A7 l sample of gas has a pressure of 1.1 atm at a temperature of 285 k. if the pressure decreases to 0.6 atm, causing the volume to increase to 10 l, what is the new temperature? round your answer to the nearest tenth.

Answer : The new temperature is, 222.1 K

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

where,

= initial pressure of gas = 1.1 atm

= final pressure of gas = 0.6 atm

= initial volume of gas = 7 L

= final volume of gas = 10 L

= initial temperature of gas = 285 K

= final temperature of gas = ?

Now put all the given values in the above equation, we get:

Therefore, the new temperature is, 222.1 K

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  the grams     of oxygen gas   that can be produced     is 20.6   grams of o₂

calculation

2liclo₃ →   2 licl + 3 o₂

step 1:   find the moles of liclo₃

moles = mass÷ molar mass

from periodic table the molar mass of liclo₃ =6.9 +35.5   +(16 x3) =90.4 g/mol

moles=38.7 g÷90.4 g/mol=0.4281   moles

step 2:   use the   mole ratio   to calculate the moles of o2

from equation above, liclo₃: o₂   is 2: 3  

therefore the moles of   o₂=0.4281 moles x3/2 =0.6422   moles

step 3: find mass   of o₂

mass= moles x molar mass

from periodic table the   molar mass of   o₂ = 16 x2= 32 g/mol

mass=0.6422   moles   x   32 g/mol = 20.6 grams of o₂