Q5.14P - Chemistry: Molecular Nature Of Matter And Change

Question

Convert each of the pressures described below to atm:

(a) At the peak of Mt. Everest, atmospheric pressure is only $2.75\times {10}^2 mmHg$ .

(b) A cyclist fills her bike tires to $86 psi$ .

(c) The surface of Venus has an atmospheric pressure of  $9.15\times {10}^6 Pa$.

(d) At 100 ft below sea level, a scuba diver experiences a pressure of $2.54\times {10}^4 torr$ .

Step-by-Step Solution

Answer

1. The pressure of atmosphere at the peak of Mt. Everest is 0.362 atm.
2. The pressure of the gas in bike is 5.8 atm.
3. The pressure of Venus’s atmosphere is 90.3 atm.
4. The scuba diver experiences the pressure of 33.5 atm.

Step 1: Conversion for (a)

1 atm = 760 mmHg

The conversion of  ${\text{2.75×10}}^{\text{2}} \text{mmHg}$toatm is,

 $2.75\times {10}^2 \text{mmHg×}\frac{\text{1} \text{atm}}{\text{760} \text{mmHg}} \text{ = } \text{0.362} \text{atm}$

Thus, the pressure of atmosphere at the peak of Mt. Everest is 0.362 atm.

Step 2: Conversion for (b)

1 psi = 0.068 atm

The conversion of  toatm is,

 $86 \text{psi} \times \frac{\text{0.068} \text{atm}}{\text{1} \text{psi}} =5.8 \text{atm}$

Thus, the pressure of the gas in bike is 5.8 atm.

Step 3: Conversion for (c)

1 Pa = 9.87x10^-6atm

The conversion of $9.15 \times {10}^6 \text{Pa}$ toatm is,

 $9.15 \times {10}^6 \text{Pa} \times \frac{9.87 \times {10}^{-6} \text{atm}}{\text{1} \text{Pa}} = 90.3 \text{atm}$

Thus, the pressure of Venus’s atmosphere is 90.3 atm.

Step 4: Conversion for (d)

1 Torr = 0.00132 atm

The conversion of $2.54 \times {10}^4 \text{Torr}$ toatm is,

 $2.54\times {10}^4 \text{Torr×}\frac{0.00132 \text{atm}}{\text{1} \text{atm}} = 33.5 \text{atm}$

Thus, the scuba diver experiences the pressure of33.5 atm.