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xz_007 [3.2K]
2 years ago
6

6. Think of some other chemical reactions. List them and the type of reaction: exothermic or endothermic. Example: Burning coal

- exothermic​
Chemistry
1 answer:
Oksanka [162]2 years ago
7 0

Remember: energy is conserved in a chemical reaction (visualize the reaction and question whether heat lies on reactant side (left) or product side (right))

-exothermic- heat is released (heat is on the product side)

>forming an ionic lattice (SALT)- mixture of Na and Cl results in a more stable ionic lattice, causing this reaction to be exothermic

>burning wood

-endothermic- heat is absorbed (heat is on the reactant side)

> cooking an egg

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How much heat energy, in kilojoules, is required to convert 72.0 gg of ice at −−18.0 ∘C∘C to water at 25.0 ∘C∘C ? Express your a
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Answer: The enthalpy change is 34.3 kJ

Explanation:

The conversions involved in this process are :

(1):H_2O(s)(-18^0C)\rightarrow H_2O(s)(0^0C)\\\\(2):H_2O(s)(0^0C)\rightarrow H_2O(l)(0^0C)\\\\(3):H_2O(l)(0^0C)\rightarrow H_2O(l)(25^0C)

Now we have to calculate the enthalpy change.

\Delta H=[m\times c_{s}\times (T_{final}-T_{initial})]+n\times \Delta H_{fusion}+[m\times c_{l}\times (T_{final}-T_{initial})]

where,

\Delta H = enthalpy change = ?

m = mass of water = 72.0  g

c_{s} = specific heat of ice = 2.09J/g^0C

c_{l} = specific heat of liquid water = 4.184J/g^0C

n = number of moles of water = \frac{\text{Mass of water}}{\text{Molar mass of water}}=\frac{72.0g}{18g/mole}=4.00moles

\Delta H_{fusion} = enthalpy change for fusion = 6010 J/mole

Now put all the given values in the above expression, we get

\Delta H=[72.0g\times 2.09J/g^0C\times (0-(-18)^0C]+4.00mole\times 6010J/mole+[72.0g\times 4.184J/g^)C\times (25-0)^0C]\Delta H=34279.8J=34.3kJ        (1 KJ = 1000 J)

Therefore, the enthalpy change is 34.3 kJ

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3 years ago
What evidence from the experiment shows that conduction occurred? In your answer, be sure to include the materials involved in t
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Answer:

uhh

Explanation:

Have no clue but I hope u get the question answered

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2. Calculate the mass of 5.35 mole of H2O2.
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Answer:

5.35m H2O2 x 34.02g/1m H2O2 = 182g H2O2

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