A sample of 02 gas occupies a volume of 1.20L at a pressure 735 mm Hg and a temperature of 225°C. What is the final volume if the temperature is increased to 685°C. and the pressure does not change? HINT: Convert temperature first

Question

A sample of 02 gas occupies a volume of 1.20L at a pressure 735 mm Hg and a temperature of 225°C. What is the final volume if the temperature is increased to 685°C. and the pressure does not change? HINT: Convert temperature first

a.1.30 L O2
b. 4.30 L 02
c. 8.60 L O2
d. 2.30 L Oz
above
e. none of the

Answer 1

above

First, we need to convert the temperature from Celsius to Kelvin:

T1 = 225°C + 273.15 = 498.15 K

T2 = 685°C + 273.15 = 958.15 K

Now we can use the combined gas law to solve for V2:

(P1V1/T1) = (P2V2/T2)

Plugging in the given values:

(735 mmHg)(1.20 L)/(498.15 K) = (735 mmHg)(V2)/(958.15 K)

Simplifying:

V2 = (735 mmHg)(1.20 L)(958.15 K) / (735 mmHg)(498.15 K)

V2 = 2.33 L

Therefore, the final volume is 2.33 L of O2 (option d).