Question

Calculate the pressure of dry O2 if the total pressure of O2 generated over water is measured to be 698 Torr and the temperature is 30.1 oC. P(H2O) = 19.8 torr.

If the volume of the O2 sample in the question above was 56.3 ml, what volume would the dry O2 occupy at 755 torr (assume the temp was unchanged).

Answer 1

`V_2=46mL`

Step-by-step explanation:

From the question we are told that:

Pressure over Water
`P=698 Torr`

Temperature
`T= 30.1 \textdegree C`

Pressure of Water
`P(H2O) = 19.8 torr.`

Volume of O2
`O_2=56.3`

Pressure of Dry O2
`P_(0)=755torr`

Generally the equation for Total Pressure is mathematically given by

`P_t = P_O + P_H`

Therefore

`P_O=P_t-P_H`

`P_O=638-19.8`

`P_O=618.2torr`

Generally the equation for Ideal gas is mathematically given by

`P_1*V_1 = P_2*V_2`

`V_2=(P_1*V_1)/(P_2)`

Therefore

`V_2=( 618.2*56.3)/(755)`

`V_2=46mL`

Hence,The volume would the dry O2 occupy at 755 torr

`V_2=46mL`