Given a gas sample with a Temperature of 298 K, a Pressure of 1.2 atm, and a molar quantity of 0.12 moles. Solve for Volume (in L) PV = nRT P in atm, V in Liters, n in moles, T in Kelvin R = 0.08206 (L*atm)/(mol*K)

Determination of the Universal Gas Constant Postlab 1. An evaluation of Rwas performed using the procedures outlined in this exercise, The barometric pressure was 735 torr and the temperature was 21.5 "C. The volume of H2(9) collected was 32.7 mL. The calculated value of Rwas 0.0817 L'atm/mol-K. a. How many grams of Mg metal were used in this determination? 0.0316 70.361 b. If the correction for the vapor pressure of water had not been performed, what would be the calculated value of R? Incorrect c. If the syringe volume had been incorrectly read, resulting in a calculated H, volume of 30.6 mL, what would be the percent error in the calculated value of Rwith respect to the originally calculated value (0.0817 L-atm/mol·K)? 6.4 %

6-25. A mixture of gases contains 66.0 g CO2, 2.02 g of H₂, and 16.0 g of O₂. If the total pressure of the mixture is 725 torr, what is the partial pressure of each gas? 6-26. Air, by weight, is essentially a mixture of 79% N₂ and 21% O₂. Calculate the partial pressure of each gas at a total pressure of 99 kPakPa.

What is the pressure (in bar) in a 4.00 L tank with 24.0 grams of oxygen gas at 350.0 K? R = 0.08314 L･bar/mol･K.

100% EXP 3- Determination of universal gas constant Thermal decomposition reaction of KCIO3 can be used to determine the universal gas constant. 2KCIO:(s) 2KCI(s) + 302(g) MnO2 (catalyst) Firstly, KCIO3 and MnO2 (catalyst) is placed in a clean and dry test tube, and it is weighed as 15.92 g. While heating the test tube, thermal decomposition reaction occurs and all the evolved O2(g) is collected in a flask filled with water at 759 mmHg and 20°C. Because of evolved O2(g), 250 mL water is transferred from the flask to a beaker. Additionally, the weight of test tube after heating is determined as 15.60 g. (Note: The partial pressure of water at 20°C is 17.5 mmHg.) (a) Calculate experimental value of the universal gas constant by using the information given above. (b) Compare the theoretical and the experimental values of gas constant and calculate the percentage error in the experiment. (KČIO:: 122.55 g/mol. Oz: 32.00 g/mol, R: 0.082 L atm/mol K) EXP 4- Diffusion

Sketch three isochores for the same gas at three different volumes V1, V2 and V3 where V1 = V3 and V2<V3. How the temperature scale (K vs oC) will change on your plot?

5. There are 1.07 X 103 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)

If you have two jars containing the same amount, n1=n2, and type of gas (for example, oxygen) and they are at the same temperature, T, what can you say about their pressure if the first jar has four times the volume of the second, V1 = 4V2?  Hint: use pV=nRT   Group of answer choices P1 = (1/4)P2 P1 = (1/3)P2 P1 = P2 P1 = 4P2 P1 = 3P2   I believe it is P1 = 4P2 but unsure...

Ammonia, NH3, can react with oxygen to form nitrogen gas and water. 4 NH3(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.85 g NH3 reacts with 5.78 g O₂ and produces 0.950 L N₂, at 295 K and 1.01 bar, which reactant is limiting? NH,(aq) 0₂(g) Calculate the percent yield of the reaction. percent yield:

The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules