If 50.0 mL of ethanol (density=0.789g/mL)) initially at 7.0 ∘C is mixed with 50.0 mL of...
If 50.0 mL of ethanol (density=0.789g/mL)) initially at 7.0 ∘C is mixed with 50.0 mL of water (density=1.0g/mL) initially at 28.7 ∘C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?
Homework Answers
heat lost by one system = heat gained by other system
q = msT
ethanol heat = water heat
(50*0.789)*2.46*(T2-7.0) = 50*4.184*(28.7 - T2)
T2 = 21.820C
Add Answer to:
If 50.0 mL of ethanol (density=0.789g/mL)) initially at 7.0 ∘C is mixed with 50.0 mL of...
If 45.0 mL of ethanol (density=0.789g/mL)) initially at 6.0 ∘C is mixed with 45.0 mL of...
If 45.0 mL of ethanol (density=0.789g/mL)) initially at 6.0 ∘C is mixed with 45.0 mL of water (density=1.0g/mL) initially at 28.2 ∘C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture? T = _______ ∘C
If 55.0 mL of ethanol ) initially at 8.0C is mixed with 55.0 ml of water...
If 55.0 mL of ethanol ) initially at 8.0C is mixed with 55.0 ml of water (density = 1.0g/mL) initially at 28.6C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?
If 46.9 mL of ethanol (density = 0.789 g/mL) initially at 7.2°C is mixed with 45.4...
If 46.9 mL of ethanol (density = 0.789 g/mL) initially at 7.2°C is mixed with 45.4 mL of water (density = 1.0 g/mL) initially at 28.5°C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?
22.7 mL of ethanol (density =0.789 g/mL) initially at 8.4 ?C is mixed with 30.5 mL...
22.7 mL of ethanol (density =0.789 g/mL) initially at 8.4 ?C is mixed with 30.5 mL of water (density = 1.0 g/mL) initially at 23.8 ?C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?
If 55.0 mL of ethanol (density = 0.789 g/mL ) initially at 6.0 ∘ C is...
If 55.0 mL of ethanol (density = 0.789 g/mL ) initially at 6.0 ∘ C is mixed with 55.0 mL of water (density = 1.0 g/mL ) initially at 28.6 ∘ C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? ( C EtOH =2.42J/(g⋅ ∘ C). ) Express the temperature in degrees Celsius to three significant figures.
If 45.0 mL of ethanol (density=0.789 g/mL) initially at 9.0 C is mixed with 45.0 mL...
If 45.0 mL of ethanol (density=0.789 g/mL) initially at 9.0 C is mixed with 45.0 mL of water (density=1.0 g/mL) initially at 28.6 C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture? I tried many times in trying to get the answer, but I keep getting it wrong. I appreciate who answers this writes it step by step. Thank you.
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml....
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml. of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL. and the density of water is 1.00 g/ml. The specific heat of ethanol is 2.46 Jig:"C and the specific heat of water is 4.184 J/g:°C. Ti = 30.7 "C Incorrect
A solution is made by mixing 223.0 mL of ethanol initially at15.3 ∘C with 223.0 mL...
A solution is made by mixing 223.0 mL of ethanol initially at15.3 ∘C with 223.0 mL of water initially at 21.1 ∘C What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g⋅°C and the specific heat of water is 4.184 J/g⋅°C. Tf= ∘C
A solution is made by mixing 207.0 mL of ethanol initially at 14.7 ∘C with 207.0...
A solution is made by mixing 207.0 mL of ethanol initially at 14.7 ∘C with 207.0 mL of water initially at 23.9 ∘C . What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL . The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C
50.0 g of water at 22 °C is mixed with 125 g of water initially at...
50.0 g of water at 22 °C is mixed with 125 g of water initially at 36 °C. What is the final temperature of the water after mixing, assuming no heat is lost to the surroundings?
A solution is made by mixing 285.0 ml. of ethanol initially at 11.7°C with 285.0 ml. of water initially at 21.9 °C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL. and the density of water is 1.00 g/ml. The specific heat of ethanol is 2.46 Jig:"C and the specific heat of water is 4.184 J/g:°C. Ti = 30.7 "C Incorrect
Most questions answered within 3 hours.
-
A new machine costs $150,000, lasts 10 years, has an annual
O&M cost of $50,000, and...
asked 11 seconds from now -
A newspaper in a large Midwestern city reported that the
National Association of Realtors said that...
asked 1 minute ago -
1. Develop a use case diagram for the bank case study described
in Chapter 1. 2....
asked 11 minutes ago -
The phylum Protista has often been referred to as a junk drawer
of classification. Explain what...
asked 17 minutes ago -
The average amount of money spent for lunch per person in the
college cafeteria is $7.09...
asked 19 minutes ago -
You follow the lab procedure and at the end of Part 4C, you used
an average...
asked 38 minutes ago -
Write 250-450 words, about the following: • Analyze how a
servant leader in your organization or...
asked 42 minutes ago -
3. American and Japanese workers can each produce 4 cars a
year. An American worker can...
asked 45 minutes ago -
On October 1, 20X1, a company purchased a piece of land by
agreeing to pay the...
asked 57 minutes ago -
Jamie is doing a survey at her school about whether the students
feel the cafeteria food...
asked 1 hour ago -
What are the roles of 3' and 5' untranslated regions in
mRNAs?
asked 1 hour ago -
A domestic television receives antenna delivers a sky noise
power of -105 dBm to a matched...
asked 1 hour ago