Calculate - Ho for the reaction between ethene and water to form ethyl alcohol from the following data -c Ho C2H5 OHl - - 1368 kJ -c Ho C2 H4g - - 1410 kJDoes the calculated - Ho represent the enthalpy of formation of liquid ethanol-

The reaction between ethene and water to form ethyl alcohol #160; is given below. CH_2=CH_2(g) +H_2O (l) → C_2H_5OH (l) The above equation can be obtained ...

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Standard XII

Chemistry

Heat of Reaction

Calculate Δ...

Question

Calculate $Δ H^{o}$ for the reaction between ethene and water to form ethyl alcohol from the following data
$Δ_{c} H^{o} C_{2} H_{5} O H_{(l)} = - 1368 k J$
$Δ_{c} H^{o} C_{2} H_{4 (g)} = - 1410 k J$
Does the calculated $Δ H^{o}$ represent the enthalpy of formation of liquid ethanol?

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Solution

The reaction between ethene and water to form ethyl alcohol is given below.
$C H_{2} = C H_{2} (g) + H_{2} O (l) \to C_{2} H_{5} O H (l)$
The above equation can be obtained from the following two equations.
$C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l) Δ_{c} H^{o} C_{2} H_{5} O H_{(l)} = - 1368 k J$ ......(1)
$C H_{2} = C H_{2} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l) Δ_{c} H^{o} C_{2} H_{4 (g)} = - 1410 k J$ ......(2)
(2) -(1) gives
$C H_{2} = C H_{2} (g) + H_{2} O (l) \to C_{2} H_{5} O H (l) Δ_{c} H^{o} C_{2} H_{4 (g)} = - 1410 k J - (- 1368 k J) = - 42 k J$
$\to Δ H^{o} = - 1368 k J$
The calculated $Δ H^{o}$ does not represent the enthalpy of formation of liquid ethanol.
The enthalpy of formation of liquid ethanol will involve a equation showing formation of liquid ethanol from elements in standard state. The equation formation of liquid ethanol is given below.
$2 C (g r a p h i t e) + 3 H_{2} (g) + \frac{1}{2} O_{2} (g) \to C_{2} H_{5} O H (l)$

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Similar questions

Q. Calculate

Δ H^{0}

for the reaction between ethene and water to form ethyl alcohol from the following data:

Δ_{c} H^{0} C_{2} H_{5} O H (l) = - 1368 k J

Δ_{c} H^{0} C_{2} H_{4} = - 1410 k J

Does the calculated

Δ H^{0}

represent the enthalpy of formation of liquid ethanol?

Q. Calculate

Δ H^{o}

of the reaction

2 N a B r + C l_{2} = 2 N a C l + {B r}_{2}

, if there is known the

Δ H^{o}

of substances formation:

Δ H^{o} (N a B r) = - 361 K J / m o l

Δ H^{o} (N a C l) = - 411 K J / m o l

Q. Calculate the enthalpy of formation of

Δ H_{f}

for

C_{2} H_{5} O H

from tabulated data and its heat of combustion as represented by the following equations:

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (g); Δ H^{o} = - 241.8 k J {m o l}^{- 1} . . . (i)

C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 393.5 k J {m o l}^{- 1} . . . (i i)

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 3 H_{2} O (g) + 2 C O_{2} (g); Δ H^{o} = - 1234.7 k J . . . (i i i)

Q. For which one of the following equations is

Δ H^{o}

(reaction) equal to

Δ H^{o}

(formation) for the product?

Q. The enthalpy changes for the following processes are listed below:

{C l}_{2} (g) ⟶ 2 C l (g); Δ H^{o} = 242.3 k J {m o l}^{- 1}

I_{2} (g) ⟶ 2 I (g); Δ H^{o} = 151.0 k J {m o l}^{- 1}

{I C l} (g) ⟶ I (g) + C l (g); Δ H^{o} = 211.3 k J {m o l}^{- 1}

I_{2} (s) ⟶ I_{2} (g); Δ H^{o} = 62.76 k J {m o l}^{- 1}

Given that the standard states for iodine and chlorine are

I_{2} (s)

and

{C l}_{2} (g)

, the standard enthalpy of formation for

I C l (g)

is:

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Calculate ΔHo for the reaction between ethene and water to form ethyl alcohol from the following dataΔcHoC2H5OH(l)=−1368kJΔcHoC2H4(g)=−1410kJDoes the calculated ΔHo represent the enthalpy of formation of liquid ethanol?

Calculate $Δ H^{o}$ for the reaction between ethene and water to form ethyl alcohol from the following data
$Δ_{c} H^{o} C_{2} H_{5} O H_{(l)} = - 1368 k J$
$Δ_{c} H^{o} C_{2} H_{4 (g)} = - 1410 k J$
Does the calculated $Δ H^{o}$ represent the enthalpy of formation of liquid ethanol?