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At 103 kPa pressure carbon monoxide turns into a liquid at a temperature of -1920C (81 K). As the temperature is reduced further to -205oC (66K) it solidifies. The critical point of CO is -140oC (132.7 K) with a pressure of 3498 kPa.
These data are very variable around the world.- IUPAC recommendations:a) 0 oC and 100 kPa orb) 25 oC and 100 kPa- NIST recommendation:20 0 oC and 101,325 kPa- methane gas measurements: 15 oCand other values also exist.
0.6
I am going to show you a way of doing this. As 1 atmosphere is equivalent to 1 kPa (101.325 kPa) we can multiply 101.325 * 1.2 to get the pressure in kilopascals. 1.2 * 101.325 = 121.59 kPa We can use the ideal gas law and substitute to find the rest. Remember to use R = 8.314 k/j mol ^-1 for kilopascals and R = 0.0821 for atmospheres pV=nRT 121.59 * 10.5 = 0.49* 8.314 * T 1276.7/4.07386 = T 313.39* C = T But as Temperature is in Kelvin add on 278.15. Therefore, T = 591.54 K
With a surface temperature of only 44 K, and a pressure of only 0.3 Pa, compared to about 287 K and 101 KPa for Earth, not to mention the lack of oxygen or carbon dioxide, it seems unlikely that a plant as we know it could grow on Pluto.No.
580k
60kpa
At 103 kPa pressure carbon monoxide turns into a liquid at a temperature of -1920C (81 K). As the temperature is reduced further to -205oC (66K) it solidifies. The critical point of CO is -140oC (132.7 K) with a pressure of 3498 kPa.
60kpa
LESS
The pressure is 207,5 kPa.
These data are very variable around the world.- IUPAC recommendations:a) 0 oC and 100 kPa orb) 25 oC and 100 kPa- NIST recommendation:20 0 oC and 101,325 kPa- methane gas measurements: 15 oCand other values also exist.
It means Standard Temperature and Pressure.-Standard temperature is equal to 0 °C, which is 273 K.-Standard pressure is equal to 1 atm 760 mmhg or torr and 101.3 KPa.
use the ideal gas last pv=nrt n= same for each one and R=8.314 j/mol*k
The number of moles is 0,03.
IUPAC defines STP as 273.15 K and 100 kPa.
Use the ideal gas equation to solve this. PV= nRT. You will have to convert your pressure to atmosphere to use the constant R = 0.0821 L*ATM/mol*K. You know your initial pressure, volume, and temperature. Moles can be neglected (n) because they will stay the same. You also know your final pressure and final volume, so you can solve for final temperature.