3 years ago

feel free to answer any of these. i need the answer to the appropriate amount of significant figures on this pleasee

Chemistry

1 answer:

jekas [21]3 years ago

4 0

Answer:

6. (2.7* $10^{5}$ )

8. (1.0* $10^{4}$ )

Explanation:

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Answer:

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Which of the following elements is the most reactive?<br> A. Ba<br> B. Cs<br> C. Hf<br> D. Lu

hodyreva [135]

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Explanation:

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3 years ago

Which of the following is NOT a reason why chemical bonds are important? *

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3 years ago

Butane C4H10 (g),(Hf = –125.7), combusts in the presence of oxygen to form CO2 (g) (Delta.Hf = –393.5 kJ/mol), and H2O(g) (Delta

shusha [124]

Answer: The enthalpy of combustion, per mole, of butane is -2657.4 kJ

Explanation:

The balanced chemical reaction is,

$2C_4H_{10}(g)+13O_2(g)\rightarrow 8CO_2(g)+10H_2O(g)$

The expression for enthalpy change is,

$\Delta H=[n\times H_f_{products}]-[n\times H_f_{reactants}]$

Putting the values we get :

$\Delta H=[8\times H_f_{CO_2}+10\times H_f_{H_2O}]-[2\times H_f_{C_4H_{10}+13\times H_f_{O_2}}]$

$\Delta H=[(8\times -393.5)+(10\times -241.82)]-[(2\times -125.7)+(13\times 0)]$

$\Delta H=-5314.8kJ$

2 moles of butane releases heat = 5314.8 kJ

1 mole of butane release heat = $\frac{5314.8}{2}\times 1=2657.4kJ$

Thus enthalpy of combustion per mole of butane is -2657.4 kJ

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3 years ago