05:11STP Gas Chemistry (Standard Temperature and Pressure) Examples Practice Problems Questions ShortcutConquer Chemistry618
Multiple ChoiceA sample of dichloromethane gas (CH2Cl2) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?3691Has a video solution.
Multiple ChoiceNitrogen and hydrogen combine to form ammonia via the following reaction: 1 N2 (s) + 3 H2 (g) → 2 NH3 (g)What mass of nitrogen is required to completely react with 800.0 mL H2 at STP?130572Has a video solution.
Multiple ChoiceWhat is the pressure inside a 1.5-L container that is charged with 3.0 moles of a gas at 35.0℃?133
Multiple ChoiceThe combustion of glucose yields carbon dioxide and water according to the following reaction: C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) Calculate the mass of H2O produced when 12.0 g of glucose is combusted in a container of oxygen with a volume of 1.3 L at a pressure of 2.2 atm and a temperature of 205℃.1507
Textbook QuestionPropane gas 1C3H82 is often used as fuel in rural areas. How many liters of CO2 are formed at STP by the complete combustion of the propane in a container with a volume of 15.0 L and a pressure of 4.50 atm at 25.0 °C? The equation for the combustion of propane is: C3H81g2 + 5 O21g2¡3 CO21g2 + 4 H2O1l2 (LO 10.4, 10.5) (a) 61.8 L (b) 186 L (c) 20.6 L (d) 2.21 * 103 L301Has a video solution.
Textbook QuestionAt standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (b) On cooling to 160 K, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to 160 K?356Has a video solution.
Textbook QuestionAt standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl2 and NH3 at 160 K are 2.02 and 0.84 g/cm3, respectively. Calculate their molar volumes.1503Has a video solution.
Textbook QuestionChlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (b) What volume will the Cl2 occupy at STP?655Has a video solution.
Textbook QuestionMany gases are shipped in high-pressure containers. Consider a steel tank whose volume is 210.0 L that contains O2 gas at a pressure of 16,500 kPa at 23 °C. (b) What volume would the gas occupy at STP?269Has a video solution.
Textbook QuestionThe surface temperature of Venus is about 1050 K, and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venusian 'STP,' what is the standard molar volume in liters of a gas on Venus?523Has a video solution.
Textbook QuestionWhich sample contains more molecules: 1.00 L of O2 at STP, 1.00 L of air at STP, or 1.00 L of H2 at STP?589Has a video solution.
Textbook QuestionA compressed air tank carried by scuba divers has a volume of 8.0 L and a pressure of 140 atm at 20 °C. What is the volume of air in the tank in liters at STP?1031Has a video solution.
Textbook QuestionUse the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.1111Has a video solution.
Textbook QuestionUse the molar volume of a gas at STP to calculate the density (in g>L) of nitrogen gas at STP.2172Has a video solution.
Textbook QuestionImagine that you have two identical flasks, one containing hydrogen at STP and the other containing oxygen at STP. How can you tell which is which without opening them?210Has a video solution.
Textbook QuestionOne mole of an ideal gas has a volume of 22.414 L at STP. Assuming ideal behavior, what are the densities of the following gases in g/L at STP? (a) CH4 (b) CO2 (c) O21945Has a video solution.
Textbook QuestionWhat are the molecular weights of the gases with the following densities: (a) 1.342 g/L at STP235Has a video solution.
Textbook QuestionTitanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2: 2 TiCl41g2 + H21g2¡2 TiCl31s2 + 2 HCl1g2 (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?165Has a video solution.
Textbook QuestionAutomobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 2 NaN3(s)¡2 Na(s) + 3 N2( g) If an automobile air bag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.40263Has a video solution.
Textbook QuestionLithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2( g)¡2 Li3N(s) What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?978Has a video solution.
Textbook QuestionHydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4( 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. What is the percent yield of the reaction?2472Has a video solution.
Textbook QuestionSuppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (b) density?181Has a video solution.
Textbook QuestionSuppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) number of molecules?202Has a video solution.
Textbook QuestionA gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, was 0.646 g. What is the molecular formula of the compound?1581Has a video solution.
Textbook QuestionConsider the reaction: 2 SO2( g) + O2( g)¡2 SO3( g) a. If 285.5 mL of SO2 reacts with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and the theoretical yield of SO3?714Has a video solution.
Textbook QuestionThe Earth's atmosphere has a mass of approximately 5.15 * 1015 kg. If the average molar mass of air is 28.8 g/mol, how many moles of gas make up the atmosphere? What is the volume of the atmosphere in liters under conditions of STP? (Note: The average molar mass of air is the weighted average of the molar mass of nitrogen and oxygen. 0.20132.0 g>mol2 + 0.80128.0 g>mol2 = 28.8 g>mol.)778Has a video solution.
Textbook QuestionAn herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor expressed at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (b) Calculate its empirical formula.1003Has a video solution.
Textbook QuestionIsooctane, C8H18, is the component of gasoline from which the term octane rating derives. (d) How many moles of air are necessary for the combustion of 1 mol of isooctane, assuming that air is 21.0% O2 by volume? What is the volume in liters of this air at STP?389Has a video solution.
