Question

9. A 32.0 g sample of water at 15.0 oC absorbs 960 cal of heat. What...

9. A 32.0 g sample of water at 15.0 oC absorbs 960 cal of heat. What is the new temperature of the water? (4 pts.)

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the final temperature (in oC) of a 38 g sample of aluminum (specific heat...
What is the final temperature (in oC) of a 38 g sample of aluminum (specific heat = 0.900 J/(g K)) which absorbs 89.9 kJ of heat when it warms from 74.6oC?
The heat of fusion of water is 79.9 cal/g, the heat of vaporization of water is...
The heat of fusion of water is 79.9 cal/g, the heat of vaporization of water is 540 cal/g, and the specific heat of water is 1.00 cal/deg/g. How many grams of ice at 0 ° could be converted to steam at 100 °C by 9,076 cal of heat?
suppose the specific heat of ice and water is 0.49 cal/g. C ( C represent degree...
suppose the specific heat of ice and water is 0.49 cal/g. C ( C represent degree Celsius) and 1.0 cal/g. C. the latent heat of fusion of water is 80 cal/g. how much heat (in calories) is required for 100 grams of ice with an initial temperature of -10 C to a. raise the ice's temperature to the melting point? b. then completely melt the ice to water? c. finally, raise the water's temperature to 50 C?
A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC....
A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC. The calorimeter contains 42.3 g of deoinized water. The initial temperature of the water is 22.3 oC. The metal is transferred to the calorimeter and the final temperature reached by the water + metal is 32.2 oC. A. Calculate ∆T for the water (Tfinal – Tinitial). B. Calculate ∆T for the metal. C. The specific heat of water is 4.18 J/goC. Calculate the specific...
Suppose the latent heat of vaporization of water is 540 cal/g. how much heat (in calories)...
Suppose the latent heat of vaporization of water is 540 cal/g. how much heat (in calories) must be added to 50 grams of water at an initial temperature of 20 C ( C represent degree Celsius) to a. heat it to the boiling point? b. then completely convert the water to steam?
803 cal of heat is added to 5.00 g ice at –20.0 °C. What is the...
803 cal of heat is added to 5.00 g ice at –20.0 °C. What is the final temperature of the water? SPecific heat H2O(s)= 2.087 J/(g*C) Specific heat H2O(l)=4.184 J/(g*C) Heat of fusion= 333.6 J/g
Water (2190 g ) is heated until it just begins to boil. If the water absorbs...
Water (2190 g ) is heated until it just begins to boil. If the water absorbs 5.29×10 to the 5th power Jules of heat in the process, what was the initial temperature of the water? Specific heat capacity for water is 4.184 J/(g*c)
Water's heat of fusion is 80. cal/g, and its specific heat is 1.0 cal/g.celsius. Some velomobile...
Water's heat of fusion is 80. cal/g, and its specific heat is 1.0 cal/g.celsius. Some velomobile seats have been designed to hold ice packs inside their cushions. If you started a ride with ice packs that held 1200 of frozen water at 0 celsius , and the temperature of the water at the end of the ride was 32 celsius , how many calories of heat energy were absorbed?
A 15.0 g sample of CaCl2(110.98 g/mol) is dissolved in 175 g of water initially at...
A 15.0 g sample of CaCl2(110.98 g/mol) is dissolved in 175 g of water initially at 23.5 degrees C. The final temperature of this solution is 37.6 degrees C. Assuming no heat loss to the surroundings, calculate the amount of heat released in this experiment. CaCl2 (s) --> Ca^2+ (aq) + 2Cl^- (aq)
5. Heat Transfer: Calculate the heat transferred by the faucet water to the ice water in...
5. Heat Transfer: Calculate the heat transferred by the faucet water to the ice water in #4 above: (a) Use the following equation: Where, Cwater is the specific heat capacity of water = 1 cal/(gram oC) mwater is the mass the faucet water added in #4 (b) ΔT is the temperature change of the water [(#2(a) - #4(b)) temperatures] Calculation: SHOW WORK Result: Q = ____________________ cal Convert the value of Q into joules: (1 calorie = 4.2 joules) Q...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT