To solve this problem, we can use the ideal gas law, which states that the volume of a gas is directly proportional to its temperature and inversely proportional to its pressure. However, since the pressure remains constant in this problem, we can simplify this to a direct relationship between volume and temperature.

The formula we will use is V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.

First, we need to convert the temperatures from Celsius to Kelvin, because the ideal gas law requires temperatures to be in Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 34.01C + 273.15 = 307.16K
And, T2 = 30.18C + 273.15 = 303.33K

Now we can plug these values into our formula:

25.22L / 307.16K = V2 / 303.33K

To solve for V2, we multiply both sides by 303.33K:

V2 = 25.22L * 303.33K / 307.16K

V2 = 24.92L

So, if the temperature is changed to 30.18C and the pressure remains constant, the volume of the balloon will be approximately 24.92 liters.

Question

To solve this problem, we can use the ideal gas law, which states that the volume of a gas is directly proportional to its temperature and inversely proportional to its pressure. However, since the pressure remains constant in this problem, we can simplify this to a direct relationship between volume and temperature.

The formula we will use is V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.

First, we need to convert the temperatures from Celsius to Kelvin, because the ideal gas law requires temperatures to be in Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 34.01C + 273.15 = 307.16K
And, T2 = 30.18C + 273.15 = 303.33K

Now we can plug these values into our formula:

25.22L / 307.16K = V2 / 303.33K

To solve for V2, we multiply both sides by 303.33K:

V2 = 25.22L * 303.33K / 307.16K

V2 = 24.92L

So, if the temperature is changed to 30.18C and the pressure remains constant, the volume of the balloon will be approximately 24.92 liters.

Knowee AI · Accepted Answer

To solve this problem, we can use the ideal gas law, which states that the volume of a gas is directly proportional to its temperature and inversely proportional to its pressure. However, since the pressure remains constant in this problem, we can simplify this to a direct relationship between volume and temperature.

The formula we will use is V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.

First, we need to convert the temperatures from Celsius to Kelvin, because the ideal gas law requires temperatures to be in Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 34.01C + 273.15 = 307.16K
And, T2 = 30.18C + 273.15 = 303.33K

Now we can plug these values into our formula:

25.22L / 307.16K = V2 / 303.33K

To solve for V2, we multiply both sides by 303.33K:

V2 = 25.22L * 303.33K / 307.16K

V2 = 24.92L

So, if the temperature is changed to 30.18C and the pressure remains constant, the volume of the balloon will be approximately 24.92 liters.

A balloon filled with helium has a volume of 25.22 L at a pressure of 21.61 kPa and a temperature of 34.01C. What will the volume of the balloon be, in L, if the temperature is changed to 30.18C and the pressure remains constant?

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