DeltaG = DeltaH - TDeltaS
dG = -54.32 kJ/mol - (54'32+273)K(-354.2J/molK)
NB Thevtemperature is quoted in Kelvin(K) and the Entropy must be converted to kJ by dividing by '1000'/
Hence
dG = - 54.32kJ/mol - (327.32K)(-0.3542 kJ/molK)
NB The 'K' cancels out. Then maker the multiplication
dG = -54/32 kJ/mol - - 115.94 kJ/mol Note the double minus; it becomes plus(+).
Hence
dG = -54.32kj/mol + 115.94 kJ/mol
dG = (+)61.61 kJ/mol
Since dG is positive, the reaction is NOT thermodynamically feasible.
The answer depends on what two (or more) things the ratio is meant to compare. The kinetic energy of several objects? The kinetic energy of an object compared to its total energy? The kinetic energy compared to its engine size?
Potential energy does not depend on an object's decimal compulsion composition.
Basal Metabolism (BMR)
Joule is a unit for measuring energy. Meter is a unit for measuring length or distance. There is no conversion. If you wanted to find the potential energy of an object, 2.04 meters off the ground, then you would need to know the mass of the object and the value of g (gravitational acceleration) at the point where you are, then you could calculate energy in Joules.
Look for the ct (current transformer). You will find a ratio rating (for example, 200:5.) This means divide 200 by 5. The result is 40. Any difference in reading from a certain time should be multiplied by 40 to get actual energy consumption. This is the basic information, but in practice it should be calibrated by a government-certified body (the department of energy, for example) to perfectly match the kwhr-meter revolution.
Exothermic, because the reaction enthalpy must be negative. With polymerization, the entropy decreases. The Gibbs energy has to be negative. Thus negative reaction enthalpy. Gibbs energy = reaction enthalpy - temperature*entropy
True, a large positive value of entropy tends to favor products of a chemical reaction. However, entropy can be offset by enthalpy; a large positive value of enthalpy tends to favor the reactants of a chemical reaction. The true measure to determine which side of a chemical reaction is favored is the change in Gibbs' free energy, which accounts for both entropy and enthalpy, as calculated by: Change in Gibbs = Change in Enthalpy - Temp in Kelvin * Change in Entropy A negative value of Gibbs free energy will always favour the products of a chemical reaction.
Temperature and energy are two of the variables included when graphing enthalpy and entropy. Enthalpy is made up of the energy, pressure, and volume of a system. Entropy is a way to determine the different ways energy can be arranged.
To feed the rise in Entropy. Enthalpy is a constant, but Entropy is always increasing.
If the ∆H is positive and the ∆S is positive, then the reaction is entropy driven. If the ∆H is negative and the ∆S is negative, then the reaction is enthalpy driven. If ∆H is positive and ∆S is negative, then the reaction is driven by neither of these. If ∆H is negative and ∆S is positive, then the reaction is driven by both of these.
Enthalpy is the amount of energy released or used when kept at a constant pressure. Entropy refers to the unavailable energy within a system, which is also a measure of the problems within the system.
Synthesis reactions such as dehydration synthesis. For a reaction to proceed the there must be a net decrease in the Gibbs Free Energy of the system. The Gibbs Free Energy is made up of two terms: Enthalpy or Heat Content H Entropy S For a reaction in which the entropy is increasing to proceed there would have to be a sufficient release of heat content (enthalpy) such that Change in Free Energy G would be negative, ie decrease...
Enthalpy- positive Entropy- decreasing Free energy- negative
S > 0 contributes to spontaneity.
The change in enthalpy between products and reactants in a reaction
An increase in entropy.
It tells if the reaction will process spontaneously or not