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dusya [7]
3 years ago
5

How much heat in kilojoules is required to heat 56 l of water from 89 ∘f to 212 ∘f?

Chemistry
1 answer:
scoundrel [369]3 years ago
3 0
You would need 67 if you add 56 and 89 = 145 and how i got 67. i went and subtract 212 and 145 = 67 and hope that answer you want if not well least i try
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Lets do process of elimination!

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B. Melting ice on a windshield - During the melting process, there is no chemical change, and therefore, no new substance is created.  

C. Burning gasoline - When gas burns it usually combines with oxygen to give carbon dioxide, water etc.  It is a chemical change.

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Determine the identity of a cube of metal that measures 1.2 cm on each side and has a mass of 15.4g.
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<span>Find the metal that has a density of approximately 8.9 g/cm³</span>
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Carbon, hydrogen and ethane each burn exothermically in an excess of air. AHⓇ =-393.7 kJ mol. C(s) + O2(g) → CO2(g) H2(g) + % O2
Salsk061 [2.6K]

<u>Answer:</u> The \Delta H^o_{rxn} for the reaction is 51.8 kJ.

<u>Explanation:</u>

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The chemical equation for the reaction of carbon and water follows:

2C(s)+2H_2(g)\rightarrow C_2H_4(g) \Delta H^o_{rxn}=?

The intermediate balanced chemical reaction are:

(1) C(s)+O_2(g)\rightarrow CO_2(g)    \Delta H_1=-393.7kJ    ( × 2)

(2) H_2+\frac{1}{2}O_2(g)\rightarrow H_2O(l)    \Delta H_2=-285.9kJ     ( × 2)

(3) 2C_2H_4(s)+2O_2(g)\rightarrow 2CO_2(g)+2H_2O(l)    \Delta H_3=-1411kJ

The expression for enthalpy of the reaction follows:

\Delta H^o_{rxn}=[2\times \Delta H_1]+[2\times \Delta H_2]+[1\times (-\Delta H_3)]

Putting values in above equation, we get:

\Delta H^o_{rxn}=[(2\times (-393.7))+(2\times (-285.9))+(1\times -(-1411))]=51.8kJ

Hence, the \Delta H^o_{rxn} for the reaction is 51.8 kJ.

6 0
3 years ago
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