Na reacts violently with H2O to produce NaOH and H2. The resulting solution has a higher T than it did before the Na was added. What are the expected changes?
deltaH ?
deltaS >0
deltaG <0
deltaP >0
I know the last three for a fact.
Is deltaG "<0" ?
If the reaction is exothermic what does that say about delta H?
Is the system more or less ordered?
For a reaction to be spontaneous, what must delta G be, + or -?
What is delta P? If that is pressure, why is delta P > 0?
To determine the expected changes for the given reaction, we need to analyze the information provided.
1. Is deltaG "<0"?
Yes, based on your statement, deltaG is expected to be less than zero (deltaG < 0). This indicates that the reaction is spontaneous under standard conditions.
2. If the reaction is exothermic, what does that say about delta H?
If the reaction is exothermic, it means that it releases heat into the surroundings. Therefore, delta H would be negative (deltaH < 0) since it represents the change in enthalpy.
3. Is the system more or less ordered?
The given information does not provide any details regarding the change in the system's order (deltaS). Hence, we cannot determine whether the system becomes more or less ordered based on the information provided.
4. For a reaction to be spontaneous, what must delta G be, + or -?
For a reaction to be spontaneous under standard conditions, delta G must be negative (deltaG < 0).
5. What is delta P? If that is pressure, why is delta P > 0?
Delta P represents the change in pressure during a chemical reaction. In this context, delta P > 0 suggests an increase in pressure. In the given reaction, which involves the reaction of sodium (Na) with water (H2O), the production of hydrogen gas (H2) leads to an increase in the number of gas molecules. As a result, the overall pressure is expected to increase, hence delta P > 0.