Question

If the flask is open to the atmosphere, the mercury levels are equal. for each of the following situations where a gas is con tained in the flask, calculate the pressure in the flask in torr, at mospheres, and pascals. c. calculate the pressures in the flask in parts a and b (in torr) if the atmospheric pressure is 635 torr.

Answer 1

When the flask is open to the atmosphere, the pressure inside the flask is equal to the atmospheric pressure. If the atmospheric pressure is 635 torr, then the pressure in the flask would also be 635 torr. The pressure in the flask can be converted to atmospheres by dividing the pressure in torr by 760 and to pascals by multiplying the pressure in torr by 133.32.

Step-by-step explanation:

When a gas is contained in an open flask, the pressure inside the flask is equal to the atmospheric pressure. In this case, since the mercury levels are equal, the pressure inside the flask is the same as the atmospheric pressure. If the atmospheric pressure is 635 torr, then the pressure in the flask (in torr) would also be 635 torr. The pressure in the flask can be converted to atmospheres by dividing the pressure in torr by 760 (since 760 torr is equal to 1 atm). So, the pressure in the flask would be 635 torr / 760 torr/atm = 0.835 atm. To convert the pressure in torr to pascals, multiply the pressure in torr by 133.32 (since 133.32 Pa is equal to 1 torr). So, the pressure in the flask would be 635 torr * 133.32 torr/Pa = 84604.2 Pa.