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suter [353]
3 years ago
7

42 At standard pressure, the total amount of heat required to completely vaporize a 100. gram sample of water at its boiling poi

nt is(1) 2.26 X 10 J (3) 2.26 X 103 J
(2) 2.26 X 102 J (4) 2.26 X 105 J
Chemistry
1 answer:
yan [13]3 years ago
4 0

Answer:

4 is the actual answer, the other answer can eat my ...

Explanation:

The answer is 100% legit answer choice 4 not 3!!!!!!

This is because the 2260 is 10^2 and then ^3 is increased when boiling a 100 gram

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The new boiling point is 101.02°C. Suppose that you add another 2.0 mol of sucrose to this solution. What do you predict the new
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2 years ago
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MAGNESIUM (Mg)<br> +FLUORINE (F) =
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3 years ago
The density of H2O2 is 1.407 g/mL, and the density of O2 is 1.428 g/L. How many liters of O2 can be made from 55 mL H2O2
balandron [24]

Explanation:

mass H2O2 = 55 mL(1.407 g/mL) = 80.85 g

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Now, you need the temperature.  If you are at STP (273 K, and 1.00 atm) then 1 mole of an ideal gas at STP has a volume of 22.4 L.  Without temperature you are not really able to continue.  I will assume you are at STP.

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8 0
2 years ago
How much heat (in kj) is required to warm 13.0 g of ice, initially at -12.0 ∘c, to steam at 113.0 ∘c? the heat capacity of ice i
olga nikolaevna [1]
The total amount of heat required is the sum of all the sensible heat and latent heats involved in bringing the ice to a desired temperature and state. The latent heat of fusion and vaporization of water 333.55 J/g and 2260 J/g, respectively. Solving for the total amount of heat,
                   total amount of heat = 13.0 g (2.09 J/gC)(12) + 13(333.55 J/g) + 13.0 g (4.18 J/gC)(100 - 0) + (13.0 g)(2260 J/g) + (13 g)(2.01 J/g)(113-100) 
                                        = 39815.88 J 
                                        = 39.82 kJ
5 0
3 years ago
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