Question

5. C(s) + O2 (g) CO2 (g) + Heat

This reaction can be classified as​

Answer 1

Answer:

bro I don't know sorry

Explanation:

Please mark me brainest .... ❤️❤️

Answer 2

An exothermic reaction occurs when the temperature of a system increases due to the evolution of heat. This heat is released into the surroundings, resulting in an overall negative quantity for the heat of reaction ( qrxn<0 ). An endothermic reaction occurs when the temperature of an isolated system decreases while the surroundings of a non-isolated system gains heat. Endothermic reactions result in an overall positive heat of reaction ( qrxn>0 ).

Exothermic and endothermic reactions cause energy level differences and therefore differences in enthalpy ( ΔH ), the sum of all potential and kinetic energies. ΔH is determined by the system, not the surrounding environment in a reaction. A system that releases heat to the surroundings, an exothermic reaction, has a negative ΔH by convention, because the enthalpy of the products is lower than the enthalpy of the reactants of the system.

C(s)+O2(g)⟶CO2(g)(ΔH = –393.5 kJ)

H2(g)+12O2(g)⟶H2O(l)(ΔH = –285.8 kJ)

The enthalpies of these reactions are less than zero, and are therefore exothermic reactions. A system of reactants that absorbs heat from the surroundings in an endothermic reaction has a positive ΔH , because the enthalpy of the products is higher than the enthalpy of the reactants of the system.

N2(g)+O2(g)⟶2NO(g)(ΔH = +180.5 kJ > 0)

C(s)+2S(s)⟶CS2(l)(ΔH = +92.0 kJ > 0)

Because the enthalpies of these reactions are greater than zero, they are endothermic reactions.