Total heat exchange = Qiron + Qwater = 0 Qiron = (462 J/K) + (T -...
Total heat exchange = Qiron + Qwater = 0
Qiron = (462 J/K) + (T - 352*C) and Qwater = (167.6 J/K) + (T - 20*C)
[(462 J/K) + (T - 352*C)] + [(167.6 J/K) + (T - 20*C)] =0
629.6 J/K + (T - 263.621) = 0
At the end they combine the two specific heats. I see that they simply added the 462 and 167.6 to get the 629.6, but I don't understand is how they got [T - 263.621] from [T - 352*C] + [T - 20*C]
Homework Answers
Add Answer to:
Total heat exchange = Qiron + Qwater = 0
Qiron = (462 J/K) + (T -...
Please show all work Compute the total quantity of heat (both in Kcal and J) required...
Please show all work
Compute the total quantity of heat (both in Kcal and J) required to raise the temperature of 1.00 kg of ice at -10.0 degrees C to 1.00 kg of steam at 110.0 degrees C. Assume no loss of mass or heat in this process. Note that this will requires several computations that must be completely added up, and you must include all phase changes and use the correct specific heats.
Gold (Au, M = 197 .0 g mol-1) melts at 1338 K with a heat of...
Gold (Au, M = 197 .0 g mol-1) melts at 1338 K with a heat of fusion of 12. 7 kJ mol-1, and boils at 3080 K with a heat of vaporization of 310 kJ mol-1. The specific heats (in units J g-1 K-1) are: Au(s) - 0.131, Au(l) - 0.149, Au(g) - 0.0632. Calculate the heat needed to convert 2.15 g of solid gold at 1000 K to liquid at 1500 K. . 286 J B. 12.8 kJ C....
Help!!! Part A If a total of 5.55 x 10% J of heat is added to...
Help!!!
Part A If a total of 5.55 x 10% J of heat is added to a mass of 555 g of water which was originally at a temperature of 555°C (and noting that the specific heat of water is 4186 J/kg-K and that the latent heat of vaporization of water is 2.26 x 106 J/kg), then what is the mass of the water that remains (ie. the mass of the water that was not vaporized)? O 335 g 258...
Path: P Words:0 QUESTION 27 A 42.9 g sample of Fe (specific heat 0.449 J/gºC) at...
Path: P Words:0 QUESTION 27 A 42.9 g sample of Fe (specific heat 0.449 J/gºC) at an initial temperature of 125.0°C is added to 185.0 g sample of water. The final temperature reached for both is 42.1°C. Assuming no heat is lost to the surroundings and given that the specific heat of water is 4.18J/g°C, what is the initial temperature of the water, in °C? Simply type the number, not the unit. QUESTION 28
Learning Goal: To understand specific heat and heat of transformation and how they are related to...
Learning Goal: To understand specific heat and heat of transformation and how they are related to temperature versus time graphs Energy can be added to a system either by doing work w an it or by adding heat tot Energy transfer by work equires a force to act through some distance Energy ansfer in the form of heat occurs between objects that are different temperatures with onergy spontaneously aveling from the higher temperature object to the lower mperature one. When...
2. A 0.825-kg block of iron, with an average specific heat of 5.60 x102 J/kg K,...
2. A 0.825-kg block of iron, with an average specific heat of 5.60 x102 J/kg K, is initially at a temperature of 352°C. It is placed in a calorimeter that has 40.0 g of water at 20.0°C. What is the final thermal equilibrium temperature? If your answer if 100.0°C, calculate the amount of water that remains in liquid form. Treat the mass and heat capacity of the calorimeter as neglible.
Consider a 2 m long metal rod. The temperature u(z,t) at a point along the rod at any time t is found by solving the heat equation k where k is the material property. The left end of the rod ( 0) is...
Consider a 2 m long metal rod. The temperature u(z,t) at a point along the rod at any time t is found by solving the heat equation k where k is the material property. The left end of the rod ( 0) is maintained at 20°C and the right end is suddenly dipped into snow (0°C). The initial temperature distribution in the rod is given by u(x,0)- (i) Use the substitution u(z,t) ta,t)+20-10z to reduce the above problem to a...
A certain substance has a specific heat 1 J/(mole.K) and has melting point of 360 K....
A certain substance has a specific heat 1 J/(mole.K) and has melting point of 360 K. If one mole of substance is at 359 degrees how much energy must be added to melt it. a. Exactly 1 J b. Lesss than 1 Joule c. Greater than 1 joule d. Less than 0 J
Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of...
Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of ice melts at 0 °C and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) Marked out of 1.00 Answer: P Flag question Calculate the change in entropy (in J/K) when 98.2 g of water is heated from 28.7 °C to 76.7 °C at 1 atm. (The specific heat is 4.184 J/(g-K).) Question 18 Not yet answered Marked out of 1.00 Notice...
The elementary, reversible gas phase reaction A B is to be carried out in a CSTR with heat exchange. Pure A is fed to t...
The elementary, reversible gas phase reaction A B is to be carried out in a CSTR with heat exchange. Pure A is fed to the reactor. The heat exchange coil in the reactor is maintained at 400K. The rate coefficient is known at 400K, but heat of reaction is unknown. Data: k1(400K) = 0.001 s.! V-1000L To=350K R-831 J/mol K h 5 mol's UA 1000 J/K Kea (450K-1 A) Calculate the conversion (X) if the steady state CSTR is operated...
Please show all work
Compute the total quantity of heat (both in Kcal and J) required to raise the temperature of 1.00 kg of ice at -10.0 degrees C to 1.00 kg of steam at 110.0 degrees C. Assume no loss of mass or heat in this process. Note that this will requires several computations that must be completely added up, and you must include all phase changes and use the correct specific heats.
Help!!!
Part A If a total of 5.55 x 10% J of heat is added to a mass of 555 g of water which was originally at a temperature of 555°C (and noting that the specific heat of water is 4186 J/kg-K and that the latent heat of vaporization of water is 2.26 x 106 J/kg), then what is the mass of the water that remains (ie. the mass of the water that was not vaporized)? O 335 g 258...
Path: P Words:0 QUESTION 27 A 42.9 g sample of Fe (specific heat 0.449 J/gºC) at an initial temperature of 125.0°C is added to 185.0 g sample of water. The final temperature reached for both is 42.1°C. Assuming no heat is lost to the surroundings and given that the specific heat of water is 4.18J/g°C, what is the initial temperature of the water, in °C? Simply type the number, not the unit. QUESTION 28
Learning Goal: To understand specific heat and heat of transformation and how they are related to temperature versus time graphs Energy can be added to a system either by doing work w an it or by adding heat tot Energy transfer by work equires a force to act through some distance Energy ansfer in the form of heat occurs between objects that are different temperatures with onergy spontaneously aveling from the higher temperature object to the lower mperature one. When...
2. A 0.825-kg block of iron, with an average specific heat of 5.60 x102 J/kg K, is initially at a temperature of 352°C. It is placed in a calorimeter that has 40.0 g of water at 20.0°C. What is the final thermal equilibrium temperature? If your answer if 100.0°C, calculate the amount of water that remains in liquid form. Treat the mass and heat capacity of the calorimeter as neglible.
Consider a 2 m long metal rod. The temperature u(z,t) at a point along the rod at any time t is found by solving the heat equation k where k is the material property. The left end of the rod ( 0) is maintained at 20°C and the right end is suddenly dipped into snow (0°C). The initial temperature distribution in the rod is given by u(x,0)- (i) Use the substitution u(z,t) ta,t)+20-10z to reduce the above problem to a...
Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of ice melts at 0 °C and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) Marked out of 1.00 Answer: P Flag question Calculate the change in entropy (in J/K) when 98.2 g of water is heated from 28.7 °C to 76.7 °C at 1 atm. (The specific heat is 4.184 J/(g-K).) Question 18 Not yet answered Marked out of 1.00 Notice...
The elementary, reversible gas phase reaction A B is to be carried out in a CSTR with heat exchange. Pure A is fed to the reactor. The heat exchange coil in the reactor is maintained at 400K. The rate coefficient is known at 400K, but heat of reaction is unknown. Data: k1(400K) = 0.001 s.! V-1000L To=350K R-831 J/mol K h 5 mol's UA 1000 J/K Kea (450K-1 A) Calculate the conversion (X) if the steady state CSTR is operated...
Most questions answered within 3 hours.
-
A 79-Ω loudspeaker, a 8.0-Ω loudspeaker, and a 3.7-Ω loudspeaker
are connected in parallel across the...
asked 25 minutes ago -
If X has a normal distribution with mean µ =
12 and variance σ2 = 9,...
asked 33 minutes ago -
An example of an operational taxonomic unit
(OTU) is
a. Multiple sequence alignment.
b. Protein sequence....
asked 35 minutes ago -
Electrons flow through a 2.7-mm-diameter aluminum wire at
2.5×10−4 m/s .
How many electrons move through...
asked 35 minutes ago -
For a recent year, McDonald’s (MCD)
company-owned restaurants had the following sales and expenses (in
millions):...
asked 34 minutes ago -
In a sample of 15 men, the mean height was 171 cm. In a sample
of...
asked 35 minutes ago -
In this exercise, we will be refactoring a working program. Code
refactoring is a process to...
asked 2 hours ago -
3
researchers at Cambrige looked at 5,000 firms in Englans and found
that, in terms of...
asked 1 hour ago -
why it is important and how it integrates within ERP? And what
the core challenges of...
asked 3 hours ago -
A strawberry farmer determines that the average weight of
individual strawberries produced by plants in his...
asked 4 hours ago -
Chargaff's results yielded a molar ratio of 0.400 for A to G in
avian tubercle bacillus...
asked 6 hours ago -
Which of the following binds ATP/ADP?
a. microfilaments
b. microtubules
c. intermediate filaments
d. microfilaments and...
asked 6 hours ago