Use the combined gas law to solve the following problem: Calculate the volume of helium gas that results when 0.550 L of the gas is heated from 22.0 degrees C at 1.00 atm to 30.0 degrees C at 1.50 atm .

(P1V1)/T1 = (P2V2)/T2

To solve this problem using the combined gas law, we need to use the following equation:

(P₁ * V₁) / (T₁) = (P₂ * V₂) / (T₂)

Where:
P₁ and P₂ are the initial and final pressures
V₁ and V₂ are the initial and final volumes
T₁ and T₂ are the initial and final temperatures

Now, let's plug in the given values:
P₁ = 1.00 atm
V₁ = 0.550 L
T₁ = 22.0 °C (Convert this to Kelvin by adding 273.15: 22.0 + 273.15 = 295.15 K)

P₂ = 1.50 atm
V₂ = ?
T₂ = 30.0 °C (Convert this to Kelvin: 30.0 + 273.15 = 303.15 K)

The equation now becomes:

(1.00 atm * 0.550 L) / (295.15 K) = (1.50 atm * V₂) / (303.15 K)

To solve for V₂, we can rearrange the equation as follows:

V₂ = [(1.00 atm * 0.550 L * 303.15 K) / (295.15 K)] / (1.50 atm)

Now, calculate V₂:

V₂ = [(1.00 * 0.550 * 303.15) / 295.15] / 1.50
V₂ ≈ 0.582 L

Therefore, the volume of helium gas at the final condition is approximately 0.582 L.