ANS:D - unpredictable.

To determine how the pressure changes when the temperature of a gas in a closed container increases, we can use the ideal gas law, which states: 𝑃𝑉=𝑛𝑅𝑇PV=nRT Where:

• 𝑃P is the pressure of the gas,
• 𝑉V is the volume of the gas,
• 𝑛n is the number of moles of the gas,
• 𝑅R is the ideal gas constant, and
• 𝑇T is the temperature of the gas in Kelvin.

Assuming the volume of the gas and the number of moles of gas remain constant (since the container is closed), we can simplify the equation to: 𝑃1𝑇1=𝑃2𝑇2T1​P1​​=T2​P2​​ Where 𝑃1P1​ and 𝑇1T1​ are the initial pressure and temperature, respectively, and 𝑃2P2​ and 𝑇2T2​ are the final pressure and temperature, respectively. Let's calculate the final pressure (𝑃2P2​) when the temperature is increased from 27°C to 300°C. Given:

• 𝑇1=27°𝐶=27+273.15=300.15 KT1​=27°C=27+273.15=300.15K
• 𝑇2=300°𝐶=300+273.15=573.15 KT2​=300°C=300+273.15=573.15K

Using the formula: 𝑃1𝑇1=𝑃2𝑇2T1​P1​​=T2​P2​​ 𝑃1300.15=𝑃2573.15300.15P1​​=573.15P2​​ Rearranging to solve for 𝑃2P2​: 𝑃2=𝑃1×𝑇2𝑇1P2​=T1​P1​×T2​​ Now, if the initial pressure 𝑃1P1​ is not provided, we can't calculate the exact pressure exerted after increasing the temperature. However, we can make a general statement based on the ideal gas law. If the pressure is directly proportional to the temperature in Kelvin (assuming volume and number of moles are constant), then when the temperature increases, the pressure will also increase. Therefore, the correct answer is unpredictable if we don't know the initial pressure. If we had the initial pressure, we could calculate the final pressure.