Un gas se encuentra a una presión constante y a una temperatura de 30°C. Si la temperatura aumenta a 45°C, su presión varía a 6 atm. ¿Cuál e

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Un gas se encuentra a una presión constante y a una temperatura de 30°C. Si la temperatura aumenta a 45°C, su presión varía a 6 atm. ¿Cuál era la presión inicial del gas? Transforma los °C en °K.

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Neala 3 years 2021-08-31T16:33:11+00:00 1 Answers 8 views 0

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  1. Eirian
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    2021-08-31T16:34:27+00:00
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    Answer:

    P1 = 5.76 atm

    Explanation:

    To find the initial pressure of the gas you use the equation for ideal gases, for both temperatures and pressures:

    P_1V=nRT_1\\\\P_2V=nRT_2\\\\

    T1: initial temperature = 30°C = 303.15K

    T2: final temperature = 45°C = 318.15K

    P1: initial pressure = ?

    P2: final pressure = 6atm

    n: number of moles

    R: ideal gas constant

    The number of moles and R are constant, you can dive the first equation into the second and solve for P1:

    \frac{P_1V}{P_2V}=\frac{nRT_1}{nRT_2}\\\\\frac{P_1}{P_2}=\frac{T_1}{T_2}

    P_1=\frac{T_1P_2}{T_2}

    Finally, you replace the values of T1, P2 and T2:

    P_1=\frac{(303.15K)(6atm)}{318.15K}=5.71atm

    hence, the initial pressure of the gas was 5.71 atm

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