An equilibrium mixture of dinitrogen tetroxide, N304, and nitrogen dioxide, NO2, is 63.6% NO, by mass at 1.00 atm pressure and 25°C. Calculate K, at 25°C for the reaction N20,(9) - 2NO2 (9) K.

When 0.200 mol of CaCO,(s) and 0.300 mol of CaO(s) are placed in an evacuated, sealed 10.0-L container and heated to 385 K, PCO, = 0.220 atm after equilibrium is established. 2 CACO,(s) = CaO(s) + CO,(g) Additional CO,(g) is pumped into the container to raise the pressure to 0.470 atm. After equilibrium is re-established, what is the total mass (in g) of CaCO, in the container?

References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer

At a certain temperature, 0.660 mol SO, is placed in a 2.50 L container. 2 SO; (g) = 2 SO,(g)+ 0,(g) At equilibrium, 0.130 mol O, is present. Calculate K. Ke

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: (3)H+(3)0ɔ= (3)0°H+(3)0) The equilibrium constant K for this reaction is 0.735 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. OM

The equilibrium constant, Kc, for the following reaction is 1.20\times 10 - 2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.331 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.