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approximately 240 ml / min of CO2 is exhaled by an average adults at rest . Assuming a temperature of 37°C and 1 atm pressure how many mol/ min of CO2 is this ? n = ... mol/ min

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you have to find the number of moles 240 ml of gas is at 37°C and 1 atm.  To do this you need to use PV=nRT and solve for n.(n=PV/RT)
remember that the ideal gas law requires that the volume be in liters and temperature be in kelvin so you need to convert 37°C to kelvin and 240 mL to liters.
37°C+273K=310K
240mL=0.240L
Even though R is not given, it is a constant and therefore we know that it can be 0.08206atmL/molK.
plug everything in.
n=(1atmx0.240L)/(0.08206atmL/molKx310K)
n=0.00943mol
since we were told that 240ml of air exhaled per minute and we know now that 240ml of air at the given conditions is 0.00943mol, we can say that the average adult exhales 0.0094 moles per minute.
The answer is 0.00943mol/min
okpalawalter8

We have that for the Question "approximately 240 ml / min of CO2 is exhaled by an average adults at rest . Assuming a temperature of 37°C and 1 atm pressure how many mol/ min of CO2 is this ? n = .. mol/ min" it can be said that he moles of CO_2  exhaled per min is

  • n=9.43m

From the question we are told

approximately 240 ml / min of CO2 is exhaled by an average adults at rest . Assuming a temperature of 37°C and 1 atm pressure how many mol/ min of CO2 is this ? n = .. mol/ min

Generally the equation for the ideal gas  is mathematically given as

[tex]PV=nRT\\\\n=\frac{PV}{RT}\\\\Therefore\\\\n=\frac{1*240}{0.08206*310.15}\\\\[/tex]

n=9.43mol

The moles of CO_2  exhaled per min

  • n=9.43mol

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