If a gas occupies 79.5 mL at -1.4°C, what temperature, in Kelvin, would it have if the volume was reduced to 35.3 mL and the pressure

Question

If a gas occupies 79.5 mL at -1.4°C, what temperature, in Kelvin, would it
have if the volume was reduced to 35.3 mL and the pressure is held constant?
constant?

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Xavia 5 months 2021-08-23T11:58:43+00:00 1 Answers 2 views 0

Answers ( )

    0
    2021-08-23T12:00:39+00:00

    Answer:

    121 K

    Explanation:

    Step 1: Given data

    • Initial volume (V₁): 79.5 mL
    • Initial temperature (T₁): -1.4°C
    • Final volume (V₂): 35.3 mL

    Step 2: Convert “-1.4°C” to Kelvin

    We will use the following expression.

    K = °C + 273.15 = -1.4°C + 273.15 = 271.8 K

    Step 3: Calculate the final temperature of the gas (T₂)

    Assuming ideal behavior and constant pressure, we can calculate the final temperature of the gas using Charles’ law.

    V₁/T₁ = V₂/T₂

    T₂ = V₂ × T₁/V₁

    T₂ = 35.3 mL × 271.8 K/79.5 mL = 121 K

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