What Is The Difference Between Specific Heat Capacity, Heat Capacity, and Molar Heat Capacity

This chemistry video tutorial explains the difference between specific heat capacity, heat capacity, and molar heat capacity. It contains a few examples and practice problems on calculating the specific heat capacity and molar heat capacity of a substance. It provides all of the equations and formulas needed to the heat capacity.
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[@TheOrganicChemistryTutor]

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[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for explaining/analyzing the difference between Specific Heat Capacity, Heat Capacity and Molar Heat Capacity in AP/General Chemistry. The different formulas /equations are needed for all specific heat problems in Chemistry. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.

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[@arift.dogan.youtube]

The SI unit for heat capacity of an object is joule per kelvin (J/K, or J K−1). Since an increment of temperature of one degree Celsius is the same as an increment of one kelvin, that is the same unit as J/°C.

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[@loganmitchell]

A lot of confusion on why specific heat is not dependent on mass is you divide out mass. Specific Heat does not depend on mass because q does, so when you divide out m you are taking away the dependence of mass from q thus making the final product not dependent on mass

[@Fesrab]

It’s not q which has the mass term, is the delta t which is dependent on mass. The temperature change only could have happened with a specific mass and a specific q

[@unnamedchannelowouwu]

@@Fesrab it'a q because q=mc∆t so q does depend on mass

[@HappyGardenOfLife]

@@unnamedchannelowouwu molar heat capacity isn't dependent on mass either, but it divides by moles instead of grams. How does it cancel out mass?
Edited: It's because q = ncΔT in that equation.

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is there a table of state transition temperature coeficents of elements, for calculating temperature of state transition in relation of external pressure???

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[@ayadmonicar.7843]

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[@supernova7321]

Why was the specific heat capacity formula used in the first exercise instead of the heat capacity formula since both substances have the same mass?

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[@Chelsea-gs7qj]

how can heat capacity be related to mass if it is not included in the formula? Likewise, you said the specific heat is not affected by mass but it is included in the formula???

[@sathyalakshmis2313]

Chelsea I was wondering about the same
thing

[@eternallolicon9578]

U can use the mass to find the specific heat capacity, but if the mass increases, the specific heat capacity stays the same

[@mohamedmagdy299]

Mass is in heat's formula
Q=mc∆T

[@yepyeniceri]

For simplicity's sake remove the temperature.
Heat capacity is xJ. It is not a ratio with mass value. It is not x joule for y gram. So it is independent of a specific mass value. It can be dependent of any mass value.
Specific heat capacity is xJ : 1g. X joules per 1 gram. It already depends a mass value which is 1 gram. So ratio only works for 1 gram, does not depend on another mass value.

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[@medgirl8792]

so if specific heat capacity does not depend on the mass then why do we use mass in its formula??

[@hunterswartz6389]

great question, seemed like such an obvious place to get confused and he just flew right over it

[@user-vq5hb5cp4n]

how does the specific heat capacity not depend on mass when it's in the equation

[@suhail_vakeel]

Think of it as density
Density is mass per unit volume d=m/v but it is independent of both mass and volume
In case of density if you increase volume the subsequent increase in mass will compensate from it
Over all ratio will be constant
You learn many terms like this eg capacitance is good example it is equal to charge per unit potential
But independent of both charge and potential

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[@hayden3511]

Calculate the amount of heat required to raise the temperature of 100.0g of water from 30.1degrees Celsius to 70.1degrees Celsius. The molar heat capacity of water is 75.3J/mol degrees Celsius. what do I do?

[@greenhighlightersrulethewo4009]

use the specific heat of water

[@pew7217]

Just multiply molar heat (75.3) by the number of moles in 100g of water, all other info is useless.
Answer: (75.3)* (5.5 moles) = 418.3 Joules/degree Celsius.

[@creativeink4407]

@@pew7217 dont you also have to multiply by a hundred too

[@saarza9991]

Cm= Q/n∆T
> Q= Cm.n∆T
>Cm= 75.3J/m °C
>n= given mass/molar mass= 100g/18g=5.5mol
>∆T= 70.1-30.1= 40K or 40°C
Hence, Q= 75.3×5.5×40=16566J
Hence, amount of heat required = 16.566kJ

[@kayden492]

16.5 J

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