A mass of gas has a volume of 4 m3, a temperature of 290 K, and an absolute pressure of 475 kPa. When the gas is allowed to expa
nd to 6.5 m3, its new temperature is 277 K. What's the absolute pressure of the gas after expansion? A. 104.1 kPa
B. 293.9 kPa
C. 279.2 kPa
D. 178.5 kPa
<span>To
solve this we assume that the gas is an ideal gas. Then, we can use the ideal
gas equation which is expressed as PV = nRT. At number of moles the value of PV/T is equal to some constant. At another
set of condition of temperature, the constant is still the same. Calculations
are as follows:</span>
P1V1/T1 = P2V2/T2
P2 = P1 (V1) (T2) / (T1) (V2)
P2 = 475 kPa (4 m^3) (277 K) / (290 K) (6.5 m^3)
P2 = 279.20 kPa
Therefore, the changes in the temperature and the volume lead to a change in the pressure of the system which is from 475 kPa to 279.20 kPa. So, there is a decrease in the pressure.
What part is the independent variable and what part is the dependent variable of the seminary the blood pressure of a soldier is measured while he’s resting soldiers and exposed to a stressful environment and his blood pressure is measured in
When the sun, moon, and Earth are in alignment (at the time of the new or full moon), the solar tide has an additive effect on the lunar tide, creating extra-high high tides, and very low, low tides—both commonly called spring tides.
