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The formation of carbon dioxide (CO2) from its elements can be represented by the reaction:
[ C(s) + O_2(g) \rightarrow CO_2(g) ]
This reaction is exothermic, meaning it releases energy. The enthalpy change (ΔH) for this reaction is -393.5 kJ/mol, indicating that when one mole of CO2 is formed from carbon and oxygen, 393.5 kJ of energy is released into the surroundings. This release of energy is often measured using calorimetry in a controlled environment.
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What of the following reactions shows that the formation of SO2 releases 296.8 kJmol?
The reaction that indicates the formation of SO2 releases 296.8 kJ/mol is typically represented as: [ S(s) + O_2(g) \rightarrow SO_2(g) , \Delta H = -296.8 , \text{kJ/mol} ] This notation shows that when one mole of sulfur reacts with one mole of oxygen to form sulfur dioxide, it releases 296.8 kJ of energy, indicating an exothermic reaction.
What of the following reactions shows that the formation of CO2 releases 393.5 kJmol?
The reaction that shows the formation of CO2 releasing 393.5 kJ/mol is typically represented as the combustion of carbon or hydrocarbons. For example, the reaction for the combustion of carbon can be written as: [ C(s) + O_2(g) \rightarrow CO_2(g) ] This reaction indicates that the formation of one mole of carbon dioxide from solid carbon and oxygen gas releases 393.5 kJ of energy, demonstrating an exothermic process.
What is the reactions shows that the formation of CO2 releases 393.5 kJmol?
The reaction that shows the formation of carbon dioxide (CO2) releasing 393.5 kJ/mol is the combustion of carbon in oxygen, represented by the balanced equation: C(s) + O2(g) → CO2(g). This exothermic reaction indicates that when one mole of carbon reacts with oxygen to form carbon dioxide, it releases 393.5 kJ of energy. This energy release is a key factor in various applications, including combustion engines and the generation of heat in industrial processes.
What reaction shows that the enthalpy of formation of H2S is Hf -20.6 kjmol?
The enthalpy of formation of H₂S (hydrogen sulfide) being -20.6 kJ/mol indicates that the formation of H₂S from its elements releases energy. This reaction can be represented as: [ \text{H}_2(g) + \text{S}(s) \rightarrow \text{H}_2\text{S}(g) ] The negative sign of the enthalpy change signifies that the process is exothermic, meaning that energy is released when hydrogen gas and solid sulfur combine to form hydrogen sulfide.
What reaction shows that the formation of SO2 releases 296.8 kJmol?
The reaction that shows the formation of sulfur dioxide (SO₂) and the associated energy release is represented by the equation: [ S(s) + O_2(g) \rightarrow SO_2(g) \quad \Delta H = -296.8 , \text{kJ/mol} ] This indicates that when one mole of sulfur reacts with one mole of oxygen to form sulfur dioxide, 296.8 kJ of energy is released, signifying an exothermic reaction. The negative sign of the enthalpy change (ΔH) indicates that energy is released into the surroundings during this process.
Which of the following reactions shows h formation of CO2 releases 393.5 kjmol?
C(s)+O2(g) yields CO2(g)+393.5kJ
What of the following reactions shows that the formation of SO2 releases 296.8 kJmol?
The reaction that indicates the formation of SO2 releases 296.8 kJ/mol is typically represented as: [ S(s) + O_2(g) \rightarrow SO_2(g) , \Delta H = -296.8 , \text{kJ/mol} ] This notation shows that when one mole of sulfur reacts with one mole of oxygen to form sulfur dioxide, it releases 296.8 kJ of energy, indicating an exothermic reaction.
What of the following reactions shows that the formation of CO2 releases 393.5 kJmol?
The reaction that shows the formation of CO2 releasing 393.5 kJ/mol is typically represented as the combustion of carbon or hydrocarbons. For example, the reaction for the combustion of carbon can be written as: [ C(s) + O_2(g) \rightarrow CO_2(g) ] This reaction indicates that the formation of one mole of carbon dioxide from solid carbon and oxygen gas releases 393.5 kJ of energy, demonstrating an exothermic process.
What is the reactions shows that the formation of CO2 releases 393.5 kJmol?
The reaction that shows the formation of carbon dioxide (CO2) releasing 393.5 kJ/mol is the combustion of carbon in oxygen, represented by the balanced equation: C(s) + O2(g) → CO2(g). This exothermic reaction indicates that when one mole of carbon reacts with oxygen to form carbon dioxide, it releases 393.5 kJ of energy. This energy release is a key factor in various applications, including combustion engines and the generation of heat in industrial processes.
Which of the following reactions shows that the formation of SO2 releases 296.8 kJ mol?
S(s) + O2(g) SO2(g) + 296.8 kJ
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 reaction shows that the formation of SO2 releases 296.8 kJmol?
The reaction that shows the formation of sulfur dioxide (SO₂) and the associated energy release is represented by the equation: [ S(s) + O_2(g) \rightarrow SO_2(g) \quad \Delta H = -296.8 , \text{kJ/mol} ] This indicates that when one mole of sulfur reacts with one mole of oxygen to form sulfur dioxide, 296.8 kJ of energy is released, signifying an exothermic reaction. The negative sign of the enthalpy change (ΔH) indicates that energy is released into the surroundings during this process.
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.
What shows that the formation of CO 2 releases 393.5 kJ mol?
C(s) + O2(g) + CO2(g) + 393.5 kJ
Which of the following reactions shows that the formation of NO2 requires 33.1 kJ mol?
1/2 N2(g) + O2(g) + 33.1 kJ NO2(g)
What is an example that shows that the combustion of methane produces 802 kJmol of energy?
The enthalpy of combustion is determined by calorimetry.
What reaction shows that the enthalpy of formation of CS2 is Hf 89.4 kJmol?
The enthalpy of formation of carbon disulfide (CS2) can be indicated by the reaction: C(s) + 2 S(s) → CS2(l). This reaction represents the formation of one mole of CS2 from its elements in their standard states. The enthalpy change associated with this reaction is +89.4 kJ/mol, meaning that 89.4 kJ of energy is absorbed when one mole of CS2 is formed from solid carbon and solid sulfur.
