How many liters of CO2(g) at (3.90 x 10^-4 atm) and (1.2 x 10^3 degrees C) from 5.60L of C4H10(g) at 1.50 atm and 25 degrees C?
Pressure for butane =1.50atm
Volume of butane= 5.60L
Temperature for butane= 27C0 = 298K
Pressure for carbon dioxide= 3.90*10-4atm
Temperature for carbon dioxide = 1.2*103 C0
Volume of carbon dioxide produce= ?
MOLES OF BUTANE
REACTED AT GIVEN CONDITIONS
= 0.3433mol of
MOLES OF CARBON
2mol of butane gives 8mol of carbon dioxide
0.3433 mol gives (8mol of carbon dioxide*0.3433)/2
= 1.3733 mol of carbon dioxide
VOLUME OF CARBON
= (1.3733) (0.0821)
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