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 in Kelvin, assuming pressure and the amount of gas are constant. This can be expressed as V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

First, we need to convert the temperatures from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 25°C + 273.15 = 298.15 K
And, T2 = 10°C + 273.15 = 283.15 K

We know that V1 = 1.88 L. We need to find V2.

Substituting the known values into the equation, we get:

1.88 L / 298.15 K = V2 / 283.15 K

Solving for V2, we get:

V2 = (1.88 L / 298.15 K) * 283.15 K = 1.78 L

So, the volume of the balloon at 10°C would be approximately 1.78 L. Therefore, the closest answer is 1.79 L.

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 in Kelvin, assuming pressure and the amount of gas are constant. This can be expressed as V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

First, we need to convert the temperatures from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 25°C + 273.15 = 298.15 K
And, T2 = 10°C + 273.15 = 283.15 K

We know that V1 = 1.88 L. We need to find V2.

Substituting the known values into the equation, we get:

1.88 L / 298.15 K = V2 / 283.15 K

Solving for V2, we get:

V2 = (1.88 L / 298.15 K) * 283.15 K = 1.78 L

So, the volume of the balloon at 10°C would be approximately 1.78 L. Therefore, the closest answer is 1.79 L.

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 in Kelvin, assuming pressure and the amount of gas are constant. This can be expressed as V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

First, we need to convert the temperatures from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15.

So, T1 = 25°C + 273.15 = 298.15 K
And, T2 = 10°C + 273.15 = 283.15 K

We know that V1 = 1.88 L. We need to find V2.

Substituting the known values into the equation, we get:

1.88 L / 298.15 K = V2 / 283.15 K

Solving for V2, we get:

V2 = (1.88 L / 298.15 K) * 283.15 K = 1.78 L

So, the volume of the balloon at 10°C would be approximately 1.78 L. Therefore, the closest answer is 1.79 L.

A balloon filled with nitrogen gas at 25 oC and 1 atm has a volume of 1.88 litres. What is the volume of the same balloon if the temperatures drops to 10 oC (assume no loss of nitrogen molecules through the walls of the balloon)Question 16Answer0.752 L1.98 L1.79 L4.70 L0.215 L

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