}We mix 0.25 g of oxygen gas (O2) and 1.5 g nitrogen gas (N2) in a 2 L container at 20oC. Assuming both gases behave ideally,
(a)what is the partial pressure of oxygen?
(b)what is the partial pressure of nitrogen?
(c)what is the total pressure in the container?
Molar masses are 32 g/mol for oxygen and 28 g/mol for nitrogen.
}We mix 0.25 g of oxygen gas (O2) and 1.5 g nitrogen gas (N2) in a...
A gas mixture contains 0.150 mol of oxygen (O2) gas, 0.116mo lof nitrogen (N2) gas. and 0.211 mol of argon (Ar) gas in a 0.500L flask at 298K. What is the partial pressure of N2 the mixture?
Nitrogen dioxide gas undergoes decomposition producing nitrogen monoxide and oxygen gases: 2 NO2(g)........ 2 NO(g) + O2(g) A sample consisting of 0.10 moles of NO2 is placed in a 10.0 L in a container that is then heated to 750 K. When equilibrium is reached, the pressure in the container is 0.827 bar. Calculate the equilibrium constant and the degree of dissociation at this temperature. (Hint: pressures are directly proportional to concentration, so they can be used in ICE tables).
The air that we breathe is composed of 78% nitrogen (N2), 21% oxygen (O2), and the other 1% includes water vapor, carbon dioxide, and pollutants. If a tire is inflated to a pressure of 33 pounds per square inch (psi) with regular air, what is the partial pressure of nitrogen and of oxygen within the tire?
A rigid container holds both oxygen gas (O2) and nitrogen gas (N2) at 100°C. The atomic mass numbers for nitrogen and oxygen atoms are 14 and 16 respectively. Which statement describes their rms speeds? A. Vrms of O2 < Vrms of N2 B. Vrms of O2 = Vrms of N2 C. Vrms of O2 > Vrms of N2 D. All of the above. E. None of the above.
7. Gas Law Problem Nitric oxide (NO) reacts with molecular oxygen 2NO(g) + O2(g) → 2NO2(g). Initially, equal volumes of the reactant gases are separated in a 2.0 L container. The pressure of the NO is 1.25 atm, while the pressure of the O2 is 0.85 atm. What are the partial pressures of the gases once the reaction has gone to completion. Assume the temperature remains constant at 0°C.
Nitric oxide (NO) gas partially decomposes into nitrogen (N2) and oxygen (O2) gases after being placed in a closed container. 2NO (8) = N2 (8) + O2 (8) What is true about the reaction? O The rate of the forward reaction is at its maximum when pure NO gas is first placed in the container. O At equilibrium, the concentration of O2 gas is the same as the concentration of NO gas. O All of the NO gas is eventually...
Hydrazine, N2H4 , reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 4.05 g of N2H4 reacts with excess oxygen and produces 0.750 L of N2 , at 295 K and 1.00 atm, what is the percent yield of the reaction?
Hydrazine, N2H4N2H4, reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 2.55 g2.55 g of N2H4N2H4 reacts with excess oxygen and produces 0.550 L0.550 L of N2N2, at 295 K295 K and 1.00 atm,1.00 atm, what is the percent yield of the reaction?
Hydrazine, N2H4N2H4, reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 2.05 g2.05 g of N2H4N2H4 reacts with excess oxygen and produces 0.650 L0.650 L of N2N2, at 295 K295 K and 1.00 atm,1.00 atm, what is the percent yield of the reaction?
We have a container enclosing a mixture of N2(g) and O2(g). The total pressure is 3.97 atm. The temperature is 25.00 oC and the volume of the container is 17.8 L. If the mass of N2 in the container is 33.4 g, what is the partial pressure of O2 (in atm) within the container?