We can use the ideal gas law to calculate the number of moles of ammonia gas in the container. The ideal gas law is:

$$PV = nRT$$

where:

P is the pressure of the gas in atm

V is the volume of the gas in L

n is the number of moles of gas

R is the ideal gas constant (0.08206 L atm / mol K)

T is the temperature of the gas in K

We need to convert the given values to the correct units:

- Convert the volume from mL to L:

$$202 \text{ mL} = 202 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.202 \text{ L}$$

- Convert the temperature from °C to K:

$$35\degree\text{C} = (35\degree\text{C} + 273.15) \text{ K} = 308.15\text{ K}$$

Now we can plug in the values into the ideal gas law:

$$(750 \text{ mmHg}) (0.202 \text{ L}) = n (0.08206 \text{ L atm / mol K}) (308.15 \text{ K})$$

Solving for n, we get:

$$n = \frac{(750 \text{ mmHg})(0.202 \text{ L})}{(0.08206 \text{ L atm / mol K})(308.15 \text{ K})}$$

$$n = 0.0064 \text{ mol}$$

Therefore, there are 0.0064 moles of ammonia gas in the 202 mL container at 35°C and 750 mmHg.