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23 January, 10:34

A sample of diborane gas a substance that bursts into flame when exposed to air, has a pressure of 345 tore at a temperature of - 15C and a volume of 3.48 L. If conditions are changed so that the temperature is 36C and the pressure is 468 tore, what will be the volume of the sample?

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  1. 23 January, 10:48
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    3.072 L

    Explanation:

    We are given;

    Initial pressure, P₁ = 345 torr Initial temperature, T₁ = - 15°C

    But, K = °C + 273

    = - 15°C + 273

    = 258 K

    Initial volume, V₁ = 3.48 L Final pressure, P₂ = 468 torr Final temperature, T₂ = 36°C

    = 36 °C + 273

    = 309 K

    We are required to calculate the new volume, V₂

    Using the combined gas law;

    P₁V₁/T₁ = P₂V₂/T₂

    We can calculate the new volume, V₂; Rearranging the formula;

    V₂ = (P₁V₁T₂) : (T₁P₂)

    = (345 torr * 3.48 L * 309 K) : (258 K * 468 torr)

    = 3.072 L

    Therefore, the new volume of the sample is 3.072 L
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