Fill a balloon with helium gas to a volume of 2.68 L at 23 celsius and 789mmHg. What would the volume of helium if the pressure changes to 632 mmHg but the temperature is unchanged.
This is how I solved it
V2 = V1 X P1/P2
2.68L X 789/632 =
ANSWER
V2 =.3.35 L
Is this correct
looks ok to me.
Yes, your calculation is correct. Using the formula V2 = V1 * P1/P2, where V1 is the initial volume (2.68 L), P1 is the initial pressure (789 mmHg), and P2 is the final pressure (632 mmHg), you correctly substituted the values and obtained V2 = 3.35 L. Therefore, the volume of helium would be 3.35 L if the pressure changes to 632 mmHg while the temperature remains unchanged.
Yes, your calculation is correct. You used the formula V2 = V1 X P1/P2 to solve for the new volume of the helium gas.
V2 represents the new volume, which is what we are trying to find.
V1 is the initial volume, which is given as 2.68 L.
P1 is the initial pressure, which is given as 789 mmHg.
P2 is the final pressure, which is given as 632 mmHg.
By plugging in these values into the formula, you get:
V2 = 2.68 L X (789 mmHg / 632 mmHg)
V2 = 2.68 L X 1.25
Calculating this, you get:
V2 = 3.35 L
So, the new volume of the helium gas would be 3.35 L if the pressure changes to 632 mmHg while the temperature remains unchanged.