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An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). The system then re - equilibrates. The appropriate chemical equation is PCl3(g) + Cl2(g) PCl5(g) Calculate the new partial pressures after equilibrium is reestablished. PpCl3 = Torr PCl2 = Torr PpCl5 = Torr 4.60 mol of solid A was placed in a sealed 1.00 - L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.30 M, where it remained constant. A(s) B(g) + C(g) Then, the container volume was doubled and equilibrium was re - established. How many moles of A remain? mol A An equilibrium mixture contains 0.400 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 - L container. CO(g) + H2O(g) CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase tne amount of carbon monoxide to 0.300 mol? mol Recall that when a reaction is at equilibrium, the forward and reverse reactions occur at the same rate. To illustrate this idea, consider the reaction of A and B to form AB. A + B AB Click the "React" button below to see what happens. Notice that the reaction never stops. Even after several minutes, there is A and B left unreacted. and the forward and reverse reactions continue to occur. Also note that amounts of each species (i.e., their concentrations) stay the same. What is the value of the equilibrium constant for this reaction? Assume each atom or molecule represents a 1 M concentration of that substance. K = What generalizations can be made about equilibrium and changes in concentration? Use the simulation below to help you answer the question. A + B AB K = 1 Q = 4.00/2.00 times 2.00 = 1.00 After changing the height of the bars in the graph, they re - adjust, but eventually stop. Why? The reaction stops once it reaches equilibrium. The forward and reverse reactions occur at the same rate keeping the concentrations constant. Click the blue triangles or drag the bars up and down. What is the value of K for this aqueous reaction at 298 K? A + B C + D DeltaGdegree = 26.82 kJ / mol Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M2O(s) 2M(s) + 1/2 O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Delta = kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = What is the equilibrium pressure of O2(g) over M(s) at 298 K? P02 = atm At 25 degree C, the equilibrium partial pressures for the following reaction were found to be PA = 1.70 atm, PB = 8.50 atm, Pc = 2.20 atm, and PD = 5.00 atm. A(g) + 2B(g) rightarrow C(g) + D(g) What is the standard change in Gibbs free energy of this reaction at 25 degree C. DeltaGdegree rxn = kJ / mol When the oxide of generic metal M is heated at 25.0 degree C, only a negligible amount of M is produced. MO2(s) M(s) + O2(g) DelteGdegree = 291.1 kJ / mol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s). What is the thermodynamic equilibrium constant for the coupled reaction? K = For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g) + 3H2(g) 2NH3(g) the standard change in Gibbs free energy is DeltaGdegree = - 69.0 kJ/mol. What is DeltaG for this reaction at 298 K when the partial pressures are PK = 0.100 atm, PH2 = 0.450 atm, and PNH3 = 0.900 atm DeltaG = kJ / mol

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