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jolli1 [7]
3 years ago
6

Consider the reaction C2H4(g) + H2O(g) --> CH3CH2OH(g)

Chemistry
1 answer:
arsen [322]3 years ago
6 0

Answer:

K = 361.369

Explanation:

C2H4(g) + H2O(g) → CH3CH2OH(g)

∴ ΔG°f(298.15K) CH3CH2OH(g) = - 174.8 KJ/mol

∴ ΔG°f(298.15) C2H4(g) =  68.4 KJ/mol

∴ ΔG°f(298.15) H2O(g) = - 228.6 KJ/mol

⇒ ΔG°f(298.15) = - 174.8 - ( - 228.6 + 68.4 ) = - 14.6 KJ/mol

  • K = e∧(-ΔG°f / RT)

∴ R = 8.314 E-3 KJ/mol.K

∴ T = 298.15 K

⇒ K = e∧(-(-14.6)/((8.314 E-3)(298.15)))

⇒ K = e∧(5.889)

⇒ K = 361.369

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A gas at constant temperature has a pressure of 404.6 kPa with a volume of 12 ml. If the volume changes to 43ml, what is the new
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Answer:

The answer is

<h2>112.912 kPa</h2>

Explanation:

The new pressure can be found by using the formula for Boyle's law which is

P_1V_1 = P_2V_2

Since we are finding the new pressure

P_2 =  \frac{P_1V_1}{V_2}  \\

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From the question we have

P_2 =  \frac{404600 \times 12}{43}  =  \frac{4855200}{43}  \\  = 112911.6279... \\  = 112912

We have the final answer as

<h3>112.912 kPa</h3>

Hope this helps you

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3 years ago
Acetylene gas (ethyne; HC = CH) burns in an oxyacetylene torch to produce carbon dioxide and water vapor. The heat of reaction f
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The mass of CO2 produced by 26g of acetylene is 88g.

Given ,

In an oxyacetylene torch, acetylene gas (ethyne; HCCH) burns to produce carbon dioxide and water vapour.

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Heat of reaction for acetylene combustion = 1259kj/mol

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On combustion, 1 mole of acetylene yields 2 moles of CO2.

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As a result, the mass of carbon dioxide produced by 26g of acetylene is 88g.

Learn more about acetylene here :

brainly.com/question/15346128

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