Here's how to calculate the pressure of the gas in the balloon:

1. Convert Units

* Temperature (Celsius to Kelvin): T(K) = T(°C) + 273.15

So, 35°C = 35 + 273.15 = 308.15 K

* Volume (Liters to Cubic Meters): 1 L = 0.001 m³

So, 0.34 L = 0.34 * 0.001 m³ = 0.00034 m³

2. Use the Ideal Gas Law

The ideal gas law is: PV = nRT

where:

* P = pressure (Pa)

* V = volume (m³)

* n = number of moles

* R = ideal gas constant (8.314 J/mol·K)

* T = temperature (K)

3. Solve for Pressure

Rearrange the ideal gas law to solve for pressure:

P = (nRT) / V

4. Substitute Values

P = (0.0233 mol * 8.314 J/mol·K * 308.15 K) / 0.00034 m³

5. Calculate

P ≈ 1.76 x 10⁵ Pa

Therefore, the pressure in the balloon is approximately 1.76 x 10⁵ Pascals.