Math- If the gas is initially at room temperature (20celsius)and is heated in an isobaric (constant pressure) processing then what will be the temperature of gas in degree Celsius when it has expanded to a volume of 0.700 m to the third power

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To solve this question, we need to apply Charles's Law, which states that the volume of a gas is directly proportional to its temperature in Kelvin (assuming constant pressure).

First, let's convert the initial temperature from Celsius to Kelvin. To convert Celsius to Kelvin, we add 273.15. Therefore, the initial temperature will be:

Initial temperature (Kelvin) = 20 + 273.15 = 293.15 K

Next, we need to find the final temperature. We have the initial volume (V1 = 0.700 m^3) and the final volume (V2 = 0.700 m^3), but we don't need the volumes to find the final temperature.

Since Charles's Law states that volume is directly proportional to temperature, we can set up the following ratio:

(V1 / T1) = (V2 / T2)

Where T1 and T2 are the initial and final temperatures respectively. We can rearrange the equation to solve for T2:

T2 = (V2 / V1) * T1

Substituting the values we have:

T2 = (0.700 m^3 / 0.700 m^3) * 293.15 K

The volumes cancel out, leaving:

T2 = 293.15 K

Thus, the temperature of the gas in degrees Celsius when it has expanded to a volume of 0.700 m^3 will still be 20 degrees Celsius since the temperature remains constant in an isobaric process.