Home
Class 11
CHEMISTRY
CH4(g) + 2O2(g) to CO2(g) + 2H2O(g), Del...

`CH_4(g) + 2O_2(g) to CO_2(g) + 2H_2O(g), Delta H = -809 kJ`
The calorific value of 1 kg of `CH_4(g)` is ………… kJ/kg.

Text Solution

AI Generated Solution

To find the calorific value of 1 kg of methane (CH₄), we will follow these steps: ### Step 1: Understand the reaction and the given data We have the combustion reaction of methane: \[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g) \] The enthalpy change (ΔH) for this reaction is given as -809 kJ. This means that when 1 mole of methane combusts, it releases 809 kJ of energy. ### Step 2: Calculate the molar mass of methane ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    ICSE|Exercise VERY SHORT ANSWER TYPE QUESTIONS |56 Videos

  • CHEMICAL THERMODYNAMICS

    ICSE|Exercise SHORT ANSWER TYPE QUESTIONS|63 Videos

  • CHEMICAL THERMODYNAMICS

    ICSE|Exercise REVIEW EXERCISES |84 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    ICSE|Exercise NCERT TEXT-BOOK EXERCISES ( WITH HINTS AND SOLUTIONS)|47 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

    ICSE|Exercise NCERT TEXT-BOOK. EXERCISE (With Hints and Solutions)|63 Videos

Similar Questions

Explore conceptually related problems

CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l), DeltaH =- 890 kJ what is the calorific or fuel value of 1kg of CH_(4) ?

Given C_((s)) + O_(2(g)) rarr CO_(2(g)), Delta H = -395 kJ , S_((g)) + O_(2(g)) rarr SO_(2(g)) , Delta H = -295 kJ , CS_(2(l)) + 3O_(2(g)) rarr CO_(2(g)) + 2SO_(2(g)) , Delta H = -1110 kJ The heat of formation of CS_(2(l)) is

Calculate the standard enthalpy change for the reaction CH_4 (g) + 2O_2(g) to CO_2(g) + 2H_2O(l) , given that the standard heatds of formation of CH_4(g, CO_2(g) and H_2O (l) are -74.91 mol^(-1), -394.12 kJ mol^(-1) and -286.31 kJ mol^(-1) respectivley.

Calculate the heat of formation of methanol (CH_3OH) from thhe following data: CH_3OH(l) + 3/2O_2(g) to CO_2(g) + 2H_2O (l),Delta =-726 kJ C(s) + O_2(g) to CO_2(g) , DeltaH = -394 kJ H_2(g) + 1/2 O_2(g) to H_2O(l) , Delta H = -286 kJ

C(s)+(1)/(2)O_(2)(g)to CO(g), Delta H =- 42 kJ/mole CO(g)+(1)/(2)O_(2)(g)to CO_(2)(g) , Delta H =-24 kJ/mole The heat of formation of CO_(2) is

The heat evolved in the combustion of methane is given by the following equation : CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(l) , Delta H = -890.3 kJ How many grams of methane would be required to produce 445.15 kJ of heat of combustion ?

H_2(g) + 1/2 O_2(g) to H_2O (l), DeltaH = - 286 kJ 2H_2(g) + O_2(g) to 2H_2O (l), DeltaH = …kJ

Compounds with carbon-carbon double bond, such as ethylene, C_(2)H_(4) , add hydrogen in a reaction called hydrogenation. C_(2)H_(4)(g)+H_(2)(g) rarr C_(2)H_(6)(g) Calculate enthalpy change for the reaction, using the following combustion data C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(g) , Delta_("comb")H^(Θ) = -1401 kJ mol^(-1) C_(2)H_(6)(g) + 7//2O_(2)(g)rarr 2CO_(2) (g) + 3H_(2)O(l) , Delta_("comb")H^(Θ) = -1550kJ H_(2)(g) + 1//2O_(2)(g) rarr H_(2)O(l) , Delta_("comb")H^(Θ) = -286.0 kJ mol^(-1)

For the reaction: 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(g), DeltaH =- 571 kJ bond enegry of (H-H) = 435 kJ and of (O=O) = 498 kJ . Then, calculate the average bond enegry of (O-H) bond using the above data.

From the following reaction, (1/2) N_2O (g) + (3/4) O_2(g) rarr NO_2(g) , delta H = -x , C_2H_2 (g) + (5/2) O_2(g) rarr 2CO(g) + 3H_2O(l) , delta H = -y , 2C_3H_8 (g) + 10 O_2(g) rarr 6CO_2(g) + 8H_2O(l) , delta H = -z , which of the following options contain all values of enthalpy of combustion (delta H°_c) for the given reaction