3. A 10.0 L cylinder contains 7.60 g of Ar(g) and 4.40 g of N2(g) at 25°C. Calculate the partial pressure of each gas and the total pressure in the cylinder. Use the equation PV = nRT for calculating the pressure of each gas R= 0.08206 L atm mol-l K-

A gas mixture in a 1.65-L container at 294 K contains 10.0 gg of Ne and 10.0 g of Ar. Calculate the partial pressure (in atm) of Ne and Ar in the container. A. PNe=5.45atm, PAr=5.45atm B. PNe=7.25atm, PAr=3.66atm C. PNe=5.40atm, PAr=2.73atm D. PNe=9.73atm, PAr=4.90atm

The oxidation of trichloroethane results in the following reaction equation: 4 C2H3CI3 (l) + 11 O2 (g) ---> 8 CO2 (g) + 6 H2O (l) + 6 CI2 (g) The reaction of 60.6 g of C2H3Cl3(l) with excess oxygen in a laboratory experiment resulted in the collection of 10.4 L of chlorine gas at SATP. Calculate the percent yield for this reaction.

A sample of gas contains 0.1100 mol of CH4(g) and 0.1100 mol of H2O(g) and occupies a volume of 7.46 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. L

A mixture of gases contains 1.60 g of N₂, 8.91 g of H₂, and 1.66 g of NH3. If the total pressure of the mixture is 5.93 atm, what is the partial pressure of each component? P-00729 Py <-5.728 P-0295 ✔atm ✔atm Xatm

A sample of an ideal gas contains 0.697 moles. If the volume of the gas is 79.7 L and the temperature is 46.9 °C, what is the pressure of the gas? O 25.6 mmHg O 33.7 mmHg O 26.4 mmHg O 175. mmHg O 230. mmHg

Consider 4.40 LL of a gas at 365 mmHgmmHg and 20. ∘C∘C . If the container is compressed to 2.40 LL and the temperature is increased to 33 ∘C∘C , what is the new pressure, P2P2P_2, inside the container? Assume no change in the amount of gas inside the cylinder.

Use the necessary constant in solving this problem. See the second image.

Calculate the volume occupied by 2.2 moles of methane gas (CH4) at 25°C and 1.0 atm. R = 0.08206 Lxatm/Kxmol. O 11.2 L 4.5 L 53.8 L 0.0186 L 49.2 L

4. Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CHA(g) + H2O(g) → CO(g) + 3 H2(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25°C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125°C). The reaction produces 26.2 L of hydrogen gas at STP. A. Determine the theoretical yield (Volume, L) of hydrogen gas (hint- calculate moles of each reactant and remember to use the limiting reactant to determine theoretical yield). B. Calculate the percent yield of the reaction. Table 1. Vapor Pressure of Water at Various Temperatures Temperature (°C) Vapor Pressure (torr) 24.0 22.4 24.1 22.5 24.2 22.6 24.3 22.8 24.4 22.9 24.5 23.1 24 6 23.2