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3 years ago

Please help fast, I will give brainliest.

Chemistry

1 answer:

frez [133]3 years ago

7 0

Answer:

The reaction is favorable at all temperatures

Explanation:

Since G = H - TS, -H and +S would result in G = -H -TS, which will always be negative.

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For a particular isomer of C8H18, the combustion reaction produces 5113.3 kJ of heat per mole of C8H18(g) consumed, under standa

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Answer: The standard enthalpy of formation of this isomer of $C_8H_{18}(g)$ is -210.9 kJ

Explanation:

The given balanced chemical reaction is,

$C_8H_{18}(g)+\frac{25}{2}O_2(g)\rightarrow 8CO_2(g)+9H_2O(g)$

First we have to calculate the enthalpy of formation of $C_8H_{18}$ .

$\Delta H^o=H_f_{product}-H_f_{reactant}$

$\Delta H^o=[n_{CO_2}\times \Delta H_f^0_{(CO_2)}+n_{H_2O}\times \Delta H_f^0_{(H_2O)}]-[n_{O_2}\times \Delta H_f^0_{(O_2)+n_{C_8H_{18}}\times \Delta H_f^0_{(C_8H_{18})}]$

where,

We are given:

$\Delta H^o_f_{(CO_2(g))}=-393.5kJ/mol\\\Delta H^o_f_{(H_2O(g))}=-241.8kJ/mol\\\Delta H^o_f_{(O_2(g)))}=0kJ/mol$

Putting values in above equation, we get:

$-511.3kJ/mol=[(8\times -393.5)+(9\times -241.8)]-[(\frac{25}{2}\times 0)+(1\times \Delta H_f^0_{(C_8H_{18})}$

$\Delta H_f^0_{(C_8H_{18})}=-210.9kJ$

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4 years ago

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When a base is dissolved in water, what is released? A. H+ B. OH− C. CO2

Svet_ta [14]

Answer:Your answer is B

Hope this helps have a great day<3

Explanation:

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3 years ago

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