a)
We can use the combined gas law:
P1*V1/T1 = P2*V2/T2
We know that: V2 = 0.24 V1
P1 = 1 atm = 101325 Pa
T1 = 10 C = 10+273 = 283 K
T2 = 47 C = 47 + 273 = 320 K
(101325)*V1/(283) = P2*(0.24V1)/320
We then get:
P2 = (320)*(101325)/(283*0.24)
= 477385.159011 Pascals
(b)
Again we have the combined gas law with:
It's because it increased by 3% so,
V2 = 1.03V1
P1 =477385.159011 Pascals
T1 = 47 C = 320 K
T2 = 85 C = 358 K
(477385.159011)(V1)/(320) = (P2)*(1.03V1)/(358)
P2 = (477385.159011)*(358)/(320)*(1.03)
P2 = 518519.074411 Pascals
I hope help you !!
+ 12 points Ser.P10 10 PO MI F My Note An automobile tire is inflated with...
An automobile tire is inflated with air originally at 10.0°C and normal atmospheric pressure. During the process, the air is compressed to 27.0% of its original volume and the temperature is increased to 39.0°C. (a) What is the tire pressure in pascals? (b) After the car is driven at high speed, the tire's air temperature rises to 85.0°C and the tire's interior volume increases by 3.00%. What is the new tire pressure (absolute) in pascals?
An automobile tire is inflated with air originally at 10.0degreesC and normal atmospheric pressure. During the process, the air is compressed to 31.0% of its original volume and the temperature is increased to 33.0degreesC. What is the tire pressure? ___ Pa After the car is driven at high speed, the tire's air temperature rises to 85.0degreesC and the tire's interior volume increases by 2.00%. What is the new tire pressure (absolute)? ____ Pa
An automobile tire is inflated with air originally at 10.0 degree C and normal atmospheric pressure. During the process, the air is compressed to 28.0% of its original volume and the temperature is increased to 40.0 degeree C. What is the tire pressure? After the car is driven at high speed, the tire air temperature rises to 85.0 degree C and the interior volume of the tire increases by 2.00%. What is the new tire pressure (absolute) in pascals?
Air at 10.0◦C and normal atmospheric pressure is pumped into a car tire, which causes the air to compress to 28.0% of its original volume and heat up to 40.0◦C (a) What is the tire pressure? (b) You take the car for a drive at high speeds, and the air temperature in the tire rises to 85.0◦C while the interior volume increases by 2.00%. What is the new absolute pressure (in pascals)?
5. A steel-belted radial automobile tire is inflated to a gauge pressure of 1.75 10 Pa when the temperature is 61 °F. Later in the day, the temperature rises to 101 °F. Assuming the volume of the tire remains constant, what is the gauge pressure at the elevated temperature? (Hint: Remember that the ideal gas law uses absolute pressure.] Pa
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A sample of pure aluminum has a mass of 15.2 g Calculate the number of moles in the sample and aluminum atoms in the sample (a) moles in the same moles (h) aluminum atoms in the sample Need Help? Bbm An Another in -/10 POINTS SERCP11 10.4.P.034.MI. MY NOTES | ASK YOUR TEACHER a ted with air originally at 10.0°C and normal atmospheric pressure. During the process of its original volume and the temperature is increased An automobile tre 45.0...
5. A steel-belted radial automobile tire is inflated to a gauge pressure of 2.00 × 10 5 Pa when the temperature is 62 °F. Later in the day, the temperature rises to 101 °F. Assuming the volume of the tire remains constant, what is the gauge pressure at the elevated temperature? [Hint: Remember that the ideal gas law uses absolute pressure.]
5. A steel-belted radial automobile tire is inflated to a gauge pressure of 2.10 x 10° Pa when the temperature is 68 °F. Later in the day, the temperature rises to 97 °F. Assuming the volume of the tire remains constant, what is the gauge pressure at the elevated temperature? [Hint: Remember that the ideal gas law uses absolute pressure.] Ра
A steel-belted radial automobile tire is inflated to a gauge pressure of 2.15×10^5 Pa when the temperature is 65 °F. Later in the day, the temperature rises to 95 °F. Assuming the volume of the tire remains constant, what is the gauge pressure at the elevated temperature? [Hint: Remember that the ideal gas law uses absolute pressure.]