0
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 else can I help you with?
Which f 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 the combustion of carbon, represented as: [ C(s) + O_2(g) \rightarrow CO_2(g) ] In this exothermic reaction, when one mole of carbon reacts with oxygen to form carbon dioxide, it releases 393.5 kJ of energy, indicating that the formation of CO2 is energetically favorable.
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 reaction shows that the formation of NO2 requires 33.1 kJmol?
The reaction that shows the formation of nitrogen dioxide (NO2) requiring 33.1 kJ/mol is typically represented as: [ N_2(g) + 2O_2(g) \rightarrow 2NO_2(g) ] In this reaction, the enthalpy change (ΔH) of +33.1 kJ/mol indicates that energy is absorbed during the formation of NO2 from nitrogen and oxygen gases. This positive value signifies that the reaction is endothermic, requiring external energy input to proceed.
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 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 h formation of CO2 releases 393.5 kjmol?
C(s)+O2(g) yields CO2(g)+393.5kJ
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)
Which f 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 the combustion of carbon, represented as: [ C(s) + O_2(g) \rightarrow CO_2(g) ] In this exothermic reaction, when one mole of carbon reacts with oxygen to form carbon dioxide, it releases 393.5 kJ of energy, indicating that the formation of CO2 is energetically favorable.
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 reaction shows that the formation of NO2 requires 33.1 kJmol?
The reaction that shows the formation of nitrogen dioxide (NO2) requiring 33.1 kJ/mol is typically represented as: [ N_2(g) + 2O_2(g) \rightarrow 2NO_2(g) ] In this reaction, the enthalpy change (ΔH) of +33.1 kJ/mol indicates that energy is absorbed during the formation of NO2 from nitrogen and oxygen gases. This positive value signifies that the reaction is endothermic, requiring external energy input to proceed.
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 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 reactions shows that the formation of CO2 releases 393.5 kJmol?
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.
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 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 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.
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
