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Sagot :
Answer:
Explanation:
From the ideal gas law, we know that
[tex]PV=\text{nrT}[/tex]where
P = pressure
V = volume
n = number of moles of gas
r = gas constant
T = temperature.
Know in our case, we know that for a certain number of moles, if V = 0.525 m^3 , P = 485 kPa, then T = -14 celsius. Putting these values (by first converting them to metric units) gives
[tex](0.525m^3)(485\cdot10^3P)=nr(-14+273.15K)[/tex]solving for nr gives
[tex]nr=\frac{(0.525m^3)(485\cdot10^3P)}{(-14+273.15)K}[/tex]which evaluates to
[tex]nr=982.54[/tex]With the value of n*r in hand, we now find the pressure at 42 degrees celsius:
[tex]P(0.525m^3)=(982.54)(42+273.15)K[/tex]Solving for P ( the pressure) gives
[tex]P=\frac{(42+273.15)(982.54)}{0.525}[/tex][tex]P=589805\approx589.805\text{kpa}[/tex]The new gauge pressure is 589.805 kPa.
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