Final answer:
There are approximately 26.59 grams of krypton gas in the balloon.
Step-by-step explanation:
The combined gas law relates the pressure, volume, and temperature of a gas. It can be written as:
P₁V₁/T₁ = P₂V₂/T₂
In this question, we are given:
- Volume (V₁) = 2 L
- Pressure (P₁) = 3.25 atm
- Temperature (T₁) = 250 K
To find the number of grams of krypton gas, we first need to calculate the number of moles using the ideal gas law:
n = PV/RT
where n is the number of moles, P is the pressure, V is the volume, R is the ideal gas constant, and T is the temperature. The ideal gas constant is 0.0821 L·atm/(mol·K).
Once we have the number of moles, we can convert it to grams using the molar mass of krypton, which is 83.8 g/mol.
Let's calculate:
- Calculate the number of moles:
- n = (3.25 atm * 2 L) / (0.0821 L·atm/(mol·K) * 250 K)
- Convert moles to grams:
- grams = moles * molar mass
Substituting the values in the formulas, we get:
- n = (6.5) / (20.525) = 0.317 moles
- grams = 0.317 moles * 83.8 g/mol = 26.59 grams
Therefore, there are approximately 26.59 grams of krypton gas in the balloon.