Consider the following reaction where Ke = 5.10 x 10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction mixture was found to contain 0.0531 moles of NH4Cl(s), 0.00147 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium. Submit Answer Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining
Consider the following reaction where Ke = 5.10 x 10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) A reaction mixture was found to contain 0.0531 moles of NH4Cl(s), 0.00147 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q, equals The reaction O must run in the forward direction to reach equilibrium. O must run in the reverse direction to reach equilibrium. O is at equilibrium. Submit Answer Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 3ALQ: For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each...
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