Answer:
You need to use the equations of motion which I wrote down in the image. Since the runner starts from rest, the initial velocity(v0) is 0 and initial position(x0) is also 0. The solution is in the image attached below.
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Answer:
the question is incomplete, here is the complete question.
"On a chilly 12∘C day, you quickly take a deep breath--all your lungs can hold, 4.0 L. The air warms to your body temperature of 37∘C.If the air starts at a pressure of 1.0 atm, and you hold the volume of your lungs constant (a good approximation) and the number of molecules in your lungs stays constant as well (also a good approximation), what is the increase in pressure inside your lungs?
1.09 atm
Explanation:
the question addresses an ideal gas. where the relationship between the volume(v),pressure(p),temperature(T) and nos of molecules(n) is expressed as
Where R us the ideal gas constant.
From the question,the number of molecules,volume are constant, we can now re-write the equation as
where pressure and temperature are the only varying parameters.
if we vary the constant K we arrive at
since the Temprature must be in absolute temperature, we add 273k to it Celsius value.
Substituting value into the generated equation, we have