10.0 °C t

Question

QUESTION 1 How much energy in kJ is needed to heat 8.36 g of ice from -10.0 °C to 30.0 °C? The heat of fusion of water is 6.02 kJ/mol, and the heat capacity is 2.03 J/g °C for ice and 4.18 J/g °C for liquid water.

iPad 8:00 PM * 70% Old Unit 1 Test #1: Attempt 1 ¥ Question Completion Status: UESTION 13 Fill the correct sign (+) or(-)for AH and AS for the following processes Dissolve NaOH(s) in water (note: solution warms) A·dH (+) and AS (+) Sublimation of dry ice, CO2(s) à CAH and AS(+) Formation of snow in a cloud D.AH(+) and AS(- Dissolve NH4CI(S) in water (note: solution cools) Your lab goggles fog up (water condenses on the lens) Click Save and Submit to save and submit. Click Save All Answers to save all answers Save All Answers Close Window Save and Submit

Explanation / Answer

1) using q = (m) (t) (Cp, metal)

Where, (t) = temperature change
Cp =specific heat of the ice
m = mass of the ice

Substitute the respective values in the eqation, we get:

q = 8.63 g x (30 - (-10))°C x 2.03 J/g °C

= 700.75 J

= 0.700 kJ

Related Questions

Navigate

• Browse (All)
• Browse Q
• Subjects

---

---

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