A compressed air tank contains 4.7 kg of air at a temperature of 81 °C. A gage on the tank reads 300 kPa. Determine the volume of the tank. volume = i m³ 3
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- perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.Ideal Gas Law The pressure P, temperature T, and volume V ofan ideal gas are related by PV = nRT, where n is the number ofmoles of the gas and R is the universal gas constant. For the pur-poses of this exercise, let nR = 1; therefore, P = T/V.a. Suppose that the volume is held constant and the temperatureincreases by ∆T = 0.05. What is the approximate change inthe pressure? Does the pressure increase or decrease?b. Suppose that the temperature is held constant and the volumeincreases by ∆V = 0.1. What is the approximate change in thepressure? Does the pressure increase or decrease?c. Suppose that the pressure is held constant and the volume in-creases by ∆V = 0.1. What is the approximate change in thetemperature? Does the temperature increase or decrease?For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of – 33. °C. Suppose the temperature of a sample of ammonia gas is raised from – 19.0 °C to 21.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.29 kPa and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. | kPa APR 24 W 80 888 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 23 2$ &
- A sample of propane (C3H8) is placed in a closed vessel together with an amount of O₂ that is 2.00 times the amount needed to completely oxidize the propane to CO2 and H₂O at constant temperature. Part A Calculate the mole fraction of each component in the resulting mixture after oxidation, assuming that the H₂O is present as a gas. Enter your answers numerically separated by commas. Use 3 significant figures.Stoichiometry with Partial Pressure Gas jar Gas collects here Trough of water Bee hive shelf Reaction mixture 2 KCIO, 3(s) + > 2 KCI (s), 30 2(g) A sample of KCIO3 is partially decomposed by heating, producing O2 gas that is collected safely over water. The volume of total gas collected is 2.50 x 10-4 m³ at 26 °C, giving 101.99 kPa total pressure. How many grams of KCIO3 were decomposed? What atom was oxidized? What atom was reduced? The pressure of water vapor at 26 °C is 25 torr. SHOW ALL WORK!A sample of unknown gas was heated to 125°C in a round bottom flask at standard pressure (1.00 atm), and its weight in a 100 ml round bottom flask was taken to be 30.098g. The round bottom flask weighs 30.0g. The gas was determined to be pure so that it can only be composed of a single element (N2, O2, F2, He, Ne, Ar, P2, S2, Cl2). Identify the gas.
- The pressure P of a sample of oxygen gas that is compressed at a constant temperature is related to the volume V of gas by a reciprocal function of the form P = k V . (a) A sample of oxygen gas that occupies 0.674 m3 exerts a pressure of 39 kPa at a temperature of 293 K (absolute temperature measured on the Kelvin scale). Find the value of k (in kPa · m3) in the given model.You want to cool a storage cylinder containing 10 moles of compressed gas from 30°C to 20°C. For which kind of gas would this be easiest? (i) A monatomic gas; (ii) a diatomic gas; (iii) a polyatomic gas; (iv) it would be equally easy for all of these.Ethanol vapours were allowed to completely fill a large jug with a volume of 15.5L. The ethanol was burned yielding 5.5mL of pure liquid water in the bottom of the jug at the end of the reaction. C2H5OH + 3 O2 ? 2 CO2 + 3 H20 If the room temperature was 21.5 oC and the pressure was 0.996atm, calculate the percentage yield of the water gathered in the jug.
- Two flasks of equal volume are connected by a narrow tube (of negligible volume). Initially, both flasks are at 27°C and contain 0.70 moles of hydrogen gas, the pressure being 50,000 Pa. One of the flasks is then immersed in a hot oil bath at 127°C, while the other is kept at 27°C. Calculate the final pressure of the system, in Pa. Calculate the final number of moles of hydrogen gas in the flask that was immersed in the oil bath. R = 0.08205 L atm mol-¹ K-₁ T(K) = T (°C) + 273.15Report all your results by using significant figures and use dimensional analysis. A flammable gas contains only C, H, N, and Cl. The complete combustion of a 100.0 mg sample of this gas in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H20 vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (a) Determine the percentage of the composition of the substance. (b) Calculate its empirical formula. (c) If the rms speed of this gas at 25°C is 131.325 m/s, calculate its molecular formula.Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.130 kPa. key carbon hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure ☐ x10 N2 ||] ☐ kPa ☑ 02 ☐ ☐ kPa
