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calculate the final pressure of a gas that is expanded from 725cm³ at 30C and 1.19 atm to 1.12cm³ at 43C​

Sagot :

Lanuel

Answer:

Final pressure, P2 = 1088.89 atm

Explanation:

Given the following data;

Initial volume, V1 = 725 cm³

Initial temperature, T1 = 30°C

Initial pressure, P1 = 1.19 atm

Final volume, V2 = 1.12 cm³

Final temperature, T2 = 43°C

To find the final pressure (P2), we would use the combined gas law.

Mathematically, the combined gas law is given by the formula;

[tex] \frac {PV}{T} = k [/tex]

[tex] \frac {P_{1}V_{1}}{T_{1}} = \frac {P_{2}V_{2}}{T_{2}} [/tex]

Substituting into the formula, we have;

[tex] \frac {1.19*715}{30} = \frac {P_{2}*1.12}{43} [/tex]

[tex] \frac {850.85}{30} = \frac {P_{2}*1.12}{43} [/tex]

[tex] 28.3617 = \frac {P_{2}*1.12}{43} [/tex]

Cross-multiplying, we have;

[tex] 28.3617 * 43 = 1.12P_{2} [/tex]

[tex] 1219.5531 = 1.12P_{2} [/tex]

[tex] P_{2} = \frac {1219.5531}{1.12} [/tex]

Final pressure, P2 = 1088.89 atm

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