Consider the following equation: C6H8O7(s)  + 3 NaHCO3(s) + H2O(l) --> Na3C6H8O7(s) + 3H2O(l) + 3CO2(g) 193.6 g C6H8O7(s)  is reacted at 313K  and the CO2 gas is collected in a 108.4 L flask. The reaction has 100 percent yield.  What is the pressure of CO2 gas in the flask in units of mm Hg? Molar mass C6H8O7 = 192.1 g   Hint: calculate the amount of moles CO2 gas that will be made, and use PV = nRT to calculate P in atm Hint: in final step you must convert atm  to mm Hg ; 760 mm Hg = 1 atm

An unknown mass of aluminum is added to HCl solution. The aluminum metal is completely dissolved in the solution and generates hydrogen gas. See the balanced equation for the gas evolution reaction: 2 Al(s) + 6 HCl(aq) ---> 2 AlCl3(aq) + 3 H2(g) The following data is collected: Mass of Al sample:                             unknown  g Volume of gas collected                     45.38 mL Barometric pressure                            754.8 mmHg Temperature                                        23.5OC Vapor pressure of H2O at 23.5OC       21.65 mmHg Hydrogen gas is collected over water. The reaction proceeds until all the amount of aluminum is consumed in the gas-evolution reaction (aluminum is the limiting reactant). (a) Calculate the mole number of the hydrogen gas generated in the reaction: Convert the volume of the collected gas to L:  45.38 mL = ___________ L Calculate the pressure exerted by H2 gas (= dry hydrogen gas):          Pressure of the dry hydrogen gas          =…

The nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound  N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.127-g sample of a compound was treated as above, producing 89.0 mL of N2 saturated with water vapor at 25 °C and 739.3 torr.What is the mass percent of nitrogen in the compound? . The vapor pressure of water at 25 °C is 23.8 torr.

4.00 mols of NH3 and 4.00 mols of H2S are placed in an 8.00 L reaction vessel and the mixture is allowed to come to equilibrium. At equilibrium, how many grams of NH4HS (51.11 g/mol) are present? (Assume volume and temperature remain constant.) NH3 (g) + H2S (g) \rightleftarrows⇄ NH4HS (s)       Kc = 400. at 35.0oC

2 H3PO4(s) --> 3 H2(g) + 2 P(s) + 4 O2(g) Using the reaction above, show step by step how many liters of oxygen can be created if I start with 0.7156 grams of H3PO4 solid at STP?

205L of carbon dioxide at STP is compressed and then dissolved in 10.0L of water. What is the molar concentration of teh resulting solution?

For NH3 (g) + O2 (g) ---> NO (g)  + H2O (g), balance the equation and find the number of liters of O2 (g) that can react with 1.5L of NH3 (g) if the gases are at the same temperature and pressure.

Calculate the partial pressure of O2 produced from 1.80 L of 0.576 M N2O5 solution at 45 ∘C over a period of 20.8 h if the gas is collected in a 10.3-Lcontainer. (Assume that the products do not dissolve in chloroform.)

8. In one lab this semester, you ran the reaction: KC1O3 (s) → KCl (s) + O2 (g). The directions asked you to add about 1.5 g KC1O3 to a crucible. How many liters of O2 should form at STP?