250ml test tube has 9.89 g of N2, 7.26 g of N2O, and 8.74 g of O2 at a temperature of 24.2∘C. Find the partial pressure of N2O in the 250ml test tube?

a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?   b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.

A 4.10 g sample of an unknown compound containing only C , H , and O combusts in an oxygen‑rich environment. When the products have cooled to 20.0 °C at 1 bar, there are 4.54 L of CO2 and 3.36 mL of H2O. The density of water at 20.0 °C is 0.998 g/mL. What is the empirical formula of the unknown compound? If the molar mass is 132.2 g/mol132.2 g/mol , what is the molecular formula of the compound?

If 42.5 g of O2 and 2.8 g of CO2 are placed in a 11.2 L container at 24 °C , what is the pressure of the mixture of gases? ΑΣφ ? atm