This problem can be solved using the ideal gas law, which states that the pressure and temperature of a gas are directly proportional when the volume and amount of gas are held constant. This relationship can be expressed as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Step 1: Convert the temperatures from Celsius to Kelvin. The Kelvin scale is used in gas law problems because it is an absolute scale, starting at zero, which corresponds to absolute zero.

T1 = 27.4C + 273 = 300.4 K

Step 2: Convert the pressures from torr to atmospheres, as the ideal gas law is usually expressed in these units. 1 atm = 760 torr.

P1 = 960 torr * (1 atm / 760 torr) = 1.263 atm
P2 = 1610 torr * (1 atm / 760 torr) = 2.118 atm

Step 3: Substitute the known values into the ideal gas law equation and solve for T2.

P1/T1 = P2/T2
1.263 atm / 300.4 K = 2.118 atm / T2
Solving for T2 gives T2 = (2.118 atm * 300.4 K) / 1.263 atm = 502.6 K

Step 4: Convert the temperature back to Celsius if desired.

T2 = 502.6 K - 273 = 229.6 C

So, the temperature inside the balloon at the higher altitude would be approximately 229.6 degrees Celsius.

Question

This problem can be solved using the ideal gas law, which states that the pressure and temperature of a gas are directly proportional when the volume and amount of gas are held constant. This relationship can be expressed as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Step 1: Convert the temperatures from Celsius to Kelvin. The Kelvin scale is used in gas law problems because it is an absolute scale, starting at zero, which corresponds to absolute zero.

T1 = 27.4C + 273 = 300.4 K

Step 2: Convert the pressures from torr to atmospheres, as the ideal gas law is usually expressed in these units. 1 atm = 760 torr.

P1 = 960 torr * (1 atm / 760 torr) = 1.263 atm
P2 = 1610 torr * (1 atm / 760 torr) = 2.118 atm

Step 3: Substitute the known values into the ideal gas law equation and solve for T2.

P1/T1 = P2/T2
1.263 atm / 300.4 K = 2.118 atm / T2
Solving for T2 gives T2 = (2.118 atm * 300.4 K) / 1.263 atm = 502.6 K

Step 4: Convert the temperature back to Celsius if desired.

T2 = 502.6 K - 273 = 229.6 C

So, the temperature inside the balloon at the higher altitude would be approximately 229.6 degrees Celsius.

Knowee AI · Accepted Answer

This problem can be solved using the ideal gas law, which states that the pressure and temperature of a gas are directly proportional when the volume and amount of gas are held constant. This relationship can be expressed as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Step 1: Convert the temperatures from Celsius to Kelvin. The Kelvin scale is used in gas law problems because it is an absolute scale, starting at zero, which corresponds to absolute zero.

T1 = 27.4C + 273 = 300.4 K

Step 2: Convert the pressures from torr to atmospheres, as the ideal gas law is usually expressed in these units. 1 atm = 760 torr.

P1 = 960 torr * (1 atm / 760 torr) = 1.263 atm
P2 = 1610 torr * (1 atm / 760 torr) = 2.118 atm

Step 3: Substitute the known values into the ideal gas law equation and solve for T2.

P1/T1 = P2/T2
1.263 atm / 300.4 K = 2.118 atm / T2
Solving for T2 gives T2 = (2.118 atm * 300.4 K) / 1.263 atm = 502.6 K

Step 4: Convert the temperature back to Celsius if desired.

T2 = 502.6 K - 273 = 229.6 C

So, the temperature inside the balloon at the higher altitude would be approximately 229.6 degrees Celsius.

Given: Kelvin = C + 273A weather balloon is launched at 960 torr pressure with an internal temperature of 27.4C. When the balloon reaches the altitude in which the pressure is reduced to 1610 torr, what temperature will the inside of the balloon possess?

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