LU how do you solve the x M due Dec 2 x C Calculate The Heat In K x G Calculate
ID: 1064044 • Letter: L
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LU how do you solve the x M due Dec 2 x C Calculate The Heat In K x G Calculate the heat (in k x C ezto mheducation.com 0.31 points Enter your answer in the provided box. The fuel value of hamburger is approximately 3.3 kcal/g. If a man eats 0.45 pounds of hamburger for lunch and none of the energy is stored in his body, estimate the amount of water that would have to be lost in perspiration to keep his body temperature constant. The heat of vaporization of water may be taken as 2.41 kJ/g. (l lb 453.6 g) 1.1 References eBook & Resources WWTB Question Difficulty: Medlum Windows 8 Report problem Hint a 4x 3 2016-12-0 903Explanation / Answer
6. Energy gained from consuming the hamburger = (0.45 lbs)*(453.6 g/1 lb)*(3.3 kcal/g)*(4.184 kJ/1 kcal) = 2818.32566 kJ (I have kept a few guard digits extra and employed the relation 1 kcal = 4.184 kJ).
The heat of vaporization of water = 2.41 kJ/g.
Let x g of water be lost. Therefore,
(x g).(2.41 kJ/g) = 2818.32566 kJ
===> x = 2818.32566 kJ/(2.41 kJ) = 1169.4297 1169.43
The mass of water lost as perspiration = 1169.43 g = 1.169 kg (ans).
9. The question seems to have missing information. What is the heat of combustion per mole of ethane?
10. Let H be the amount of heat given. We know that
H = (mass of copper)*(specific heat of copper)*(change in temperature) = (592 g)*(0.377 J/g.C)*(49.8 – 22.3)C = 6137.56 J 6.14*103 J = 6.14 kJ (ans).
13. The given equation is
2 NO (g) + O2 (g) ------> 2 NO2 (g); H = -114.6 kJ/mol
The heat of reaction is given as -114.6 kJ for production of 1 mole of NO2.
We have 1.68*104 g NO2. The molar mass of NO2 = 46 g/mol.
Therefore, moles of NO2 produced = (1.68*104 g)*(1 mol/46 g) = 365.2174 mol.
The amount of heat involved = (-114.6 kJ/mol)*(365.2174 mol) = -41853.914 kJ = -4.18*104 kJ (ans).
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