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Bond [772]
3 years ago
13

The decomposition of 57.0 g of Fe2O3 results in Consider the following reaction. 2Fe2O3 ---> 4Fe + 3O2 deltaH degree rxn = +

824.2 kJ decomposition of 57.0 g of Fe2O3 results in the release of 294 kJ of heat. A. the absorption of 23500 kJ of heat. B. the absorption of 147 kJ of heat. C. the absorption of 294 kJ of heat. D. the release of 23500 kJ of heat. E. the release of 147 kJ of heat.
Chemistry
1 answer:
lozanna [386]3 years ago
3 0

Answer:

The correct answer is option E.

Explanation:

2Fe_2O_3\rightarrow 4Fe + 3O_2 \Delta H^o_{rxn} = 824.2 kJ

Mass of ferric oxide decomposed = 57.0 g

Moles of ferric oxide decomposed = \frac{57.0 g}{160 g/mol}=0.35625 mol

According to reaction, 2 moles ferric oxide on combustion gives 824.2 kJ of heat.

Then heat given by on decomposition of 0.35625 mol of ferric oxide will be:

\frac{824.2 kJ}{2}\times 0.35625 =146.81 kJ\approx 147 kJ

So, on decomposition of 57.0 grams of ferric oxide 147 kilo Joules of heat was released.

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A horizontal cylinder equipped with a frictionless piston contains 785 cm3 of steam at 400 K and 125 kPa pressure. A total of 83
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Answer:

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Thus, n = PV/RT = (125000 × 0.000785)/(8.314 × 400) = 0.03 mol

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To calculate this, we use the constant pressure process;

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83.8 = 0.03 × [34980 + 35.5T_{1} - (34980 + 35.5T_{o})]

83.8 = (0.03 × 35.5) (T_{1} - 400K)

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T_{1} = 400 + 78.69

T_{1}  = 478.69 K

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To calculate this, we make use of the Charles' law(Temperature and pressure are directly proportional)

V_{1}/T_{1} = V_{o}/T_{o}

V_{1}  =  V_{o}T_{1}/T_{o}

V_{1}   = (785 × 478.69)/400

V_{1}   = 939.43 cm^{3}

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Mathematically, the work done by the system is calculated as follows;

w = P(V_{1}- V_{o}) = 125 KPa ( 939.43 - 785) = 19.30 J

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ΔU = q - w = 83.8 - 19.3 = 64.5J

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