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For the equations C("diamond") +2H(2)(...

For the equations
`C("diamond") +2H_(2)(g) rarr CH_(4)(g) DeltaH_(1)`
`C(g)+4H(g) rarr CH_(4)(g) DeltaH_(2)` Predict whther

A

`DeltaH_(1) = DeltaH_(2)`

B

`DeltaH_(1) gt DeltaH_(2)`

C

`DeltaH_(1) lt DeltaH_(2)`

D

`DeltaH_(1) = DeltaH_(2) + Delta_(vap)H(C )+ Delta_(diss)H(H_(2))`

Text Solution

AI Generated Solution

To solve the problem, we need to analyze the two given reactions and their enthalpy changes, ΔH₁ and ΔH₂. ### Step-by-Step Solution: 1. **Identify the Reactions**: - The first reaction is: \[ C(\text{diamond}) + 2H_2(g) \rightarrow CH_4(g) \quad \Delta H_1 ...
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Consider the reactions : C_((s))+2H_(2(g)) rarr CH_(4(g)), DeltaH=-X kcal C_((g))+4H_((g)) rarr CH_(4(g)),DeltaH-X_(1)kcal CH_(4(g))rarr CH_(3(g))+H_((g)), DeltaH=+Ykcal The average bond energy of C-H bond is :

With the help of thermochemical equations given below, determine Delta_(r )H^(Θ) at 298 K for the following reaction: C("graphite")+2H_(2)(g) rarr CH_(4)(g),Delta_(r )H^(Θ) = ? C("graphite")+O_(2)(g) rarr CH_(2)(g), Delta_(r )H^(Θ) = -393.5 kJ mol^(-1) ...(1) H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l) , Delta_(r )H^(Θ) = -285.8 kJ mol^(-1) ...(2) CO_2(2)(g)+2H_(2)O(l) rarr CH_(4)(g)+2O_(2)(g) , Delta_(r )H^(Θ) = +890.3 kJ mol^(-1) ...(3)

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Calculate in kJ for the following reaction : C(g) + O_(2)(g) rarr CO_(2)(g) Given that, H_(2)O(g) + C(g) + H_(2)(g) , Delta H = +131 kJ CO(g) + 1/2 O_(2)(g) rarr CO_(2)(g), " " Delta H = -242 kJ H_(2)(g) + 1/2 O_(2)(g) rarr H_(2)O(g), " "DeltaH = -242 kJ

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Determine the heat of transformaiton of C_(("dimamond"))rarrC_(("graphite")) form the following data: i. C_(("diamond"))+O_(2)(g) rarr CO_(2)(g), DeltaH^(Theta) =- 94.5 kcal ii. C_(("graphite")) +O_(2)(g) rarr CO_(2)(g),DeltaH^(Theta) =- 94.0 kcal

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CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Exercises (Single Correct)
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