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[" 31.The value of "/E" for combustion o...

[" 31.The value of "/_E" for combustion of "16g" of "],[CH_(4)" is - "885389" ] at "298K" .The "Delta H],[" combustion for "CH_(4)" in "Jmol^(-1)" at this "],[" temperature will be "],[" (Given that,"R=8.314JK^(-1)mol^(-1)" ) "],[[" a) "-55337," b) "-880430],[" c) "-885389," d) "-890348]]

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The value of DeltaE for combustion of 16 g of CH_4 is -885389 at 298 K. The DeltaH combustion for CH_4 in Jmol^(-1) at this temperature will be : (Given that, R = 8.314 JK^(-1) mol^(-1) )

The value of DeltaE for combustion of 16 g of CH_4 is -885389 at 298 K. The DeltaH combustion for CH_4 in Jmol^(-1) at this temperature will be : (Given that, R = 8.314 JK^(-1) mol^(-1) )

The equilibrium constant for a reaction is 10 what will be the value of Delta G^@ ? [R= 8.314 JK^(-1)mol^(-1) ,T=300K]

The heat of combustion of C_10H_8(s) at constant volume is -5133kJ mol_-1 at 298K. Calculate the value of enthalpy change. (R=8.314 JK_-1 mol_-1)

The heat of combustion of CH_(4) is -400 KJ mol^(-1) . Calculate the heat released when 40g of H_(2)O is formed upon combustion :-

The heat of combustion of CH_(4) is -400 KJ mol^(-1) . Calculate the heat released when 40g of H_(2)O is formed upon combustion :-

Heat of combustion of CH_4 (g) at constant volume and at 298 K has been found to be - 885 kJ mol^(-1) , calculate the enthalpy of its combustion under constant pressure condition ( R = 8.31 J K^(-1) mol^(-1) ).

The equilibrium constant for a reaction is 10. What will be the value of Delta G^(@) ? R = 8.314 jK^(-1) mol^(-1), T = 300K .