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Alexxx [7]
3 years ago
6

A molten sample of 1.00kg of iron with a specific heat of 0.385J/g.K at 1000.K is immersed in a sample of water. If the water ab

sorbs 270 kJ of heat what is the final temperature of the iron?
Chemistry
1 answer:
Schach [20]3 years ago
6 0

Answer:

Final T = 298.7K

Explanation:

In this problem, the heat given for the iron is equal to the heat that water absorbs. Using the equation:

Q = C*m*ΔT

<em>Where Q is heat given = 270000J</em>

<em>C is specific heat of substance = 0.385J/gK</em>

<em>m is mass of iron = 1000g</em>

<em>ΔT is change in temperature = Initial temperature - Final temperature.</em>

<em />

270000J = 0.385J/gK*1000g*(1000K-Final temperature)

701.3J/K = 1000K - Final T

<h3>Final T = 298.7K</h3>
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mol\text{ }Ca(NO_3)_2=2.40\text{ }mol\text{ }Li_3PO_4*\frac{3\text{ }mol\text{ }Ca(NO_3)_2}{2\text{ }mol\text{ }Li_3PO_4}=3.60\text{ }mol\text{ }Ca(NO_3)_2

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