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

Answer:

$V_2=46mL$

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

$P_1*V_1 = P_2*V_2$

$V_2=\frac{P_1*V_1}{P_2}$

Therefore

$V_2=\frac{ 618.2*56.3}{755}$

$V_2=46mL$

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

$V_2=46mL$