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Maurinko [17]
3 years ago
7

How many liters of fluorine gas, at standard temperature and pressure, will react with 23.5 grams of potassium metal? Show all o

f the work used to solve this problem.
2 K + F2 ---> 2 KF
Chemistry
1 answer:
Degger [83]3 years ago
8 0
1) Molar mass:

K = <span> 39.0983 g/mol
F</span>₂ = <span> 37.99 g/mol

moles ratio:

2 K + F</span>₂<span>   =   2 KF

2 x 39.0983 g K ----------------- 37.99 g F</span>₂
23.5 g K -------------------------- ( mass of F₂)
<span>
mass of F</span>₂ = 23.5 x 37.99 / 2 x 39.0983
<span>
mass of F</span>₂ = 892.765 / 78.1966
<span>
mass of F</span>₂ = 11.4169 g
<span>
Therefore:

</span>37.99 g F₂------------------ 22.4 L ( at STP)
11.4169 g F₂ --------------- ( volume F₂ )

Volume F₂ = 11.4169 x 22.4 / 37.99

Volume F₂ = 255.73856 / 37.99

Volume F₂ = 6.731 L
<span>


</span>
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\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f_{(product)}]-\sum [n\times \Delta H^o_f_{(reactant)}]

The equation for the enthalpy change of the above reaction is:

\Delta H^o_{rxn}=[(5\times \Delta H^o_f_{(B_2O_3(s))})+(9\times \Delta H^o_f_{(H_2O(l))})]-[(2\times \Delta H^o_f_{(B_5H_9(l))})+(12\times \Delta H^o_f_{(O_2(g))})]

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If 2 moles of B_5H_9 produces -9078.57 kJ of energy.

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If (2\times 63.12)g of B_5H_9 produces -9078.57 kJ of energy

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