For the reaction: PH4Cl(g) qe PH3(g) + HCl(g), Kc = 1.10*1010 (451 K), held within a 1.00 L flask  Is the reaction at equilibrium if [PH4Cl] = 0.350 M, [PH3] = 3.31*10-3 M and [HCl] = 0.137 M? If not, what direction must the reaction proceed to achieve equilibrium.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2 (g) + 2 H,0(g) =2H,(g) + 2 NO (g) 8. :4. × 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? x10 no If you said yes, then enter the equilibrium pressure of NO at right. O Round your answer to 1 significant digit. atm

Calculatıng équllibiiuml CompositiUIT iTum un Suppose a 250. mL flask is filled with 0.70 mol of O, and 1.9 mol of NO. The following reaction becomes possible: N2(3) + 0,(g) - 2NO(3) The equilibrium constant K for this reaction is 1.81 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. | M Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use

Consider the formation of phosphorus pentachloride from phosphorus trichloride and chlorine gas: PCl3 (g) + Cl2 (g) <---> PCl5 (g) If the equilibrium constant at a certain temperature is Kc = 1.36, what will the equilibrium concentration of PCl5 (g) be if the initial concentrations of the two reactant gases was each 0.450 M and that of the product was 0.100 M?  (Note - the value of Q for the initial concentrations is 0.494, which is just a little below the value of Keq - although the reaction will proceed toward products, the final concentration of PCl5 will not increase very much).