A gas is in a container at a pressure of 38.6 atm and a temperature of 16.5 °C. What will the final pressure be if the temperature is increased to 37.9 °C? (Round your answer to 1 decimal place.)

The final pressure of the gas in the container, after the temperature increase from 16.5°C to 37.9°C, is approximately 41.6 atm.

To calculate the final pressure, we can use the ideal gas law and the relationship between pressure and temperature in a constant volume system. The formula we'll use is P1/T1 = P2/T2, where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature.

First, convert the temperatures to Kelvin by adding 273.15 to each. T1 = 16.5°C + 273.15 = 289.65 K and T2 = 37.9°C + 273.15 = 311.05 K.

Now, we can use the formula: (38.6 atm / 289.65 K) = (P2 / 311.05 K). To solve for P2, multiply both sides by 311.05 K: P2 = (38.6 atm / 289.65 K) * 311.05 K. Calculate P2 to get approximately 41.6 atm as the final pressure, rounded to one decimal place.

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