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Butoxors [25]
3 years ago
6

If the total amount of energy required to change a substance to a different phase and temperature is positive, then does that me

an that the
phase change has moved in the direction of solid gas or gas - solid and has the temperature increased or decreased?
A. solid-gas temperature increase
B. solid-gas temperature decrease
C. gas sold temperature increase
D. gas - solid temperature decrease
Chemistry
1 answer:
diamong [38]3 years ago
8 0
It would be A. Solid-gas temperature increases ( think of a block of ice, you have to increase temperature to make it melt, then the water would evaporate into a gas)
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Most minerals are _______ at room temperature.<br><br> solid<br> gas<br> liquid
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Answer:

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Explanation:

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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)]

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\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
List the four groups attached to the central carbon of an amino acid.
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A study of the decomposition reaction 3RS2  3R + 6S yields the following initial rate dat
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Missing question: What is the rate constant for the reaction?
<span>[RS2](mol L-1) Rate (mol/(L·s))
0.150                0.0394
0.250                0.109
0.350                0.214
0.500                0.438</span>
Chemical reaction: 3RS₂ → 3R + 6S.
Compare second and fourth experiment, when concentration is doubled, rate of concentration is increaced by four. So rate is:
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k = 0,438 ÷ (0,500)².
k = 1,75 L/mol·s.
3 0
3 years ago
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