Part A- Calculate the density of sulfur hexafluoride gas at 704 torr and 21 ∘C.
Part B- Calculate the molar mass of a vapor that has a density of 7.125 g/L at 12 ∘C and 744 torr .
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Part A- Calculate the density of sulfur hexafluoride gas at 704 torr and 21 ∘C. Part...
6. a. Calculate the density of sulfur hexafluoride gas at 709 torr and 23 C. b. Calculate the molar mass of a vapor that has a density of 7.125 g/L at 11 ∘C and 745 torr . c. Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2(s)+2H2O(l)→Ca(OH)2(aq)+2H2(g) This reaction is sometimes used to inflate life rafts, weather balloons, and the like, where a simple, compact means of generating H2 is desired. How many grams of CaH2 are needed...
please help Calculate the density of sulfur hexafluoride gas at 709 torr and 20 degree C. Express the density in grams per liter to three significant digits. d = g/L
Density of an Ideal Gas Calculate the density of sulfur hexafluoride (SF6) gas at 293°C and 2.36 atm. Submit Answer Tries 0/5 Post Discussion
A student analyzes a gas mixture of sulfur hexafluoride (SF_6) and selenium hexafluoride (SeF_6) and finds that the density of the sample is 6.90 g/L at a temperature of 23 degrees C and a pressure of 0.942 atm. Calculate the partial pressure of sulfur hexafluoride.
A reaction at 28.0 °C evolves 223. mmol of sulfur hexafluoride gas. Calculate the volume of sulfur hexafluoride gas that is collected. You can assume the pressure in the room is exactly I atm. Round your answer to 3 significant: digits. volume: |L
calculate the mass of sulfur dioxide gas at 212 C, 622 torr and a volume of 0.270 L
A 5.00 L tank at 2.04 °C is filled with 3.27 g of sulfur hexafluoride gas and 9.57 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: Tx 5 ? mole fraction: dinitrogen difluoride partial pressure: Total pressure...
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...
The density of a gas is 2.08 g/Lg/L at a temperature of 21 ∘C∘C and a pressure of 0.784 atmatm . Calculate the molar mass of the gas.
A reaction at -10.0 °C evolves 300. mmol of sulfur hexafluoride gas. Calculatet volume of sulfur hexafluoride gas that is collected. You can assume the pressur the room is exactly 1 atm. Be sure your answer has the correct number of signi igits