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What energy profile best shows that the formation of NO2 requires 33.1 kJmol?
Wiki User
∙ 6y ago
Verified answer
Brainly says it’s energy profile B for APEX please correct if i’m wrong.
Bella Fuentes
Julio Portillo
A reaction energy profile with a reactant energy level higher than the product energy level by 33.1 kJ/mol at the transition state represents the formation of NO2. The reactants start at a higher energy level, transition to a higher energy state at the activation energy point, then decrease in energy to form the product.
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.
An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
The significant jump in ionization energy from the first to the second indicates the removal of an electron from a filled energy level. This suggests the atom is in the second group of the periodic table, since elements in this group have a filled outer s sublevel before starting to fill the p sublevel in the subsequent period.
Which of the following reactions shows h formation of CO2 releases 393.5 kjmol?
C(s)+O2(g) yields CO2(g)+393.5kJ
What is an example that shows that the combustion of methane produces 802 kJmol of energy?
When one mole of methane ($CH_4$) combusts, it releases 802 kJ of energy. The balanced chemical equation for this reaction is: $CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) + 802 kJ$.
Which energy profile best shows that the Hf of H2S is -20.6 kJmol?
Energy profile A
An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
The significant jump in ionization energy from the first to the second indicates the removal of an electron from a filled energy level. This suggests the atom is in the second group of the periodic table, since elements in this group have a filled outer s sublevel before starting to fill the p sublevel in the subsequent period.
The ionization energy for sodium is 496 kJmol The electron affinity for chlorine is -349 kJmol what is the enthalpy?
The enthalpy change for forming sodium chloride from its elements can be calculated using the equation: Enthalpy change = Ionization energy of sodium + Electron affinity of chlorine. Plugging in the values, we get: 496 kJ/mol + (-349 kJ/mol) = 147 kJ/mol. Therefore, the enthalpy change for forming sodium chloride is 147 kJ/mol.
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 is an example that shows that the combustion of methane produces 802 kJmol of energy?
When one mole of methane ($CH_4$) combusts, it releases 802 kJ of energy. The balanced chemical equation for this reaction is: $CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) + 802 kJ$.
Which of the following reactions shows h formation of CO2 releases 393.5 kjmol?
C(s)+O2(g) yields CO2(g)+393.5kJ
What is the standard enthalpy of hydrogenation of 1-butene?
The standard enthalpy of hydrogenation of 1-butene is -30.1 kJ/mol. This value represents the amount of heat released when one mole of 1-butene is completely hydrogenated to form butane.
The minimum energy required to break the oxygen oxygen bond is 495 kJmol The wavelength of sunlight that can cause this bond breakage is 241nm How do you obtain this wavelength?
To find the wavelength, first convert the energy required to break the bond from kJ/mol to J/molecule. Then use this energy value to calculate the frequency of the light required using the formula E=hf, where E is the energy, h is Planck's constant, and f is the frequency. Finally, use the relationship between frequency and wavelength (c = λf) to find the wavelength, where c is the speed of light.
How many kJ of energy are required to melt 30.7 g of ice The heat of fusion of water is 6.02 kJmol. The temperature remains constant at 0 and degC. kJ?
10,267 kJ are needed
What is the standard enthalpy of formation of hydrogen bromide?
[from wikipedia] The standard enthalpy of formation"standard heat of formation" of a compound is the change of enthalpy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 degrees Celsius). Its symbol is ΔHfO.
What can be said about a reaction with H 620 kJmol and S -0.46 kJ(molK)?
it can never be spontanious
At which temperature would a reaction with H -92 kJmol S -0.199 kJ(molK) be spontaneous?
The condition for a reaction to be spontaneous is ΔG < 0, where ΔG = ΔH - TΔS. At the temperature where ΔG becomes negative, the reaction will be spontaneous. You can calculate this temperature using the given values of ΔH and ΔS.
