Calculate Δ H rxn for the reaction: 5 C ( s ) + 6 H 2 ( g ) → C 5 H 12 ( l ) Use the following reactions and given ΔH’s: C 5 H 12 ( l ) + 8 O 2 ( g ) → 5 CO 2 ( g ) + 6 H 2 O ( g ) Δ H = − 3244.8 kJ C ( s ) + O 2 ( g ) → CO 2 ( g ) Δ H = − 393.5 kJ 2 H 2 ( g ) + O 2 ( g ) → 2 H 2 O ( g ) Δ H = − 483.5 kJ

The enthalpy of reaction is, -173.2 kJ

Explanation:

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The intermediate balanced chemical reaction will be,

(1)    

(2)    

(3)    

Reversing (1) , Multiply (2) by 5 , (3) by 3 and add

Therefore, the enthalpy of reaction is, -173.2 kJ

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation: