formulas and constants

• Boiling point of water in celsius

  100 degrees
• boiling point in fahrenheit

  212 degrees
• boiling point in rankine

  671.67 degrees
• boiling point in kelvin

  373.15
• freezing point of water

  0 degrees
• freezing point of fahrenheit

  32 degrees
• freezing point of rankine

  459.67 degrees
• freezing point of kelvin

  273.15
• absolute zero in celsius


  -273.15 degrees
• absolute zero in Fahrenheit


  -459.65 degrees
• absolute zero in rankine


  0 degrees
• absolute zero in kelvin


  0
• celsius to fahrenheit


  $f=$$9/5 c +$$32$
• celsius to kelvin


  $k =$$c +$$273.15$
• fahrenheit to celsius


  $c=$$5/9(F-32)$
• fahrenheit to rankine

  $R =$$F+$$459.67$
• mass density


  $\rho =$${\frac {m}{V}}$
• weight density


  $\rho =$${\frac {W}{V}}$
• specific volume

  $v =$${\frac {V}{m}}=$$\frac{1}{\rho m}$
• specific gravity


  
  

  for solid: 1000 kg/m^3

  for gas: 1.4 kg/m^3

  $sp.gr.=$${\frac{\rho substance}{\rho standard}}$
• pressure


  $P =$${\frac {F}{A}}$
• Gauge Pressure


  $Pgauge =$$Pabs-Patm$
• total pressure


  $Ptotal=$$Patm+$$Pgauge$
• pressure gauge


  $P=$${\rho}{h}{g}$
• pascal's principle


  $P1=$$P2$${\frac{F1}{A2}}=$${\frac{F2}{A2}}$
• expansion by length


  $ΔL =$$αLΔT$

  $LN =$$L0 +$$ΔL$
• expansion by volume

  $ΔV =$$βV0ΔT$

  $VN =$$V0 +$$ΔV$

  for almost all types of gases have the

  same value at standard temperature 0℃

  𝛽𝑔𝑎𝑠𝑒𝑠 = 3.66 × 10−3/℃
• FOURIER’S LAW OF THERMAL CONDUCTION


  ${\frac{Q}{t}}=$${\frac{kAΔT}{L}}$
• CONVECTION

  ${\frac{Q}{t}}=$$hAΔT$
• STEFFAN BOLTZMANN LAW


  ${\frac{Q}{t}}=$$σeA((T2)^4 − (T1)^4)$
• sensible heat


  $Q =$$mcΔT$
• specific heat

  For water and ice:

  cw = 1 cal/g-°C

  ci = 0.5 cal/g-°C
• ABSOLUTE ENTROPY


  $S=$${\frac{Q}{TK}}$
• IDEAL GAS LAW


  $𝑃𝑉 =$$𝑛𝑅𝑇$
• UNIVERSAL GAS LAW


  $R=$$8.314{\frac{J}{mol-K}}$$=$$1.986{\frac{BTU}{mol-k}}$$=$$1545{\frac{ft-lb}{mol-K}}$
• BOYLE'S LAW


  $𝑃1𝑉1 =$$𝑃2𝑉2$
• CHARLES' LAW


  ${\frac{V1}{T1}}=$${\frac{V2}{T2}}$
• GAY-LUSSAC'S LAW


  ${\frac{P1}{T1}}=$${\frac{P2}{T2}}$
• THE COMBINES GAS LAW


  ${\frac{P1V1}{T1}}=$${\frac{P2V2}{T2}}$
• Standard conditions STP


  $𝑇 =$$273.15 𝐾 =$$0 °𝐶$

  $𝑃 =$$1 𝑎𝑡𝑚 =$$1.013 × 105 𝑃𝑎$

  Note: Under standard conditions, 1 kmol of ideal gas

  occupies a volume of 22.4 m^3