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Elena-2011 [213]
2 years ago
14

Study the reactions.

Chemistry
1 answer:
yulyashka [42]2 years ago
3 0

Answer:

\displaystyle \Delta H = -2426\text{ kJ}

Explanation:

To find the enthalpy change of the target reaction, we can use Hess's Law.

Reversing the third reaction yields:

\displaystyle \text{C$_3$H$_8$(g)} \longrightarrow 3\text{C(s)} + 4\text{H$_2$(g)}\;\;\;\;\;\Delta H = -106\text{ kJ}

Multiplying the first reaction by three yields:

\displaystyle 3\text{C(s)} + 3\text{O$_2$(g)} \longrightarrow 3\text{CO$_2$}(g)}\;\;\;\;\; \Delta H = -1.18\times 10^3\text{ kJ}

Multiplying the second reaction by four yields:

\displaystyle 4\text{H$_2$(g)} + 2\text{O$_2$(g)} \longrightarrow 4\text{H$_2$O($\ell$)} \;\;\;\;\;  \Delta H = -1.14\times 10^3 \text{ kJ}

Adding all equations yield:

\displaystyle \text{C$_3$H$_8$(g)} + 5\text{O$_2$(g)} \longrightarrow 3\text{CO$_2$(g)} + 4\text{H$_2$O($\ell$)} \;\;\;\;\; \Delta H = -2426\text{ kJ}

Hence, the enthalpy change of the target reaction is -2426 kJ.

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Answer:

Mass of original sample = 100 g

Explanation:

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k=\frac{\ln2}{30.17}\ year^{-1}

The rate constant, k = 0.02297 year⁻¹

Time = 90.6 years

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

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12.5\ g=[A_0]e^{-0.02297\times 90.6}

[A_0]=\frac{12.5}{e^{-0.02297\times 90.6}}\ g=100\ g

<u>Mass of original sample = 100 g</u>

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