A syringe containing 1.63 mL of oxygen gas is cooled from 91.0 ∘C to 0.9 ∘C. What is the final volume Vf of oxygen gas? (Assume that the pressure is constant.) Vf = nothing mL Request Answer Provide Feedback

Vf = 1.22 mL

Explanation:

If we assume that the pressure is constant and the number of moles does not change, we can say that the volume of the gas is modified in a directly ratio, to the Absolute Temperature.

Let's convert the values:

91°C + 273 = 364K

0.9°C + 273 = 273.9K

Volume decreases if the temperature is decreases

Volume increases if the T° increases

V₁ / T₁  = V₂ / T₂ → 1.63mL /364K = V₂ / 273.9K

V₂ = (1.63mL /364K) . 273.9K → 1.22 mL

The final volume of the oxygen gas is 1.23 mL

Explanation:

Step 1: Data given

Volume of the syringe = 1.63 mL = 0.00163 L

Initial temperature = 91.0°C = 364.15 K

Final temperature = 0.9 °C = 274.05 K

Step 2: Calculate the final volume

V1/T1 = V2/T2

⇒with V1 = the initial volume = 0.00163 L

⇒with T1 = the initial temperature = 364.15 K

⇒with V2 = the final volume = TO BE DETERMINED

⇒with T2 = the final temperature = 274.05 K

0.00163/364.15 = V2 / 274.05

V2 = 0.00123 L = 1.23 mL

The final volume of the oxygen gas is 1.23 mL

if you mean hydrogen and oxygen then water is the product