The heat of combustion of methane at 298 K is expressed by: CH4(g)+2O2(g)→ CO2(g)+2H2O(l) Δ H=890.2 textkJ text. The magnitude of AE of the reaction at this temperature is:

Question

The heat of combustion of methane at 298 K is expressed by: CH4(g)+2O2(g)→ CO2(g)+2H2O(l) Δ H=890.2 textkJ text. The magnitude of AE of the reaction at this temperature is: (A) infinity (B) less than Δ H  (C) equal to Δ H  (D) greater than Δ H

Tardigrade Admin · Accepted Answer

CH4(g)+2O2(g) xrightarrow CO2(g)+2H2O(l)-890.2 kJ Δ H=Δ E+Δ nRT Δ n= moles of gaseous products - moles of gaseous reactants =1-3=-2 So, for the above reaction Δ Epsilon value is greater than Δ H.

Q. The heat of combustion of methane at 298 K is expressed by: $C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l)$ $Δ H = 890.2 kJ .$ The magnitude of AE of the reaction at this temperature is:

infinity

less than $Δ H$

equal to $Δ H$

greater than $Δ H$

$C H_{4} (g) + 2 O_{2} (g)$ $C O_{2} (g) + 2 H_{2} O (l) - 890.2 k J$ $Δ H = Δ E + Δ n RT$ $Δ n =$ moles of gaseous products - moles of gaseous reactants $= 1 - 3 = - 2$ So, for the above reaction $Δ E$ value is greater than $Δ H .$

Q. The heat of combustion of methane at 298 K is expressed by: CH4​(g)+2O2​(g)→CO2​(g)+2H2​O(l) ΔH=890.2kJ. The magnitude of AE of the reaction at this temperature is:

infinity

less than ΔH

equal to ΔH

greater than ΔH

CH4​(g)+2O2​(g)​ CO2​(g)+2H2​O(l)−890.2kJ ΔH=ΔE+ΔnRT Δn= moles of gaseous products - moles of gaseous reactants =1−3=−2 So, for the above reaction ΔE value is greater than ΔH.

Q. The heat of combustion of methane at 298 K is expressed by: $C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l)$ $Δ H = 890.2 kJ .$ The magnitude of AE of the reaction at this temperature is:

less than $Δ H$

equal to $Δ H$

greater than $Δ H$

$C H_{4} (g) + 2 O_{2} (g)$ $C O_{2} (g) + 2 H_{2} O (l) - 890.2 k J$ $Δ H = Δ E + Δ n RT$ $Δ n =$ moles of gaseous products - moles of gaseous reactants $= 1 - 3 = - 2$ So, for the above reaction $Δ E$ value is greater than $Δ H .$