Answer:

This is a problem involving the combined gas law, which states that:

(P1 Ã V1) / (T1 Ã n1) = (P2 Ã V2) / (T2 Ã n2)

where P is pressure, V is volume, T is temperature, and n is the number of moles of gas.

Assuming that the volume and number of moles of gas remain constant, we can simplify the equation to:

P1 / T1 = P2 / T2

We can solve for T2 by rearranging the equation:

T2 = (P2 Ã T1) / P1

We are given that the pressure increases by a factor of 2, so P2 = 2 à P1 = 2 à 1.20 atm = 2.40 atm. We are also given that the initial temperature is 18°C, which is 291 K (since 0°C = 273 K). Plugging in these values, we get:

T2 = (2.40 atm à 291 K) / 1.20 atm = 582 K

Converting this temperature back to Celsius, we get:

T2 = 582 K - 273 K = 309°C

Therefore, the resulting temperature would be 309°C.

Explanation:

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