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blackjack18
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If 0.5 mol of nitrigen gas occupies a volume of 11.2 L at 0 degrees Celsius, what volume will 2 mol of nitrogen gas occupy at the same temperature and pressure?
blackjack18 said:If 0.5 mol of nitrigen gas occupies a volume of 11.2 L at 0 degrees Celsius, what volume will 2 mol of nitrogen gas occupy at the same temperature and pressure?
blackjack18 said:all i really need help with is the pressure... i have the formula for the problem i think (boyle's law) but i do not know the what the pressure is...
blackjack18 said:is 44.8 L/mol is the answer?
blackjack18 said:i don't know...boyles law states P x V = constant...and i don't know what the pressure is
blackjack18 said:Should Boyle's Law be used in this problem, since the temperature remains constant:
What is the volume of an ideal gas at 1 atm, 12 L, and 25 degrees Celsius if the pressure is decreased to 0.8 atm at 25 degrees Celsius?
blackjack18 said:is the answer v2=15 L?
"2 mol N2" refers to the amount of nitrogen gas present in the given volume. One mole of any substance contains 6.022 x 10^23 particles, in this case, nitrogen molecules. Therefore, 2 moles of N2 would contain 2 x 6.022 x 10^23 particles.
The temperature of 0°C is the standard temperature used in scientific calculations. It is equivalent to 273.15 Kelvin (K) or 32°F. This helps to establish a common reference point for comparing different volumes of gases.
The pressure of 1 atmosphere (atm) is the standard pressure used in scientific calculations. At this pressure, the volume of a gas is directly proportional to its temperature. This means that as the temperature increases, the volume of the gas will also increase, and vice versa.
"11.2 L" is the volume of the gas, nitrogen (N2), at 0°C and 1 atm pressure. This means that if 2 moles of N2 gas are present at 0°C and 1 atm, it will occupy a volume of 11.2 liters.
At the same conditions of 0°C and 1 atm, the volume of 2 mol N2 is equal to the volume of any other gas. This is because the volume of a gas is directly proportional to its temperature and pressure, regardless of the type of gas present.