you have 25 L cylinder of helium at a pressure of 135 atm and a temperature of 23 degrees celcius. the He is used to fill balloons toa volume of 1 L at .982 atm and 27 degrees celcius. how many balloons can be silled with He?

To solve this problem, we can use the ideal gas law equation: PV = nRT.

First, let's convert the given temperatures to Kelvin. Since temperature in Kelvin is equal to degrees Celsius plus 273.15, we have:
T1 = 23°C + 273.15 = 296.15 K (initial temperature)
T2 = 27°C + 273.15 = 300.15 K (final temperature)

Now, we need to find the number of moles of helium in the cylinder before any balloons are filled. We can rearrange the ideal gas law equation to solve for n:
n = PV / RT

Using the given values for pressure, volume, and temperature, we have:
n1 = (135 atm) * (25 L) / [(0.0821 L*atm/(mol*K)) * (296.15 K)]

Next, let's determine the number of moles of helium used to fill one balloon. We can use the same ideal gas law equation, using the final pressure and volume of one balloon:
n2 = (0.982 atm) * (1 L) / [(0.0821 L*atm/(mol*K)) * (300.15 K)]

Finally, we can calculate the number of balloons that can be filled with the given cylinder of helium by dividing the initial moles by the moles used to fill one balloon:
Number of balloons = n1 / n2

You can substitute the given values into the above equations to get the final answer.