How many moles of sodium are needed to produce 17.7 L of hydrogen gas according to the following reaction at 0 °C and 1 atm? sodium(s) + water (l) → sodium hydroxide (aq) + hydrogen (g) Amount = moles

9. How many liters of oxygen are required to react completely with 2.4 liters of hydrogen to form water? 2H 2H.O

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 125 L tank with 20. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.0 mol of carbon monoxide gas, 11. mol of water vapor and 13. mol of carbon dioxide. The engineer then adds another 7.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. mol

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

At a certain temperature, 0.9239 mol of SO3 is placed in a 3.00 L container, and it reacts according to the balanced chemical equation below. 2 SO3 (g) ⇋ 2 SO2 (g) + O2 (g) At equilibrium, 0.6431 mol of SO2 is present. Calculate the Kc (molar Keq)

Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

Consider the following reaction. 2 NO₂(g) = N₂O4(g) 4 When the system is at equilibrium, it contains NO₂ at a pressure of 0.860 atm, and N₂O at a pressure of 0.0740 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? atm PNO₂ = atm PN₂0₁ =

For the reaction shown, how many grams of Hg can be produced by the reaction of 18.0 g of HgO? Report 3 sig figs and don't put in units, just enter a number.                                                         2HgO(s) -->  2Hg(l) + O2(g)

11. How much iron, in kg, would need to be used in excess oxygen to produce 1,679 g of rust (iron(III) oxide)?  use dimensional analysis to complete this question

0.840 mol of SO3 (g) was placed in a 3.00 L reaction vessel and underwent the reaction shown below: 2 SO3 (g) = 2 SO2 (g) + O2(g) 7 If there is 0.140 mol of O₂ (g) in the reaction vessel when the system reaches equilibrium, what is the equilibrium constant, Kc, for the reaction. Ke: