3) A rigid 11.7 L sealed vessel containing 3.3 mol of O2(e), 1.6 mol of CH4(g), and 2.3
mol of He has an internal temperature of 78°C.
a. Calculate the partial pressure of each gas.
b. W hat is the total pressure in the vessel?
c. Find the mole fraction of each gas in the vessel.
d. A lab technician ignites the mixture in the flask and the following reaction
occurs: CH4(g) +2 02(g)→ CO2(g) + 2 H2O(g). Find the mole fraction of
each gas in the mixture after the reaction.
(Hint: Use an ICE chart. There is a limiting reactant.)

Many reactions take place in aqueous solution. when potential reactants are mixed, a reaction will occur if there is some driving force that favors the formation of products. it is often convenient to categorize reactions in terms of these driving forces: precipitate formation, in which an insoluble solid is formed, weak electrolyte formation, as in a neutralization reaction involving water, or transfer of electrons, as in a redox reaction. these reactions can be represented by full molecular equations, which contain all species in the reaction mixture, or by net ionic equations, which show only the species that actually undergo a change. the latter does not contain the spectator ions, which do not undergo a net change or do not take part in the reaction. part a when the following two solutions are mixed: k2co3(aq)+fe(no3)3(aq) the mixture contains the ions listed below. sort these species into spectator ions and ions that react. drag the appropriate items to their respective bins. view available hint(s) spectator ions ions that react part b what is the correct net ionic equation, including all coefficients, charges, and phases, for the following set of reactants? assume that the contribution of protons from h2so4 is near 100 %.ba(oh)2(aq)+h2so4(aq)→ express your answer as a chemical equation. view available hint(s) nothing provide feedback