1. Convert Units

* Volume: 202 mL = 0.202 L (1 L = 1000 mL)

* Temperature: 35°C = 308 K (K = °C + 273.15)

* Pressure: 750 mmHg = 0.987 atm (1 atm = 760 mmHg)

2. Use the Ideal Gas Law

The ideal gas law is: PV = nRT

* P: Pressure (in atm)

* V: Volume (in L)

* n: Number of moles

* R: Ideal gas constant (0.0821 L·atm/mol·K)

* T: Temperature (in K)

3. Solve for n (moles)

Rearrange the ideal gas law to solve for n:

n = PV / RT

4. Plug in the Values

n = (0.987 atm)(0.202 L) / (0.0821 L·atm/mol·K)(308 K)

5. Calculate

n ≈ 0.0078 moles

Therefore, there are approximately 0.0078 moles of ammonia gas in the container.