Question

The boiling temperature of water is directly related to the atmospheric pressure. At sea level, the atmospheric pressure is 760 torr whereas the boiling temperature is 100equationC. If the atmospheric pressure is lower than 760 torr, then the boiling temperature will be less than 100equationC. If the atmospheric pressure is higher than 760 torr, then you would expect the boiling temperature to be higher than 100equationC. At higher elevations, the atmospheric pressure is lower resulting in a lower boiling temperature. For example: Denver, CO experiences a boiling temperature at ~ 94equationC. If you were conducting an experiment that involved boiling water, what would you expect the boiling temperature to be if the atmospheric pressure was 790 torr

Answer 1

Answer:

If the atmospheric pressure is lower than 760 torr, then the boiling temperature will be less than 100equationC.

B. 97.7°C

Explanation:

The question mentions the fact that temperature and pressure are directly proportional. This means that if one quantity is increasing the other increases simultaneously and vice versa.

Hence, if the atmospheric pressure is lower than 760 torr, then the boiling temperature will be less than 100equationC.

From;

PαT

P=kT

Hence

P/T = k

P1/T1 = P2/T2

P1T2 = P2T1

P1 =  760 torr

T1 = 94°C

T2 = ?

P2 = 790 torr

T2 =  P2T1/P1

T2 = 790 * 94/760

T2 = 97.7°C