Use the ideal gas law to calculate the moles of gas required to fill your bag. Determine the molecular weight of each of

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Use The Ideal Gas Law To Calculate The Moles Of Gas Required To Fill Your Bag Determine The Molecular Weight Of Each Of 1 (79.99 KiB) Viewed 72 times

Use the ideal gas law to calculate the moles of gas required to fill your bag. Determine the molecular weight of each of your reagents. Calculate how many grams of sodium bicarbonate will produce that number of moles of gas. Calculate the volume of 6.0 Macetic acid that you will use. (Remember that the mole ratios are 1:1, so you will need the same number of moles of sodium bicarbonate as acetic acid as carbon dioxide gas you want to produce.) 5. Measure out the calculated amount of sodium bicarbonate and acetic acid. If you get acid on your skin, wash immediately with water. 6. Hold your bag with a fold in the bottom that will prevent the reagents from mixing until after you've sealed the bag. Add the sodium bicarbonate to one corner, and the acetic acid to the other corner. Seal the bag without trapping air in it. Release the fold, and shake the bag to mix the reagents. 7. Assess the fullness of your "airbag” after 8-10 minutes. If it is not full, adjust your amounts and repeat the experiment using the same bag. Fluid in the bag can be poured down the drain. Be sure to show your successful “airbag” to your instructor. Data Room temperature: _68F_= 20_°C = _293.15_K Atmospheric pressure: 30.111_inHg = _764.79401_mmHg Bag volume (L) determined using water mL Calculate the moles of CO2 needed to fill your bag. Show your work. 2900 Name 3 Moles CO2 needed Moles NaHCO3 needed g NaHCO, needed Moles CH3COOH needed ml CH3COOH needed Show your calculations of g NaHCO3, mL CH3COOH Observations: What did it look like? (including success or failure): If you need to repeat the experiment, provide the same information as above in the space below.