H2(g) + S(s) —> H2S + 20.6 kJ
The reaction that shows the enthalpy of formation of H2S as -20.6 kJ/mol is: 2H2(g) + S(s) → 2H2S(g) with ΔH = -20.6 kJ/mol. This means that forming 1 mole of H2S from its elements H2 and S releases 20.6 kJ of energy.
H2(g) + S(s) H2S + 20.6 kJ
2C(s) + 2H2(g) + 52.5 kJ -> C2H4
The reaction showing the enthalpy of formation of CS2 as -89.4 kJ/mol is: C(s) + 1.5S2(g) -> CS2(l) with ΔH = -89.4 kJ/mol
C(s)+O2(g) yields CO2(g)+393.5kJ
When one mole of methane ($CH_4$) combusts, it releases 802 kJ of energy. The balanced chemical equation for this reaction is: $CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) + 802 kJ$.
When one mole of methane ($CH_4$) combusts, it releases 802 kJ of energy. The balanced chemical equation for this reaction is: $CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) + 802 kJ$.
C(s) + 2S(s) + 89.4kJ --} CS2(l)
2C(s) + 2H2(g) + 52.5 kJ -> C2H4
H2(g) + S(s) H2S + 20.6 kJ
2C(s) + 2H2(g) + 52.5 kJ -> C2H4
The reaction showing the enthalpy of formation of CS2 as -89.4 kJ/mol is: C(s) + 1.5S2(g) -> CS2(l) with ΔH = -89.4 kJ/mol
C(s)+O2(g) yields CO2(g)+393.5kJ
graph D
Brainly says it’s energy profile B for APEX please correct if i’m wrong.
Molar enthalpy change, also known as molar enthalpy of reaction, is the amount of heat energy released or absorbed during a chemical reaction per mole of a substance. It is usually expressed in units of kJ/mol. The molar enthalpy change can be positive (endothermic) if heat is absorbed or negative (exothermic) if heat is released during the reaction.
Energy profile A
Formation of a precipitate; change in color; change in temperature; formation of a gas; emission of light.