Q5.9P - Chemistry: Molecular Nature Of Matter And Change

Question

Convert the following:

(a) 76.8 cmHg to atm          (b) 27.5 atm to kPa

(c) 6.50 atm to bar               (d) 0.937 kPa to torr

 

Step-by-Step Solution

Answer

1. The pressure of 76.8 cmHg in atm units  is 1.01 atm.
2. The pressure of 27.5 atm in kPa unit is 2786 kPa.
3. The pressure of 6.50atm in bar unit is 6.59 bar.
4. The pressure of 0.937 kPa in torr unit is 7.03 torr.

Step 1: Conversion for (a)

Convert the unit from cmHg to mmHg,

 $\text{1} \text{cmHg = } \text{10} \text{mmHg}$

$\text{76.8} \text{cmHg} \times \frac{\text{10} \text{mmHg}}{\text{1} \text{cmHg}} \text{ = } \text{768} \text{mmHg}$

 $\text{atm} \text{ = } \text{760} \text{mmHg}$

 The conversion of  $\text{768} \text{mmHg}$ to atm is,

 $\text{768} \text{mmHg×}\frac{\text{1 atm}}{\text{760} \text{mmHg}} \text{ = } \text{1.01} \text{atm}$

Thus, the pressure in the atm unit is 1.01 atm.

 

Step 2: Conversion for (b)

 $\text{101.325} \text{kPa} \text{ = } \text{1} \text{atm}$

The conversion of 27.5 atm to kPa is,

 $\text{27.5} \text{atm} \times \frac{\text{101.325} \text{kPa}}{\text{1} \text{atm}} \text{ = } \text{2786} \text{kPa}$

Thus, the pressure in the kPa unit is 2786 kPa

Step 3: Conversion for (c)

 $\text{atm} \text{ = } \text{1.01325} \text{bar}$

The conversion of 6.50 atm to bar is,

 $\text{6.5} \text{atm} \times \frac{\text{1.01325} \text{bar}}{\text{1} \text{atm}} \text{ = } 6.59 \text{bar}$

Thus, the pressure in bar unit is 6.59 bar.

Step 4: Conversion for (d)

Convert kPa into atm,

 $\text{101.325} \text{kPa} \text{ = 1atm}$

 $0.937 \text{kPa×}\frac{\text{1 atm}}{\text{1} 01.325 \text{kPa}} \text{ = } 0.009247\text{atm}$

 

The conversion of 0.009247 atm to torrs is,

1 atm = 760 torr

 $0.009247\text{atm} \times \frac{\text{760} \text{torr}}{\text{1} \text{atm}} \text{ = } 7.03 \text{torr}$

Thus, the pressure in torr unit is 7.03 torr.