Question

If 133.2 kJ of heat are added to 5.80 × 102 g of water at 22.0°C,...

If 133.2 kJ of heat are added to 5.80 × 102 g of water at 22.0°C, what is the final temperature of the water? Specific heat of water at 1.00 atm and 20.0°C is 4.186 kJ/kg·K.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Specific of water is given as 4.186 kJ/Kg.K which means it will take 1kJ of energy to heat up 1Kg of water to raise its temperature by 1 degrees (Kelvin or celcius).

In this type of questions we use the formula to calculate the energy which is:

Now we are given E=133.2 KJ so,

So change(rise) in temperature is 54.9 oC. Hence the final temperature Tf is:

So final temperature is about 77o C or more precisely 76.9oC.

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
1. If 121.4 kJ of heat are added to 6.10 × 102 g of water at...
1. If 121.4 kJ of heat are added to 6.10 × 102 g of water at 22.0°C, what is the final temperature of the water? Specific heat of water at 1.00 atm and 20.0°C is 4.186 kJ/kg·K. (Refer to Table 14.1.) 2. It takes 880 J to raise the temperature of 350 g of lead from 0°C to 20.0°C. What is the specific heat of lead? 3. A 4.00-kg steel ball at 27.3°C is dropped from a height of 10.8...
Question1: If 2.72 kJ of heat are supplied to 2.4 × 102 g of water at...
Question1: If 2.72 kJ of heat are supplied to 2.4 × 102 g of water at 25 °C, what is the final temperature of the water? Question 2: Compute the heat of fusion from these data. 21.08 kJ will change  0.33 kg of the solid at 18.5 oC to 327 o C., the melting point. Specific heat capacity of solid :0.129 KJ/KgK. Give your answer as a positive number. please solve both, I need them!!!!
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
An 100-g aluminum calorimeter contains 280 g of water at an equilibrium temperature of 20°C. A...
An 100-g aluminum calorimeter contains 280 g of water at an equilibrium temperature of 20°C. A 170-g piece of metal, initially at 277°C, is added to the calorimeter. The final temperature at equilibrium is 32°C. Assume there is no external heat exchange. The specific heats of aluminum and water are 910 J/kg·K and 4190 J/kg·K, respectively. The specific heat of the metal is closest to: a) 270 J/kg·K. b) 240 J/kg·K. c) 330 J/kg·K. d) 390 J/kg·K. e) 360 J/kg·K.
1) A certain substance has a heat of vaporization of 36.02 kJ/mol.36.02 kJ/mol. At what Kelvin...
1) A certain substance has a heat of vaporization of 36.02 kJ/mol.36.02 kJ/mol. At what Kelvin temperature will the vapor pressure be 3.503.50 times higher than it was at 347 K? 2) A total of 767 cal767 cal of heat is added to 5.00 g5.00 g of ice at −20.0 °C.−20.0 °C. What is the final temperature of the water? Specific heat of H2O(s)H2O(s) 2.087 J/(g⋅°C)2.087 J/(g⋅°C) Specific heat of H2O(l)H2O(l) 4.184 J/(g⋅°C)4.184 J/(g⋅°C) Heat of fusion for H2OH2O 333.6...
If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane under 1...
If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane under 1 atm of pressure at a temperature of -170 ∘C, what is the final state of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5 ∘C. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J/g⋅K, respectively. Why is it be gas veres liqiud? also What is the final...
You add 50.0 g of ice initially at ‒20.0 °C to 1.00 x 102 mL warm...
You add 50.0 g of ice initially at ‒20.0 °C to 1.00 x 102 mL warm water at 67.0 °C. When all the ice melts, the water temperature is found to be somewhere above 0 °C. Calculate the final temperature of the water. [ Cice = 2.06 J/g⋅°C; CH2O = 4.184 J/g⋅°C; dH2O = 1.00 g/mL; heat of fusion of water = 333 J/g ]
A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C....
A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K). a. 40.8°C b. 61.0°C c. 39.6°C d. 82.4°C e. 79.2°C
A 190 g copper bowl contains 230 g of water, both at 22.0°C. A very hot...
A 190 g copper bowl contains 230 g of water, both at 22.0°C. A very hot 430 g copper cylinder is dropped into the water, causing the water to boil, with 6.44 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat...
A 110 g copper bowl contains 100 g of water, both at 22.0°C. A very hot...
A 110 g copper bowl contains 100 g of water, both at 22.0°C. A very hot 360 g copper cylinder is dropped into the water, causing the water to boil, with 7.52 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT