For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in th
ermodynamic values for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 180.5kJ/mol
ΔS∘rxn 24.80J/(mol⋅K)
a. Calculate the temperature in kelvins above which this reaction is spontaneous
b. The thermodynamic values from part A will be useful as you work through part B:
ΔH∘rxn 180.5kJ/mol
ΔS∘rxn 24.80J/(mol⋅K)
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C :
The reaction in which C3H6Br2 (1,2-Dibromopropane) is created is:
C3H6 + Br2 → C3H6Br2
We can see that the only difference between the product (C3H6Br2) and the known reactant (C3H6) of the reaction is two bromine atoms (Br2). Br2 is diatomic bromine - a molecule we get after combining two bromine atoms. This compound is a red-brown liquid at room temperature, which means that that is the liquid described in your question.
During cellular respiration<span>, glucose is broken down in the presence of oxygen to produce carbon dioxide and water,energy is </span><span>released.</span>