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ExtremeBDS [4]
2 years ago
10

If 4.00 moles of gasoline are burned according to the chemical

Chemistry
1 answer:
omeli [17]2 years ago
8 0

Answer: The volume of oxygen at STP is needed for complete given combustion is 1121.28 L.

Explanation:

The given reaction equation is as follows.

2C_{2}H_{18}(l) + 25O_{2}(g) \rightarrow 16CO_{2}(g) + 18H_{2}O(g)

This shows that 2 moles of gasoline requires 25 moles of O_{2}. Hence, moles of oxygen required to react with 4 moles of gasoline are calculated as follows.

\frac{25 mol O_{2}}{2 mol C_{8}H_{18}} \times 4 mol C_{8}H_{18}\\= 50 mol O_{2}

At STP, the pressure is 1 atm and temperature is 273.15 K. Therefore, using ideal gas equation the volume of oxygen is calculated.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

PV = nRT\\1 atm \times V = 50 mol \times 0.0821 L atm/mol K \times 273.15 K\\V = 1121.28 L

Thus, we can conclude that volume of oxygen at STP is needed for complete given combustion is 1121.28 L.

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Answer:

44.7 kWh

Explanation:

Let's consider the reduction of Al₂O₃ to Al in the Bayer process.

6 e⁻ + 3 H₂O + Al₂O₃ → 2 Al + 6 OH⁻

We can establish the following relations:

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When the applied electromotive force is 5.00 V, the energy required to produce 3.00 kg (3.00 × 10³ g) of aluminum is:

3.00 \times 10^{3} gAl.\frac{1molAl}{26.98gAl} .\frac{6mole^{-}}{2molAl}.\frac{96468c}{1mole^{-}}.\frac{5.00J}{c}.\frac{1kWh}{3.6 \times 10^{6}J} =44.7kWh

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The answer has to be 62.2

Explanation:

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