Liquid butane (C4H10) is stored in cylinders to be used as a fuel...

Question

Liquid butane (C4H10) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as -0.5 °C. (c) How much heat must be added to vaporize 250 g of butane if its heat of vaporization is 21.3 kJ/mol? What volume does this much butane occupy at 755 torr and 35 °C?

Accepted Answer

Everyone. So here we have propane which is C2H8 and has a normal boiling point of negative 42 degrees Celsius and the entropy of vaporization is 14. kg per mole will ask how the heat that must be added to convert 300 g of propane into vapor and determine the volume of this propane gas that occupies its 765 tour and 40 degrees Celsius. So for this we're gonna use our occasion heat. It was mauled as an entropy of vaporization. We need to first find the moles of propane using the molar mass. They have 300 g propane And then one more of propane, the mother mass. And this is three Times 12.011g plus eight Times 1.008g. They get 44.097 g per mole. These cancel out and we left the malls of propane. Let's give us 6.8 malls in Q. Is what we're looking for. For malls. We have 6.8 malls for the entropy of vaporization. We're given this which is 14.79. They'll just promote. Now we're gonna plug in our values. So for cute. There are 6.8 moles 14. they'll just promote, Let me get 101 killed Jules. Now we're gonna use our ideal gas equation to find the volume of the propane gas and this is the pressure times volume equal to the number of moles times of our gas constant times the temperature in kelvin. If we rearrange this is all for volume, we're going to get volume. It was N R T I P. Our pressure 765 Tour. But we need to convert this to atmosphere 760 tour in one atmosphere. I get 1.0066 atmosphere for volume is what we're looking for. The number of moles of 6.8 malls For the r gas constant of 0.08206. Later sounds atmosphere provided by malls times kelvin. For our temperature We have 40°C. We need to convert to Kelvin. We need to add 273.15. We get 3 - 13.15 Kelvin. Now if we plug in the values to solve for the volume, you get volume equals 6.8 malls Time 0.08 206. There's some atmosphere by by Moles and Kelvin 313 15 Kelvin By 1.0066 atmosphere. They get 174 leaders. Thanks for watching my video and I hope it was helpful

Liquid butane (C4H10) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as -0.5 °C. (c) How much heat must be added to vaporize 250 g of butane if its heat of vaporization is 21.3 kJ/mol? What volume does this much butane occupy at 755 torr and 35 °C?

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