Mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 molof H2O is placed in a 2.000-Lvessel. The following equilibrium is established at 500 K: CO2(g) + H2(g)CO(g) + H2O(g). (a)Calculate the initial partial pressures of CO2, H2, and H2O.(R=0.0821 L. atm/K. mol)(b)At equilibrium PH2O= 3.51 atm. Calculate the equilibrium partial pressures of CO2, H2, and H2O.(c)Calculate Kp for the reaction.

the law of conservation of mass states that in a chemical reaction, the total mass of reactants is equal to the total mass of products. because atoms are only rearranged in a chemical reaction, there must be the same number of sodium atoms and chlorine atoms in both the reactants and products

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.