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xxTIMURxx [149]
3 years ago
13

It has been suggested that hydrogen gas obtained by the decomposition of water might be a substitute for natural gas (principall

y methane). To compare the energies of combustion of these fuels, the following experiment was carried out using a bomb calorimeter with a heat capacity of 11.3 kJ/oC. When a 1.50 g sample of methane gas was burned with excess oxygen in the calorimeter, the temperature increased by 7.3oC. When a 1.15 g sample of hydrogen gas was burned with excess oxygen, the temperature increase was 14.3oC. Compare the energies of combustion (per gram) for hydrogen and methane.
Chemistry
1 answer:
Aleks [24]3 years ago
3 0

Answer:

Hydrogen: -141 kJ/g

Methane: -55kJ/g

The energy released per gram of hydrogen in its combustion is higher than the energy released per gram of methane in its combustion.

Explanation:

According to the law of conservation of the energy, the sum of the heat released by the combustion and the heat absorbed by the bomb calorimeter is zero.

Qc + Qb = 0

Qc = -Qb  [1]

We can calculate the heat absorbed by the bomb calorimeter using the following expression.

Q = C . ΔT

where,

C is the heat capacity

ΔT is the change in the temperature

<h3>Hydrogen</h3>

Qc = -Qb = -C . ΔT = -(11.3 kJ/°C) . (14.3°C) = -162 kJ

The heat released per gram of hydrogen is:

\frac{-162kJ}{1.15g} =-141 kJ/g

<h3>Methane</h3>

Qc = -Qb = -C . ΔT = -(11.3 kJ/°C) . (7.3°C) = -82 kJ

The heat released per gram of methane is:

\frac{-82kJ}{1.50g} =-55kJ/g

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A reaction was performed in which 4.0 g of cyclohexanol was reacted with an acid catalyst to obtain 2.8 g of cyclohexene. calcul
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Answer:

              %age Yield  =  85.36 %

Solution:

The Balance Chemical Reaction is as follow,

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According to Equation ,

              100 g (1 mole) C₆H₁₂O produces  =  82 g (1 moles) of C₆H₁₀

So,

                       4.0 g of C₆H₁₂O will produce  =  X g of C₆H₁₀

Solving for X,

                      X =  (4.0 g × 82 g) ÷ 100 g

                      X  =  3.28 g of C₆H₁₀   (Theoretical Yield)

As we know,

                     %age Yield  =  (Actual Yield ÷ Theoretical Yield) × 100

                     %age Yield  =  (2.8 g ÷ 3.28 g) × 100

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2 years ago
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stellarik [79]

Answer:

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3.Using the mole ratio, calculate the moles of substance yielded by the reaction.

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2 years ago
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Answer:

0.156mol

Explanation:

Number of moles of a substance can be calculated from its mass by dividing its mass by molar mass i.e.

Number of moles (n) = mass/molar mass

Molar mass of PbCl4 is as follows, where Pb = 207.2g/mol, Cl = 35.5g/lol

PbCl4 = 207.2 + 35.5(4)

= 207.2 + 142

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Using: mole = mass/molar mass

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