H and q
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Re: H and q
I believe q denotes heat, which is basically a transfer of energy in chemical reactions. On the other hand, H is enthalpy, which is a state property.
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Re: H and q
q is the measurement for heat (in joules) and H is for enthalpy. While enthalpy is a state property (not dependent on the path taken to obtain that state), heat is not.
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Re: H and q
I think q typically denotes a change in heat energy while H denotes a change in enthalpy.
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Re: H and q
q is the denotation for heat (in joules), which is not a state property, and H is the denotation for enthalpy, which is a state property.
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Re: H and q
q refers to heat whereas H refers to enthalpy. Enthalpy is known as a state function, meaning that if you knew the state of a reaction (how the reaction was before and after it occurred), the enthalpy can be calculated. On the other hand, heat is not a state function and cannot be calculated from the starting and ending states of a reaction.
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Re: H and q
H is for enthalpy and is a state property and q is not so it's for heat! Hope this helps :D
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Re: H and q
ΔH is for enthalpy, which is specifically the energy absorbed/released as heat by a system under constant pressure. It's a state function. Heat, q, is not a state function.
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Re: H and q
The symbol q is intended to express heat and H is to represent enthalpy is a state function while heat is not.
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Re: H and q
q represents the amount of heat released or absorbed in a system in J. Delta H represents the amount of heat released or absorbed AT CONSTANT PRESSURE. So you can think of it like q sub p = deltaH.
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Re: H and q
q is heat, while H is used to describe a change in enthalpy. As we discussed in class, enthalpy is a state function, while heat is focused more on heat released/absorbed from a system.
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Re: H and q
Q refers to heat which is not a state property and H is the enthalpy which is a state function.
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Re: H and q
q is the heat that is transferred to or from a system, and it is not a state function. However, H is the total heat of the system at constant pressure and it is a state function.
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Re: H and q
H is the enthalpy of the system while q is the amount of heat transferred in a system and is used to describe the change in enthalpy.
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Re: H and q
Q represent heat, while H is a state function for enthalpy meaning the change in amount of heat.
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Re: H and q
I think q represents heat, but its not a state function. H is a state function that represents the net heat of a system at a specific pressure.
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Re: H and q
"q" denoted heat, while H represents enthalpy. If I am not mistaken, heat (q) of a gas under constant pressure equals the change in Enthalpy (H). Hope this helps!
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Re: H and q
Q represents heat/energy but is not a state function. H is representative of enthalpy and is a state function.
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Re: H and q
Heat, which is not a state function, is denoted by q, while enthalpy, which is a change in heat at constant pressure, is a state function, and thus, it is denoted by delta H.
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Re: H and q
I believe q can also be used for enthalpy if it is qp or heat absorbed/released at constant pressure.
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Re: H and q
H is for enthalpy and q is for heat but when q is under constant pressure, q=h. This is because enthalpy relates to heat under the terms of constant pressure.
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Re: H and q
q is the measurement of heat (transfer of heat energy) and H is the measurement of enthalpy! Enthalpy is a state function but heat is not. If the system in question is at constant pressure, then I believe delta H is equal to q.
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