Home
Class 12
CHEMISTRY
A natural gas may be assumed to be a mix...

A natural gas may be assumed to be a mixture of `CH_(4)` and `C_(2)H_(6)` only. On complete combination of 10 L of the gas at STP, the heat evolved was 474.6 kJ. Assuming `DeltaH_(c)(CH_(4)(g)) = -894` kJ/mol and `DeltaH_(c)(C_(2)H_(6)(g)) = -1560 kJ//mol`. Calculate the % of volume of each gas in the mixture.

Text Solution

Verified by Experts

`K_(s) to K(g), DeltaH_(5) = 89.8 kJ mol^(-1)`
We have to find `DeltaH` of the following equation.
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL ENERGETICS

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SECTION (I) JEE MAINS : SINGLE CORRECT OPTION)|92 Videos

  • CHEMICAL ENERGETICS

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SECTION (II) JEE ADVANCED WITH SINGLE CORRECT CHOICE)|84 Videos

  • CARBOXYLIC ACIDS AND ITS DERIVATIVES

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTIONS|1 Videos

  • CHEMICAL EQUILIBRIUM

    FIITJEE|Exercise MATCHING TYPE QUESTIONS|3 Videos

Similar Questions

Explore conceptually related problems

A natural gas may be assumed to be a mixture fo methane and ethane only. On complete combustion of 10L of gas at STP the heat evolved was 474.6 kJ . Assuming Delta_(comb) H^(Theta) CH_(4)(g) =- 894 kJ mol^(-1) and composition of the mixture by volume.

The standard enthalpy of formation of ammonia gas is Given: N_(2)H_(4) (g) + H_(2) (g) rarr 2NH_(3) (g), Delta H_(r)^(@) = - 40 kJ//mol DeltaH_(f)^(@) [N_(2)H_(4) (g)] = - 120 kJ//mol

Calculate the enthalpy of formation of ethane from the follwong enthalpy of combustion data: C(s) : - 393.5 kJ, H_(2)(g) : - 285.8 kJ and C_(2)H_(6)(g) : - -1560.0 kJ

Bond dissociation energy of CH_(4) si 360 kJ/mol and C_(2)H_(6) has 620 kJ mol. Then bond dissociation energy of C-C bond is :-

The heats of combustion of C_(2)H_(4(g)), C_(2)H_(6(g)) and H_(2(g)) are -1405,-1558.3 and -285.6 kJ respectively. Calculate heat of hydrogenation of ethylene.