Question

How many grams of ice at -14°C must be added to 710 grams of water that...

How many grams of ice at -14°C must be added to 710 grams of water that is initially at a temperature of 81°C to produce water at a final temperature of 12°C. Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg·C° and of ice is 2050 J/kg·C°. For water the normal melting point is 0.00°C and the heat of fusion is 334 × 103 J/kg. The normal boiling point is 100°C and the heat of vaporization is 2.26 × 106 J/kg.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
How many grams of ice at -13°C must be added to 714 grams of water that...
How many grams of ice at -13°C must be added to 714 grams of water that is initially at a temperature of 83°C to produce water at a final temperature of 11°C. Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg·C° and of ice is 2050 J/kg·C°. For water the normal melting point is 0.00°C and the heat of fusion is 334 × 103...
How many grams of ice at -13°C must be added to 711 grams of water that...
How many grams of ice at -13°C must be added to 711 grams of water that is initially at a temperature of 87°C to produce water at a final temperature of 10°C? Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg • C° and of ice is 2100 J/kg • C°. For water the normal melting point is 0.00°C and the heat of fusion...
You have a pitcher with 2.00 L of water at an initial temperature of 12.0 oC...
You have a pitcher with 2.00 L of water at an initial temperature of 12.0 oC and you wish to add ice to it to bring the temperature down. If the ice starts at an initial temperature of T1 = -18.4 oC, calculate the mass of ice required to reach a final state of all liquid water at 0.00 oC. *****Assume no heat is gained or lost to the surroundings.***** More information: Melting point of water - 0.00 degrees celcius...
How much energy is required to change a 34 g ice cube from ice at −10◦C...
How much energy is required to change a 34 g ice cube from ice at −10◦C to steam at 119◦C? The specific heat of ice is 2090 J/kg · ◦ C, the specific heat of water is 4186 J/kg · ◦ C, the specific heat of stream is 2010 J/kg · ◦ C, the heat of fusion is 3.33 × 105 J/kg, and the heat of vaporization is 2.26 × 106 J/kg. Answer in units of J
An insulated beaker with negligible mass contains a mass of 0.200 kg of water at a...
An insulated beaker with negligible mass contains a mass of 0.200 kg of water at a temperature of 81.7 ∘C. How many kilograms of ice at a temperature of − 21.1 ∘C must be dropped in the water to make the final temperature of the system 30.8 ∘C? Take the specific heat for water to be 4190 J/(kg⋅K) , the specific heat for ice to be 2100 J/(kg⋅K) , and the heat of fusion for water to be 334 kJ/kg...
100. g of ice at 0 degrees C is added to 300.0 g of water at...
100. g of ice at 0 degrees C is added to 300.0 g of water at 60 degrees C. Assuming no transfer of heat to the surroundings, what is the temperature of the liquid water after all the ice has melted and equilibrium is reached? Specific Heat (ice)= 2.10 J/g C Specific Heat (water)= 4.18 J/g C Heat of fusion = 333 J/g Heat of vaporization= 2258 J/g
If you pour 0.600 kg of 20.0ºC water onto a 1.20-kg block of ice (which is...
If you pour 0.600 kg of 20.0ºC water onto a 1.20-kg block of ice (which is initially at 0 ºC), what is the final temperature? You may assume that the water cools so rapidly that effects of the surroundings are negligible. The specific heat of water is 4 186 J/(kg * ºC), the specific heat of ice is 2 090 J/(kg * ºC), and the heat of fusion of water is 334 x103 J/kg.
Adding Ice to Water An insulated beaker with negligible mass contains liquid water with a mass...
Adding Ice to Water An insulated beaker with negligible mass contains liquid water with a mass of 0.340 kg and a temperature of 66.3 ∘C . How much ice at a temperature of -17.9 ∘C must be dropped into the water so that the final temperature of the system will be 22.0 ∘C ? Take the specific heat of liquid water to be 4190 J/kg⋅K , the specific heat of ice to be 2100 J/kg⋅K , and the heat of...
A 60 kg block of ice begins at -60 degrees the specific heat of ice is...
A 60 kg block of ice begins at -60 degrees the specific heat of ice is 2090 j/(kg)C. The latent heat of fusion of water is 3.3 x 10^5 and the latent heat of vaporization is 2.3 x 10^6 J/kg. How much energy is required to heat the ice to 0 degrees Celcius (melting point)? How much energy is required to heat the ice from -50C to the melting point and melt the ice? How much energy is required to...
What mass of steam at 100°C must be mixed with 216 g of ice at its...
What mass of steam at 100°C must be mixed with 216 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 65.0°C? The specific heat of water is 4186 J/kg·K. The latent heat of fusion is 333 kJ/kg, and the latent heat of vaporization is 2256 kJ/kg.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT