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What would make G become negative at a given enthalpy and entropy?
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What could make G become negative at a given enthaply and entropy?
Changing the temperature. my only explanation is I got it right so I hope this helps.
What explains the entropy change of a gas reaction?
if there is an increase in the number of gas molecules , then ^S > 0
How is the h vaporization used to calculate the mass of liquid boiled by on of energy?
The specific enthalpy of vaporization (usually represented by the letter H with a carat above it) is generally given as units of energy per unit mass or per mole. If given in terms of per unit mass, the mass boiled can be calculated by dividing the energy input by the specific enthalpy. If given in terms of per mole, first divide the energy by the specific enthalpy then multiply the result by the mass per mole.
How do natural systems move toward entropy?
Basically everything will reach an equilibrium, and homogeneous mixture of "everything", if given enough time. Living systems stay living by maintain a specific range of disequilibrium within its components (for the most part). The 2nd Law of thermodynamics states basically that temperature, pressure, and chemical potential goes into equilibrium given enough time. this equilibrium is entropy, when things become compartmentalized (ordered) its always do to living systems.
What blood group is given to someone who is RH negative blood group A?
You would give them A Rh Negative blood or you could also give them O Rh Negative as well. Group O is the universal donor so it can be given to anyone. If the patient is Rh Negative, they can only receive Rh Negative blood. If the patient was Rh positive, they can receive Rh positive or Rh negative.
What could make G become negative at a given enthalpy and entropy?
Changing the temperature
What could make Delta become negative at a given enthalpy and entropy?
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
What could make delta G become negative at a given enthalpy and entropy?
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
What could make G become negative at a given enthaply and entropy?
Changing the temperature. my only explanation is I got it right so I hope this helps.
How is enthalpy related to spontaneity of a reaction?
S > 0 contributes to spontaneity.
Why is the enthalpy change of combustion always negative?
It is and exothermic reaction, which means energy is given out heating the surroundings.
Define enthalpy and how it is measured?
Enthalpy is a particular amount of heat that is produced or released at a given pressure. There are specific equations that must be used to calculate enthalpy.
When does entropy increases?
Entropy increases when ever energy is used up. Energy cannot be destroyed, but it is always lost in the form of unusable energy. Entropy is the % of unusable energy compared to usable energy in a given system.
What part is in charge of automatic processes?
In science, Gibbs free energy can tell if a chemical reaction is spontaneous. It is given by the formula: G = H - TS H = enthalpy of reaction S = entropy of reaction T = temperature in Kelvin If G is negative the reaction is spontaneous. However if activation energy is high, reaction rate is slow and the reaction may take a while to progress, regardless of its spontaneity.
Heat given off or absorbed in a reaction is called?
Enthalpy
The amount of useable energy decreases when?
The quality of energy decreases when you use it due to the second law of thermodynamics. Essentially, the energy spent from various reactions is processed, which reduces the amount of work needed to extract it.
Calculate the entropy of vaporization per mole of ethanol Given enthalpy change is 109.8 JK-1 mol-1 and boiling point of ethanol is 78.50C?
OK.With entalpy od vaporization and temperature of vaporization is very easy to calculate entropy of vaporization of etanol.So the equation to calculate this is:Delta_S=-Delta_H/TbWhere:Delta_S= Entropy of vaporizationDelta_H=Entalpy of vaporizationTb= Normal Boiling point temperatureSo the Delta_S become:Delta_S=-(-109000.8)/(78.5+273)Delta_S=310.1 J.mol-1.K-1
