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Stella [2.4K]
3 years ago
5

If the specific heat of iron is 0.449 J/g·K, what is the enthalpy change of this process for 100 g of Fe (s)? Is the process end

othermic or exothermic? Explain.
Chemistry
1 answer:
katrin2010 [14]3 years ago
8 0

Full Question:

Although it is not really a chemical reaction, one could consider a cooling process to be analogous to the enthalpy change that occurs in a reaction. Consider the transformation

Fe (s, T = 300 K) → Fe (s, T = 250 K)

If the specific heat of iron is 0.449 J/g·K, what is the enthalpy change of this process for 100 g of Fe (s)? Is the process endothermic or exothermic? Explain.

Answer:

ΔH = - 2245J

Explanation:

Specific heat capacity, Cp = 0.449 J/g·K

ΔH=MCpΔT

ΔT = 250K - 300K = - 50K

ΔH = 100 * 0.449 * (-50)

ΔH = - 2245J

The iron will lose (give off) heat energy to cool down. Hence, it is an exothermic process. The negative sign of the enthalpy confirms this.

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Answer : The number of moles of solute Ca(OH)_2 is, 0.0788 moles.

Explanation : Given,

Molarity = 0.225 M

Volume of solution = 0.350 L

Formula used:

\text{Molarity}=\frac{\text{Moles of }Ca(OH)_2}{\text{Volume of solution (in L)}}

Now put all the given values in this formula, we get:

0.225M=\frac{\text{Moles of }Ca(OH)_2}{0.350L}

\text{Moles of }Ca(OH)_2=0.0788mol

Therefore, the number of moles of solute Ca(OH)_2 is, 0.0788 moles.

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Answer:

True

Explanation:

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Answer:

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