For an endothermic reaction, ΔH represents the enthalpy of the reaction in kJ mol-1. The minimum amount of activation energy will be

Question

For an endothermic reaction, ΔH represents the enthalpy of the reaction in kJ mol-1. The minimum amount of activation energy will be (A) less than zero (B) equal to Δ H (C) less than Δ H (D) more than Δ H.

Tardigrade Admin · Accepted Answer

For a reaction, E a pr =Δ H+E a BR . For endothermic reaction, Δ H= positive; thus E a FR >Δ H For exothermic reaction, Δ H= negative, thus nothing can be said.

Q. For an endothermic reaction, $Δ$ H represents the enthalpy of the reaction in $k J m o l^{- 1}$ . The minimum amount of activation energy will be

less than zero

equal to $Δ H$

less than $Δ H$

more than $Δ H .$

For a reaction, $E_{a_{p r}} = Δ H + E_{a_{BR}}$ . For endothermic reaction, $Δ H =$ positive; thus $E_{a_{FR}} > Δ H$
For exothermic reaction, $Δ H =$ negative, thus nothing can be said.

Q. For an endothermic reaction, ΔH represents the enthalpy of the reaction in kJmol−1. The minimum amount of activation energy will be

less than zero

equal to ΔH

less than ΔH

more than ΔH.

For a reaction, Eapr​​=ΔH+EaBR​​. For endothermic reaction, ΔH= positive; thus EaFR​​>ΔH For exothermic reaction, ΔH= negative, thus nothing can be said.

Q. For an endothermic reaction, $Δ$ H represents the enthalpy of the reaction in $k J m o l^{- 1}$ . The minimum amount of activation energy will be

equal to $Δ H$

less than $Δ H$

more than $Δ H .$

For a reaction, $E_{a_{p r}} = Δ H + E_{a_{BR}}$ . For endothermic reaction, $Δ H =$ positive; thus $E_{a_{FR}} > Δ H$
For exothermic reaction, $Δ H =$ negative, thus nothing can be said.