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Which energy profile best shows that the Hf of H2S is -20.6 kJmol?
Energy profile A
Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJmol?
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.
What energy profile best shows that the formation of NO2 requires 33.1 kJmol?
Brainly says it’s energy profile B for APEX please correct if i’m wrong.
What is the relationship between Gibbs free energy and enthalpy in a chemical reaction?
In a chemical reaction, the relationship between Gibbs free energy and enthalpy is described by the equation G H - TS, where G is the change in Gibbs free energy, H is the change in enthalpy, T is the temperature in Kelvin, and S is the change in entropy. This equation shows that the Gibbs free energy change is influenced by both the enthalpy change and the entropy change in a reaction.
Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJ mol?
H2(g) + S(s) H2S + 20.6 kJ
which energy profile best shows that the enthalpy of formation of CS2 is 89.4 kJ/mol?
graph D
Which energy profile best shows that the Hf of H2S is -20.6 kJmol?
Energy profile A
Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJmol?
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.
What energy profile best shows that the formation of NO2 requires 33.1 kJmol?
Brainly says it’s energy profile B for APEX please correct if i’m wrong.
What reaction shows that the enthalpy of formation of C2H4 is Hf 52.5 kjmol?
The enthalpy of formation (ΔHf) of C2H4 can be determined through the reaction of its constituent elements in their standard states: 2 C(s) + 2 H2(g) → C2H4(g). The enthalpy change for this reaction is measured to be +52.5 kJ/mol, indicating that forming ethylene (C2H4) from graphite (C) and hydrogen gas (H2) requires this amount of energy. This value represents the standard enthalpy of formation for C2H4, defined as the heat absorbed when one mole of a compound is formed from its elements at standard conditions.
What Reactions shows that the formation of NO2 requires 33.1 kJmol?
The formation of nitrogen dioxide (NO2) from its elemental constituents can be represented by the reaction: N2(g) + 2 O2(g) → 2 NO2(g). The enthalpy change for this reaction indicates that 33.1 kJ/mol of energy is required to form NO2. This value reflects the energy needed to break the bonds in the reactants and form the bonds in the product. Thus, the positive enthalpy change signifies that the reaction is endothermic, necessitating an input of energy for the formation of NO2.
which reaction shows that the enthalpy of formation of C2H4 is Hf = 52.5 kJ/mol?
2C(s) + 2H2(g) + 52.5 kJ -> C2H4
What is the relationship between Gibbs free energy and enthalpy in a chemical reaction?
In a chemical reaction, the relationship between Gibbs free energy and enthalpy is described by the equation G H - TS, where G is the change in Gibbs free energy, H is the change in enthalpy, T is the temperature in Kelvin, and S is the change in entropy. This equation shows that the Gibbs free energy change is influenced by both the enthalpy change and the entropy change in a reaction.
Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJ mol?
H2(g) + S(s) H2S + 20.6 kJ
Which reaction shows that the enthalpy of formation of C2H4 is Hf 52.5 kJ mol?
2C(s) + 2H2(g) + 52.5 kJ -> C2H4
Which reaction shows that the enthalpy of formation of CS2 is H89.4 kj mol?
C(s) + 2S(s) + 89.4kJ --} CS2(l)
Which reaction shows that the enthalpy of formation of cs2 is hf 89.4 kJ mol?
C(s) + 2S(s) + 89.4 kJ --> CS2(l)
