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VII(15pts) The following nitrocubane structure. CxHOis was thought to be a possible explosive A possible decompositi...
VII(15pts) The following nitrocubane structure, CH,O16, was thought to be a possible explosive: ON. NO2 O2N...
VII(15pts) The following nitrocubane structure, CH,O16, was thought to be a possible explosive: ON. NO2 O2N NO2 O2N NO2 NO2 O2N :> 8 C(s) +8 O:(g) +4 N,(g) C,N,O(s) A possible decomposition reaction is What is the total volume of gases collected at 1.6 atm and 28.0°C from 2.75 x 102 g of nitrocubane. Also, calculate the partial pressure of cach gas under these conditions.
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it...
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it explodes) as shown in the equation below. Calculate the volume in mL of nitrogen gas that will be collected at 1.25 atm and 112°C by the decomposition of 12.8 g of nitroglycerin, C3H5(NO3)3. Use the correct SF and units. 4 C3H5(NO3)3 (1) -->6 N2(g) + O2 (g) + 12 CO2 (g) + 10 H20 (g)
Ideal Gas Law and Partial Pressures Name Directions: Calculate/answer the following: 1. 7.70 moles of Argon...
Ideal Gas Law and Partial Pressures Name Directions: Calculate/answer the following: 1. 7.70 moles of Argon at a pressure of 0.190 atm and at a temperature of 65.8 °C, what is the volume of the container that the gas is in? 2. A sample of gas is 17.0 moles at a temperature of 77.0 °C, and a volume of 98.9 liters, what is the pressure of the gas? 3. 28.0 moles of gas held at a pressure of 580 atm...
Can I have help with these questions based off the information provided? Information: The explosive picric...
Can I have help with these questions based off the information provided? Information: The explosive picric acid is also known by the IUPAC name 2,4,6-Trinitrophenol. Picric acid is known as a primary explosive and the balanced equation for the explosion is 4 C6H3N3 O7 (aq) + 13 O2 (g) --> 6 H2O (g) + 6 N2 (g) + 24 CO2 (g) volume of gas produced by 1 g is 0.89 L Type bond broken # bond type Enthalpy (KJ/mol Total...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas and 16.5 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: 3 dinitrogen difluoride partial pressure: atm Х ? mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure...
Ta=191.4k| 4 P = 850 forr Pa -0.65 om. 2496 ore A 5.50 L volume of...
Ta=191.4k| 4 P = 850 forr Pa -0.65 om. 2496 ore A 5.50 L volume of gas has a pressure of 0.950 atm at 0°C. What is the pressure volume decreases to 4.75 L and the temperature increases to 35°C? V=5.SOL P=0.950 atm P2=1.22atml S. A 0.112 mol quantity of gas has a volume of 2.54 L at a certain temperature and pressure. What is the volume of 0.0750 mol of gas under the same conditions? V2 = 1902) (6....
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas...
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas and 3.32 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: carbon dioxide partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas and 10.1 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas and 13.0 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: sulfur hexafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 10.0 I. tank at 13.4 °C is filled with 10.3 g of dintrogen dinluoride gas...
A 10.0 I. tank at 13.4 °C is filled with 10.3 g of dintrogen dinluoride gas and 10.6 g of dinitrogen monoxide gas. You can assume both gases behave as ideal gases under these conditions. Galculate the mole fraction and partial pressure of each gas, and the total pressure in the tank Round cach of your answers to 3 significant digits. 0 3931 dinitrogen difluoride atn 0.607 dinitrogen monoxide atm 949 atm e gas and 10.6 g of assume both...
VII(15pts) The following nitrocubane structure, CH,O16, was thought to be a possible explosive: ON. NO2 O2N NO2 O2N NO2 NO2 O2N :> 8 C(s) +8 O:(g) +4 N,(g) C,N,O(s) A possible decomposition reaction is What is the total volume of gases collected at 1.6 atm and 28.0°C from 2.75 x 102 g of nitrocubane. Also, calculate the partial pressure of cach gas under these conditions.
Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it explodes) as shown in the equation below. Calculate the volume in mL of nitrogen gas that will be collected at 1.25 atm and 112°C by the decomposition of 12.8 g of nitroglycerin, C3H5(NO3)3. Use the correct SF and units. 4 C3H5(NO3)3 (1) -->6 N2(g) + O2 (g) + 12 CO2 (g) + 10 H20 (g)
Ideal Gas Law and Partial Pressures Name Directions: Calculate/answer the following: 1. 7.70 moles of Argon at a pressure of 0.190 atm and at a temperature of 65.8 °C, what is the volume of the container that the gas is in? 2. A sample of gas is 17.0 moles at a temperature of 77.0 °C, and a volume of 98.9 liters, what is the pressure of the gas? 3. 28.0 moles of gas held at a pressure of 580 atm...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas and 16.5 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: 3 dinitrogen difluoride partial pressure: atm Х ? mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure...
Ta=191.4k| 4 P = 850 forr Pa -0.65 om. 2496 ore A 5.50 L volume of gas has a pressure of 0.950 atm at 0°C. What is the pressure volume decreases to 4.75 L and the temperature increases to 35°C? V=5.SOL P=0.950 atm P2=1.22atml S. A 0.112 mol quantity of gas has a volume of 2.54 L at a certain temperature and pressure. What is the volume of 0.0750 mol of gas under the same conditions? V2 = 1902) (6....
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas and 3.32 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: carbon dioxide partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas and 10.1 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas and 13.0 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: sulfur hexafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 10.0 I. tank at 13.4 °C is filled with 10.3 g of dintrogen dinluoride gas and 10.6 g of dinitrogen monoxide gas. You can assume both gases behave as ideal gases under these conditions. Galculate the mole fraction and partial pressure of each gas, and the total pressure in the tank Round cach of your answers to 3 significant digits. 0 3931 dinitrogen difluoride atn 0.607 dinitrogen monoxide atm 949 atm e gas and 10.6 g of assume both...
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