How many liters of CO2 gas can you produce at STP from 30.0 liters O2 at STP?

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Three 4−L flasks, fixed with pressure gauges and small valves, each contain 9 g of gas at 281 K. Flask A contains He, flask B contains H2, and flask C contains CH4. Rank the flask contents in terms of:   Multiple Choice: (a) pressure.      A > B > C    A > C > B    B > C > A    B > A > C    C > B > A    C > A > B    A = B = C (b) average molecular kinetic energy.      A > B > C    A > C > B    B > C > A    B > A > C    C > B > A    C > A > B    A = B = C (c) diffusion rate after valve is opened.      A > B > C    A > C > B    B > C > A    B > A > C    C > B > A    C > A > B    A = B = C (d) total kinetic energy of the molecules.      A > B > C    A > C > B    B > C > A    B > A > C    C > B…

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How many liters of NH3 (gas) at STP can be produced by the reaction of 7.5 g of H2O according to the equation shown below? Mg3N2 + 6H2O   --->  3 Mg(OH)2 + 2NH3

Be sure to answer all parts. Three 9−L flasks, fixed with pressure gauges and small valves, each contain 8 g of gas at 275 K. Flask A contains CH4, flask B contains H2, and flask C contains He. Rank the flask contents in terms of: (a) pressure. A > B > C   A > C > B   B > C > A   B > A > C C > B > A C > A > B A = B = C b) average molecular kinetic energy. A > B > C A > C > C B > C > A   B > A > C C > B > A C > A > B A = B = C c) diffusion rate after valve is opened. A > B > C A > C > C B > C > A   B > A > C C > B > A C > A > B A = B = C  d) total kinetic energy of the molecules. A > B > C A > C > C B > C > A   B > A > C C > B > A C > A > B A = B = C e) density. A > B > C A > C > C B > C > A   B > A > C C > B > A C > A > B A = B = C f) collision frequency. A > B > C A…

When 25.0 g of potassium chlorate (KCIO3) decomposes, how many L of O2 gas are formed at STP? Refer to the chemical equation below. 2 KCIO3(s) - 2 KCl(s) + 3 O2(g) 012.4 L 02 024.8 L 02 06.85 L 02

113 STARTING AMOUNT X Calculate the amount of liters of CO2 gas produced when 113 grams of NaHCO reacts completely according to the following balanced equation at STP. Remember 1 mol of an ideal gas has a volume of 22.7 L at STP. NaHCO3(s) + C2H4O2(aq) → NaC2H3O2(aq) + H2O(l) + CO2(g)

Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide. 2NaN3(s) →2Na(s) + 3N2(g) How many moles of sodium azide are needed to produce sufficient nitrogen to fill a 50.0 L air bag to a pressure of 1.25 atm at 25°C? Select one: a. 5.31 mol b. 1.70 mol c. 4.92 mol d. 2.56 mol e. 3.83 mol

15. A fuel-air mixture contains 0.5 mol CH4(g), 1.5 mol 02(g), and 6.0 mol N2(g), under a total pressure Ptot = 25 atm. Find the partial pressure of 02(g) in it: A) 25 atm B) 0.063 atm C) 1.6 atm D) 19 atm E) 4.7 atm