Powdered charcoal, C(s), ignites spontaneously in F2 (g) at room temperature and forms carbon tetrafluoride, CF4 (g). What volume of CF4 at 20C and 760Torr will be produced by reacting 250mL of F2 at 20C and 1200Torr with 26.2mg of charcoal?
I know the answer is 52.4mL. I attempted to solve this problem, but couldn't figure it out? Help please and thank you!
I know the answer is 52.4mL. I attempted to solve this problem, but couldn't figure it out? Help please and thank you!
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C + 2F2 --> CF4
PV = nRT
1. atm*.V=n*0.0821*(273+20)
26.2mg/1000=.0262g C(s)
.0262g(1 mole/12g C)=.002183 mle C
1. atm*.V=.002183*0.0821*(273+20)
V=.052400L
.052400L(1000ml/L)=52.4ml
PV = nRT
1. atm*.V=n*0.0821*(273+20)
26.2mg/1000=.0262g C(s)
.0262g(1 mole/12g C)=.002183 mle C
1. atm*.V=.002183*0.0821*(273+20)
V=.052400L
.052400L(1000ml/L)=52.4ml