Aballoon filled with helium has a volume of 30.0 l at a pressure of 100 kpa and a temperature of 25.0 degrees c. what will the volume of the balloon be if the temperature is increased to 80.0 degress c and the pressure remains constant?

The final volume of the balloon has been 35 L.

The gas in the balloon has been assumed to be an ideal gas. The relationship between volume and temperature at constant pressure has been given by:

The initial volume of balloon has been,

The initial temperature of the balloon has been,

The final temperature of the balloon has been,

The final volume of the balloon, has been given by substituting the values as:

The final volume of the balloon has been 35 L.

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Answer : The volume of the balloon will be 35.5 L at 80°C

Explanation :

The pressure is kept constant. Therefore any change in temperature would affect the volume. This can be explained with the help of Charles Law

According to this law, at constant pressure, the volume of an ideal gas varies directly with its absolute temperature ( K)

In equation form, the law can be stated as

We have been given

V₁ = 30.0 L

We need temperature in kelvin unit .

T₁ = 25 °C = 25 + 273 = 298 K

V₂ = ?

T₂ = 80 + 273 = 353 K

Let us plug in these values in Charles law equation.

On cross multiplication, we get

The volume of the balloon will be 35.5 L

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of carbon is as shown here in the image.

c. 75.7

i think that is the right