How many moles of ammonia gas are found in a 202mL container at 35 degreas and 750mmHg?

To find the number of moles of ammonia gas, we can use the ideal gas law, which is (PV = nRT). First, we convert the volume from mL to liters (202 mL = 0.202 L) and the pressure from mmHg to atmospheres (750 mmHg = 750/760 atm ≈ 0.9868 atm). Using the ideal gas constant (R = 0.0821 , \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}) and converting the temperature to Kelvin (35°C = 308 K), we can rearrange the formula to solve for (n):

[ n = \frac{PV}{RT} = \frac{(0.9868 , \text{atm})(0.202 , \text{L})}{(0.0821 , \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K})(308 , \text{K})} \approx 0.0077 , \text{moles}. ]

Thus, there are approximately 0.0077 moles of ammonia gas in the container.