CHEM101 Lecture Notes - Lecture 19: Ideal Gas Law, Airbag, Stoichiometry
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25 May 2018
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CHEM101- Lecture 19
Charles’ Law
● As the temperature increases, the volume increases
𝑣 = 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑥 𝑇
𝑉
𝑇= 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡
𝑣1
𝑇1
=𝑣2
𝑇2
Example:
𝑉1=750 𝑚𝐿
𝑇1= −10 ℃
𝑉2= ?
𝑇2=25 ℃
● First convert ℃ to Kelvin
𝑇1= −10 ℃→263 𝐾
𝑇2=25 ℃ → 298 𝐾
● Then plug into Charles’ Formula
750 𝑚𝐿
263 𝐾 =𝑉2
298 𝐾 → 𝑉2+(750 𝑚𝐿)(298 𝐾)
263𝐾=850 𝑚𝐿
Confined Gas Law
𝑃1𝑉1
𝑇1
=𝑃2𝑉2
𝑇2
Example:
𝑉1=6.0𝐿
𝑃1=1.0 𝑎𝑡𝑚
𝑃2= .45 𝑎𝑡𝑚
𝑇1=22 ℃→ 295 𝐾
𝑇2= −21 ℃→252 𝐾
𝑉2= ?
(1.0 𝑎𝑡𝑚)(6.0 𝐿)
295 𝐾 =(.45 𝑎𝑡𝑚)(𝑉
2)
252 𝐾 →(252 𝐾)(1.0 𝑎𝑡𝑚)(6.0 𝐿)
(295𝐾)(.45 𝑎𝑡𝑚)
𝑉2=11 𝐿
Avogadro’s Law
2 𝐻2(𝑔) + 1 𝑂2 (𝑔) → 2 𝐻2𝑂 (𝑔)
2 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠: 1 𝑚𝑜𝑙𝑒𝑐𝑙𝑒 ∶ 2 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠
2 𝑚𝑜𝑙𝑒𝑠: 1 𝑚𝑜𝑙𝑒: 2 𝑚𝑜𝑙𝑒𝑠
2 𝑣𝑜𝑙𝑢𝑚𝑒𝑠: 1 𝑣𝑜𝑙𝑢𝑚𝑒: 2 𝑣𝑜𝑙𝑢𝑚𝑒𝑠
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