Using the data below, calculate the enthalpy for the combustion of C to CO C(s) + O2(g)--> CO2 (g) ΔH1 = -393.5 kJ CO(g) + 1/
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Answer:
Explanation:
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In this case, since the given 5-M concentration of magnesium chloride is expressed as:
We can notice that one mole of salt contains two moles of chloride ions as the subscript of chlorine is two, in such a way, with the volume of solution we obtain the moles of chloride ions as shown below:
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Answer:
Usually give off heat energy
Explanation:
Exergonic reactions are the ones which are spontaneous. Spontaneous reactions are indicated by the negative change in the Gibbs free energy. In order to provide characteristics for an exergonic reaction, we need to define the Gibbs free energy in terms of the enthalpy change and the entropy change:
Here:
is the enthalpy change;
is the entropy change;
is the absolute temperature.
In order to achieve a negative value in the Gibbs free energy change, we should have:
This is true for all temperatures if:
The major term here is the change in enthalpy, notice that we wish the enthalpy change to be negative.
Negative enthalpy change corresponds to an exothermic reaction, the one which releases heat. This means exergonic reactions would usually give off heat.
Answer:
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