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Calculate the mass grams of N2 gas required to occupy a 3.0 mL container at 100 C and 0.914 ATM and explain how you did it?
Wiki User
∙ 13y ago
Use equation n=PV/RT where n is number of moles and R is gas constant. Use R= .8314 L-Atm/mol-K. convert 3 ml to liters(3/1000) and 100C to Kelvin (100+273) and solve for moles.
Convert moles to grams. 1 mol of N2 equals 28 grams
Wiki User
∙ 13y ago
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grams law of diffusion deals with gases spreading out to occupy the shape of their container.
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Well, since a gas spreads to encompass its container, it should have the same volume as its container.
Calculate the mass in grams of N2 gas required to occupy a 3.0 mL container at 100 C and 0.914 ATM and explain how you did it?
Whilst I'm not going to do the actual calculation for you, I suggest you use the ideal gas law. PV=nRT P is Pressure in pascals (1 ATM is roughly 100,000pa) V is Volume in cubic metres (be careful converting mL to cubic metres) n is the number of mols R is the molar gas constant which is roughly 8.31 T is temperature in kelvin so to find mass you rearrange for number of mols n=PV/RT Work it out and then use the molar mass of nitrogen to convert into grams
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What is true of all particles of a gas encloosed within a container?
Well, since a gas spreads to encompass its container, it should have the same volume as its container.
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Calculate the mass in grams of N2 gas required to occupy a 3.0 mL container at 100 C and 0.914 ATM and explain how you did it?
Whilst I'm not going to do the actual calculation for you, I suggest you use the ideal gas law. PV=nRT P is Pressure in pascals (1 ATM is roughly 100,000pa) V is Volume in cubic metres (be careful converting mL to cubic metres) n is the number of mols R is the molar gas constant which is roughly 8.31 T is temperature in kelvin so to find mass you rearrange for number of mols n=PV/RT Work it out and then use the molar mass of nitrogen to convert into grams
