Answer- diagram ( 3)
Ideal gas constant-
PV= n RT
It T and P is the same
Volume is proportional to number of mole ( molecule)
n1 = .6 mole,
n2 = 2 × .6 mole = 1.2 mole
V1/V2 = n1 / n2 =.6 mole/1.2 mole = 1/2
V2 = 2 × V1
Volume is doubled.
Which diagram (2)-(4) best represents the result of doubling the number of moles of gas while keeping the pressure and temperature constant?
Doubling the gauge pressure of an ideal gas, while keeping the volume of the gas fixed, implies that the temperature changes how? The temperature stays the same. There is not enough information to solve this. The temperature halves
Doubling the gauge pressure of an ideal gas, while keeping the volume of the gas fixed, implies that the temperature changes how?
If you decrease the moles of gas while holding volume and pressure constant, the temperature will __(decrease/increase) because moles and temperature are __(directly/inversely) related to an ideal gas.
Which diagram best represents the final system, if the pressure of the gas in this cylinder were doubled and the temperature increased from 200 K to 400 K?
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