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15 Cards in this Set
- Front
- Back
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Heat definition |
kind of energy which is possibly transferred from a body or a system to another due to temp difference provided that those systems are completely isolated (heat energy transfer). |
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Thermal equilibrium |
Physical state at which temperature of two systems stabilize T1=T2 |
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temperature of two systems stabilize due to: |
1.Ultimate contact 2.Heat loss at constant range in both systems |
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Zero Law in Thermodynamics |
Whenever possible to have two systems in individual thermal equilibrium with third party, then it is possible to indicate that those systems are in thermal equilibrium with each other. |
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Ways of temp measurement |
Direct- using thermo-meter In direct - using quantities affected by temperature difference such as (fluids volume, gas pressures, length of metallic materials, etc.) |
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Celsius and Fahrenheit conversion |
𝐓c =𝟓/9(𝐓f −𝟑𝟐)
𝐓f =(𝟑𝟐 + 9/𝟓 𝐓c) |
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Celsius to kalvin conversion |
TK = (TC + 273.16) |
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What is the ideal Gas |
assumes identical gas point molecules with no interactions, Ideal for expression of low density gases where no molecules are formed but only individual atoms |
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Relation between gas volume and pressure |
PV/T=C PV = C (Cons T) - boyles law P/T= C (Cons V)- Lusacs law V/T = C(Cons P) - Charles law |
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Ideal gas law |
PV= nRT
R = 8.314 j/k/mole STP= 0C & 1atm=1.013×10^5Pa |
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Thermal system |
thermal sample or material placed at thermal environment. |
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Types of thermal systems |
x Closed system: Heat transfer occurs under no mass change x Open system: Heat transfer occurs under mass change xAdiabatic system: No heat transfer is possible |
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Energy conservation law states |
‘Energy can neither be created nor destroyed; rather, it transforms from one form to another’ |
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1st law of thermodynamics states: |
‘Thermal energy absorbed by a thermal system= internal energy change plus work done by the system’ Q= >U + W - Q = Thermal energy absorbed (+Q if added / -Q if taken) in Joules - ΔU= Internal energy change (+ΔU if it is added /-ΔU if taken) in Joules,cal -W= Work achieved (+ W if done by the system / - W if done at the system) in joules |
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Work for gases |
ΔW = P (V2-V1) -P: Gas Pressure (in Pascal) -V: Gas Volume (in m3) |
