Consider the following reaction where Kc = 5.10×10-6 at 548 K. NH4CI(s)NH3(g) + HCI(g) A reaction mixture was found to contain 5.75×10 2 moles of NH4CI(s), 2.96×10 3 moles of NH3(g), and 2.26x10 3 moles of HCI(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, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Consider the following reaction where Kc = 5.10×10-6 at 548 K. NH4CI(s)NH3(g) + HCI(g) A reaction mixture was found to contain 5.75×10 2 moles of NH4CI(s), 2.96×10 3 moles of NH3(g), and 2.26x10 3 moles of HCI(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, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 92QRT

See similar textbooks

Similar questions

Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?
9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
Calculate rH for the reaction 2 C(s) + 3 H2(g) + O2(g) C2H5OH() given the information below. C(s) + O2(g) CO2(g) rH = 393.5 kJ/mol-rxn 2 H2(g) + O2(g) 2 H2O() rH = 571.6 kJ/mol-rxn C2H5OH() + 3 O2(g) 2 CO2(g) + 3 H2O() rH= 1367.5 kJ/mol-rxn
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
Methane, ethyne and hydrogen form the following mixture at equilibrium. 2 CH4(g) ↔ C2H2(g) + 3 H2(g) To study this reaction mixture, a chemist analyzes a 4.0 L sealed flask at 1700°C. There are 0.46 mol of CH4(g), 0.64 mol of C2H2(g) and 0.93 mol of H2(g). What is the value of Kc for the reaction at 1700 oC?
Cl2 (g) + CO (g) <-> COCl2 (g) Delta Hrxn = -109 kj/molrxn 1. At equilibrium, the container holds the most molecules of which gas, Cl2(g) of COCl2(g)? Explain you answer. 2. A student hypothesizes that if the temperature of the container is decreased after time t9, the mole fraction of Cl2 in the container will increase. Do you agree or disagree with the student's hypothesis? Justify your answer. 3. Which gas, Cl2(g) or COCl2(g), will deviate most from the ideal gas law at low temperature? Justify your answer.
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc= (_______) / (_______) = (______) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. N₂(g) + O₂(g) ⇌ 2 NO(g) Initial (M) Change (M) Equilibrium (M) Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the…
The value of Keq for the following reaction is 0.25: SO2 (g) + NO2 (g) <==> SO3 (g) + NO (g) The value of Keq at the same temperature for the reaction below is ________. 3SO2 (g) + 3NO2 (g) <==> 3SO3 (g) + 3NO (g) A) 1.6 x 10-2B) 7.5 x 10-1 C) 8.3 x 10-2D) 6.4 x 101E) 0.25
For certain chemical reaction ∆H = 15 kJ/mol and ∆S = 51 J mol-1 K-1, What is ∆G (in kJ/mol) for the reaction when T = a 0o ? A) 1.07 B) -1007 C) 0.107 D) 1007 E) -1.07
For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification
Consider the following reaction that has a Kc = 2.4 x 10^-3 at 1000K: N2(g) + 3 H2(g) = 2NH3(g) in a reaction vessel that is 5.0 x 10^3 L, 250 moles of N2, 250 mol of H2, and 50.0 mol of NH3 are mixed. write the reaction quotient. Calculate Qc.