Ammonia, NH3, reacts with oxygen to form nitrogen gas and water. 4 NH3(aq) + 30₂(g) → 2N₂(g) + 6H₂O(1) If 4.05 g of NH3 reacts with 6.08 g of O₂ and produces 0.950 L of N₂ at 295 K and 1.00 atm, which reactant is limiting? NH3 (aq) 0₂ (g) What is the percent yield of the reaction?

How many grams of Magnesium Oxide form when 14.8L of oxygen gas, measured in STP, completely reacts with Magnesium metal in accordance with the following reaction : 2MgO (s) + O2 (g) = 2MgO (s)

an aerosol can has a volume of 450 mL and contains 2.18g of propane (C3H8) as a propellant. if the van is 23°c, what is the pressure in the can?

A gas mixture contains 14.8 mol of Br2 and 66.5 mol of F2.(a) Compute the mole fraction of Br2 in the mixture.XBr2 = (b) The mixture is then heated, and the Br2 starts to react with the F2 to give BrF5: Br2(g) + 5F2(g) -> 2BrF5(g) At a certain point in the reaction, 7.70 mol of BrF5 is present. Determine the mole fraction of Br2 in the new mixture. XBr2 =

Automobile airbags are inflated by the rapid decomposition of sodium azide (NaN3). 2 NaN3(s) --> 2 Na(s) + 3 N2(g) What volume of N2 gas, at 0.973 atm and 21.3 oC, is produced by the complete decomposition of 119 g of sodium azide? V = ___ L

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnClą(aq) +H2(g) The product gas, H,, is collected over water at a temperature of 20 °C and a pressure of 755 mm Hg. If the wet H, gas formed occupies a volume of 6.66 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.

T8 When 1.836 L of 6.000 M hydrochloric acid react with excess iron how many liters of hydrogen gas form at 25.0°C and 1.00 atm? This and the next 2 questions use the reaction: 2 Fe (s) + 6 HCI (aq) → 2 FeCl3 (aq) + 3 H2 (g) Select one: a. 0.5637 mol b. 0.03132 mol C. none of these d. 0.09395 mol e. 16.4 L f.5.508 mol g. 0.1879 mol h. 135 L

Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4 NH₂(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.95 g NH3 reacts with 5.93 g O₂ and produces 0.850 L. N₂ at 295 K and 1.00 bar, how many moles of N₂ can be produced by each reactant? It may be useful to consult the periodic table. NH₂: 0₂: Based on the theoretical yields, which reactant is limiting? NH,(aq) 0₂(g) What is the percent yield of the reaction? percent yield: mol N₂ mol N₂ 28

Consider the reaction shown below: 2 HCl (aq) + CaCO3 (s) ⟶ CO2 (g) +  CaCl2 (aq) + H2O (l) How many grams of CaCO3 would need to be consumed to fill a 908.001 mL balloon with CO2 gas, assuming a constant temperature of 21.7 oC and constant pressure of 0.958 atm? Express your answer in units of grams using at least three significant figures.