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Use the following scenario for the next two questions The reaction for the refo…

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Wize University Chemistry Textbook > Equilibrium

Solving for K in Different Scenarios

2 Activities

Wize University Chemistry Textbook > Equilibrium

Q (Reaction Quotient)

4 Activities

Use the following scenario for the next two questions
The reaction for the reforming of methane from steam is given by:
CH4(g)+H2O(g)⇌CO(g)+3H2(g)CH_4 (g) + H_2 O (g) ⇌ CO (g) + 3 H_2 (g)
A closed reaction vessel starts with initial concentrations of 1.00 M for every gas.
After some time had elapsed, researchers found that the H2 concentration was 0.70 M. What was the concentration of CH4 (g) in the vessel at this time?
More Solving for K in Different Scenarios Questions:
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Concept Clarifier
Consider the following reaction
2 SO2+O2⇌2 SO3\rm 2\ {SO_2} \quad+\quad {O_2}\quad \xrightleftharpoons{\hspace{1.5cm}}\quad 2\ {SO_3}
ΔH0=−180 kJ/mol\Delta H^0=-180\ kJ/mol
Equilibrium constant
The value of Kp for the reaction: NO (g) ⇌ ½ N2 (g) + ½ O2 (g) is 2.5x107. What is the Kp for the reaction: N2 (g) + O2 (g) ⇌ 2 NO (g)?
Equilibrium constant
The equilibrium constant for reaction #1 below is K. The equilibrium constant for reaction #2 is therefore ________.
(1) 2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
(2) SO2 (g) + ½ O2 (g) ⇌ SO3 (g)
Equilibrium constant
Consider the following equilibrium: 2 HI (g) ⇌ H2 (g) + I2 (g)
If the equilibrium constant for this reaction at a certain temperature is Kc = 0.04, what is the equilibrium constant K’c for the following reaction at the same temperature:
½ H2 (g) + ½ I2 (g) = HI (g)
Equilibrium constant
For the following equilibria determine whether K>1K > 1, K<1K < 1 or K≈1K \approx 1. Enter your answers as "Greater", "Less", "1" respectively.
A)
B)
Equilibrium: Equilibrium constant
If the equilibrium constant for reaction 1 below is K, what is the equilibrium constant for reaction 2?
(1) SO2 (g) + ½ O2 (g) ⇌ SO3 (g)
(2) 2SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
Equilibrium: Equilibrium constant
If Kc = 0.212 at 100oC for N2O4 (g) ⇌ 2 NO2 (g)
Determine the value of Kc at 100oC for 2 NO2 (g) ⇌ N2O4 (g)
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_{2(g)} \hspace{20pt} K_{c,1}
2H2S(g)⇌2H2(g)+S2(g)Kc,22H_2S_{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_{c,2}
A reaction is found to have an equilibrium constant of 3.5 x 10-3 at standard temperature. If the enthalpy change of this process is +45.6 kJ/mol, what will be the value of the equilibrium constant at 455 K?
At 450 K, the equilibrium constant in terms of pressure,
CO(g)+H2O(g)→H2(g)+CO2(g)Kp=34.7CH4(g)+O2→CO2(g)+2 H2(g)Kp=119.2\begin{array}{cc} CO_{(g)}+H_2O_{(g)}\rightarrow H_{2(g)}+CO_{2(g)} & K_p=34.7 \\ CH_{4(g)}+O_{2}\rightarrow CO_{2(g)}+2\ H_2{(g)} & K_p=119.2 \end{array}
What is Kp for the following reactio at 450 K?
The equilibrium constant, Kc, for the following reaction below was measured at 7.7.
SO3(g)+NO(g)⇌NO2(g)+SO2(g)SO_{3}(g)+NO(g)\rightleftharpoons NO_{2}(g)+SO_{2}(g)
At the same temperature the measurement was taken, a mixture of 0.4 M SO3 and 0.4 M NO was generated. After allowing the system to reach equilibrium what is the concentration of SO2?
Equilibrium constant
At a certain temperature, the value of the equilibrium constant for the following reaction is
Kc = 100. N2 (g) + 2 O2 (g) ⇌ 2 NO2 (g)
What is the equilibrium constant for the following reaction?
Equilibrium: ICE Table
Cyclohexane (C6H12) undergoes an isomerization in the presence of the appropriate catalyst to form a compound called MCP.
C6H12 (g) ⇌ MCP (g) Kc = 0.143 at 25oC
The initial concentrations are [C6H12] = 0.800 M and [MCP] = 0.100 M. What are the equilibrium concentrations of these two compounds?
Equilibrium: Equilibrium Constant
For the equilibrium process 2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g), determine the value of Kc when an equilibrium mixture contains 0.025 mol O2, 0.27 mol SO2, and 0.018 mol SO3 in a 5.00 liter container at 220oC.
A reaction mixture consisting of 0.400 mol H2 and 1.60 mol I2 was introduced into a 3.00 L flask and heated. At equilibrium 60% of the hydrogen gas had reacted. What is the equilibrium constant Kc for the reaction H2 (g) + I2 (g) ⇌ 2 HI (g)?
If the equilibrium constant for reaction 1 below is K, what is the equilibrium constant for reaction 2?
1. SO2(g) + ½ O2(g) ⇌ SO3(g)
2. 2 SO3(g) ⇌ 2 SO2(g) + O2(g)
If Kc = 0.212 at 100oC for N2O4(g) ⇌ 2 NO2(g)
Determine the value of Kc at 100oC for 2 NO2(g) ⇌ N2O4(g)
Equilibrium constant
At 550oC acetic acid (CH3COOH) is a gas. A sample of pure acetic acid vapour at 550oC decomposes into carbon dioxide (CO2) and methane (CH4) with an equilibrium constant of 3.40 X 104 measured in kPa. At equilibrium a near-IR spectrometer meassures the methane partial pressure to be 255 kPa. What are the equilibrium partial pressures for carbon dioxide and acetic acid?
Express your answer in units of kPa to three significant figures. do not include units in the answer field
Equilibrium Constant
A one liter vessel was filled with 0.398 mol of NOCl(g). Then the temperature of the system was increased to 245 °C to undergo the following reaction:
2NOCl(g)⇌2NO(g)+Cl2(g)2NOCl(g) \rightleftharpoons 2NO(g) +Cl_2(g)
When equilibrium was attained, the concentration of Cl2 was 0.0225 mol/liter. Calculate the value of Kc at 245 °C for the reaction.
Equilibrium
Consider the following equilibria:
2HCl(g)⇌H2(g)+Cl2(g)Kc,12HCl_{(g)} \rightleftharpoons H_{2(g)} +Cl_2{(g)} \hspace{20pt} K_c,1
2H2S2(g)⇌2H2(g)+S2(g)Kc,22H_2S_2{(g)} \rightleftharpoons 2H_{2(g)} +S_2{(g)} \hspace{20pt} K_c,2
Equilibrium: Equilibrium constant
For the equilibrium process NH4SH (s) ⇌ NH3 (g) + H2S (g), Kc = 1.2x10-4 at 218oC. What is the equilibrium concentration of NH3 if a sample of NH4SH is allowed to achieve equilibrium at 218oC in a sealed rigid vessel?
Equilibrium: Equilibrium Constant
For the equilibrium process 2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g), determine the value of Kc when an equilibrium mixture contains 0.025 mol O2, 0.27 mol SO2, and 0.018 mol SO3 in a 5.00 liter container at 220oC.
Equilibrium: Equilibrium Constant
If Kc = 0.212 at 100oC for N2O4 (g) ⇌ 2 NO2 (g)
Determine the value of Kc at 100oC for 2 NO2 (g) ⇌ N2O4 (g)
Equilibrium constant
A 1.0 L flask was loaded and the system was allowed to reach equilibrium at 25 °C. The equilibrium mixture was found to contain: 1.5 mol Cr (S), 1.5 mol CCI4 (g), 2.3 mol CrCl3, (g), and 2.5 mol C (S). Determine the Kc value for this reaction at 25 °C.
Equilibrium Constant
Based on the reactions and equilibrium constants given below, determine the value of the equilibrium constant (Kf) for the formation of the soluble PbI42- complex:
𝑃𝑏𝐼2(𝑠)⇌𝑃𝑏2+(𝑎𝑞)+2𝐼−(𝑎𝑞)𝐾𝑠𝑝=7.9×10−9𝑃𝑏𝐼2(𝑠)+2𝐼−(𝑎𝑞)⇌𝑃𝑏𝐼42−(𝑎𝑞)𝐾=2.37×10−4𝑃𝑏2+(𝑎𝑞)+4𝐼−(𝑎𝑞)⇌𝑃𝑏𝐼42−(𝑎𝑞)𝐾𝑓=?\begin{alignedat}{} &𝑃𝑏𝐼_2 (𝑠) ⇌𝑃𝑏^{2+}(𝑎𝑞)+2 𝐼^− (𝑎𝑞) &&𝐾_{𝑠𝑝}=7.9×10^{−9}\\ &𝑃𝑏𝐼_2(𝑠)+2 𝐼^− (𝑎𝑞) ⇌𝑃𝑏𝐼_4^{2−} (𝑎𝑞) &&𝐾=2.37×10^{−4}\\ &𝑃𝑏^{2+} (𝑎𝑞)+4 𝐼^− (𝑎𝑞)⇌𝑃𝑏𝐼_4^{2−} (𝑎𝑞) &&𝐾_𝑓= ? \end{alignedat}
Which answer below correctly describes the calculation to find the equilibrium expression K4?
CH4(g)+H2O(g)⇌CO(g)+3H2(g)K1CH4(g)+2S2(g)⇌CS2(g)+2H2S(g)K2CO2(g)+H2(g)⇌CO(g)+H2O(g)K3CS2(g)+2H2S(g)+3CO2(g)⇌4CO(g)+2S2(g)+2H2O(g)K4\def\arraystretch{1.5} \begin{array}{c:c} CH_4 (g)+H_2 O(g)⇌CO(g)+3H_2 (g) & K_1 \\ CH_4 (g)+2S_2 (g)⇌CS_2 (g)+2H_2 S(g) & K_2\\ CO_2 (g)+H_2 (g)⇌CO(g)+H_2 O(g) & K_3\\ CS_2 (g)+2H_2 S(g)+3CO_2 (g)⇌4CO(g)+2S_2 (g)+2H_2 O(g) & K_4 \end{array}
Equilibrium Constant
Given the following information:
Ni(OH)2(s)⇌Ni2+(aq)+2OH−(aq)Ksp=6.0×10−16H2O(l)⇌H+(aq)+OH−(aq)Kw=1.0×10−14\def\arraystretch{1.5}\begin {array}{cc}Ni(OH)_2 (s) ⇌Ni^{2+} (aq)+2OH^- (aq)&&K_{sp}= 6.0 ×10^{-16}\\ H_2 O(l) ⇌H^+ (aq)+OH^- (aq) &&K_w= 1.0×10^{-14}\end{array}
What is the equilibrium constant for the reaction,
Equilibrium: Equilibrium constant
At 25 ˚C, KP = 5.2 × 10–2 for the following decomposition reaction:
NH4HS(s)⇌NH3(g)+H2S(g)NH_4HS(s)⇌NH_3(g)+H_2S(g)
Given the following information at 298 K:
SnO2(s)+2H2(g)⇌Sn(s)+2H2O(g)K1=8.12H2(g)+CO2(g)⇌H2O(g)+CO(g)K2=0.771\def\arraystretch{1.5} \begin{array}{cc} SnO_2 (s) + 2 H_2 (g) ⇌ Sn (s) + 2 H_2 O (g) & K_1 = 8.12 \\ H_2 (g) + CO_2 (g) ⇌ H_2 O (g) + CO (g) &K_2 = 0.771 \end{array}
Determine the K for the overall reaction: SnO2(s)+2CO(g)⇌Sn(s)+2CO2(g).SnO_2 (s) + 2 CO (g) ⇌ Sn (s) + 2 CO_2 (g).
Equilibrium and Le Chatelier's Principle
At time = t0, 0.40 mol of Br2 (ℓ) and 0.40 mol of Cℓ2 (g) are placed in an empty, rigid 10.00 L flask and allowed to reach equilibrium.
After reaching equilibrium at time = t2, the flask is found to contain 0.20 mol of BrCℓ (g). The temperature is held constant throughout the reaction.
Equilibrium: Keq Values
Consider the following equilibria:
2HBr(g)⇌H2(g)+Br(g)Kc,12HBr_{(g)} \rightleftharpoons H_{2(g)} +Br_{(g)} \hspace{20pt} K_c,_1
2H2O(g)⇌2H2(g)+O(g)Kc,22H_2O_{(g)} \rightleftharpoons 2H_{2(g)} +O_{(g)} \hspace{20pt} K_c,_2
More Q (Reaction Quotient) Questions:
Practice: Calculating Equilibrium Concentrations
Iodine chloride (ICl) can decompose, forming iodine and chlorine gases. If a reaction vessel is prepared by filling a 5.00 L container with 0.500 mol each of ICl, I2, and Cl2.
2ICl(g)⇌I2(g)+Cl2(g)KC=0.110 (at 25°C)2ICl(g)⇌I_2 (g)+Cl_2 (g)\qquad K_C = 0.110\ (at \ 25°C)
a) In which direction will the reaction proceed (towards products or reactants)? Show how you determined your answer.
Equilibrium constant: Reaction quotient
Consider the reaction:
A+2B⇌C+DA + 2B ⇌ C + D
At a particular temperature this reaction is reactant-favoured at equilibrium. If for the current concentrations the forward reaction is favoured, which of the following statements is true?
The system: H2(g)+X2(g)⇌2HX(g)H_2(g) + X_2(g) \rightleftharpoons 2 HX(g) has a value of 24.4 for K. A system being studied in a 3.00 liter reactor was charged with 0.150 moles of H2, 0.150 moles of X2, and 0.600 moles of HX. A catalyst was introduced using a remote unit. Which statement below describes the situation?
Express the reaction quotient for the following equilibria in terms of partial pressures and concentration.
2 H2O(l)⇌2 H2(g)+O2(g)\rm 2\ H_2O_{(l)} \quad\xrightleftharpoons{\hspace{1.5cm}}\quad 2\ H_{2(g)}\quad+\quad O_{2(g)}
Express the reaction quotient for the following equilibria in terms of partial pressures and concentration.
 CH4(g)+2 O2(g)⇌CO2(g)+2 H2O(g)\rm \ {CH_{4(g)}} \quad+\quad 2\ {O_{2(g)}}\quad \xrightleftharpoons{\hspace{1.5cm}}\quad {CO_{2(g)}}\quad+\quad 2\ H_2O_{(g)}
At 425 °C, Kp = 4.18 x 10-9 for the reaction:
2HBr(g)↔H2(g)+Br2(g)2HBr_{(g)}\leftrightarrow H_{2(g)}+Br_{2(g)}
In one experiment 0.20 atm of HBr, 0.100 atm of H2 and 0.010 atm of Br2 are placed in a container. Is the reaction at equilibrium? If not, in which direction will it proceed?
At 425 °C, Kp = 4.18 x 10-9 for the reaction:
2HBr(g)↔H2(g)+Br2(g)2HBr_{(g)}\leftrightarrow H_{2(g)}+Br_{2(g)}
In one experiment 0.20 atm of HBr, 0.100 atm of H2 and 0.010 atm of Br2 are placed in a container. Is the reaction at equilibrium? If not, in which direction will it proceed?
Which of the following statements regarding the reaction quotient Qc and the equilibrium constant Kc is true?
Consider the reaction of nitrogen and oxygen gases to produce nitric oxide:
N2(g)+O2(g)⇌2NO(g)                   Kc=4.0×10−4  at  1750 oCN_2(g)+O_2(g) \rightleftharpoons 2NO(g)\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ K_c=4.0\times 10^{-4}\ \ at\ \ 1750 \ ^oC
What is the value of Kp for this reaction at 1750 °C?
At 425 °C, Kp = 4.18 x 10-9 for the reaction:
2HBr(g)↔H2(g)+Br2(g)2HBr_{(g)}\leftrightarrow H_{2(g)}+Br_{2(g)}
In one experiment 0.20 atm of HBr, 0.100 atm of H2 and 0.010 atm of Br2 are placed in a container. Is the reaction at equilibrium? If not, in which direction will it proceed?
Equilibrium: Reaction quotient
The system: H2(g) + X2(g) : 2 HX(g) has a value of 24.4 for Kc. A system being studied in a 3.00 liter reactor was charged with 0.150 moles of H2, 0.150 moles of X2, and 0.600 moles of HX. A catalyst was introduced using a remote unit. Which statement below describes the situation
Consider the following reaction to answer the next two questions:
4Cr(s)+3CCl4(g)⇄4CrCl3(g)+3C(s)        ΔH=26.9kJ4Cr(s)+3CCl_4(g) \rightleftarrows 4CrCl_3(g) +3C(s)\ \ \ \ \ \ \ \ \Delta H=26.9kJ
Equilibrium: Reaction quotient
Consider the following reaction:
4 HCl (g) + O2 (g) ⇌ 2 Cl2 (g) + 2 H2O (g) Kc = 0.063 at 400 K
If the reaction quotient, Q, is 0.100, which of the following statements is FALSE?
Equilibrium: Reaction quotient
The equilibrium constant expressed in terms of partial pressure for the water gas reaction (shown) is Kp = 2.6 at a temperature of 1000 K. C (s) + H2O (g) ⇌ CO (g) + H2 (g)
A closed vessel initially has a sample of solid carbon (graphite), and P(H2O(g)) = 0.600 atm and
P(CO(g)) = 1.525 atm and P(H2(g)) = 0.804 atm. Which one of the following statements is TRUE?
Equilibrium: Magnitude of equilibrium constant
The value of Kc for a particular chemical equilibrium is 1.0x1013. Hence, we can conclude:
Equilibrium: Reaction quotient
The Kc for the Haber process N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) is 9.60 at 573 K. When 1.0x10-3 moles of ammonia is mixed in a 1 L flask at 573 K with 1.0x10-2 moles of hydrogen and 5.0x10-1 moles of nitrogen, one can conclude that:
Equilibrium: Reaction quotient
Which statement is CORRECT for a reaction that has Kc = 2.43x10-12?
Equilibrium: Reaction quotient
Sulfuryl dichloride (SO2Cl2) can be prepared by the following two-step reaction sequence.
H2S (g) + 1.5 O2 (g) ⇌ SO2 (g) + H2O (g)
SO2 (g) + Cl2 (g) ⇌ SO2Cl2 (g)
Equilibrium: Reaction quotient
For the equilibrium process N2O4 (g) ⇌ 2 NO2 (g), Kc = 0.212 at 100oC. If a reaction is initiated with 0.70 mol of N2O4 and 0.35 mol of NO2 in a 1.0 liter container that is heated to 100oC. At equilibrium, how will the amounts of N2O4 and NO2 compare with the initial amounts?
In a large vessel the following reaction is taking place, PCl5(g)⇌PCl3(g)+Cl2(g)PCl_5\left(g\right)\rightleftharpoons PCl_3\left(g\right)+Cl_2\left(g\right) , Kc=4.18×10−2 at 225°CK_c=4.18 \times 10^{-2}\ at\ 225\degree C . I
A lab partner fills an identical vessel with these gases such that the initial concentrations are [PCl5]=0M, [PCl3]=7.2M, and [Cl2]=2.35M Which of the following statement is TRUE?
Does any solid Cu(OH)2 (Ksp =1.6 x 10-19) form when 0.075g of KOH dissolves in 1.0 L of 1 x 10-3 M Cu(NO3)2
Equilibrium: Reaction quotient
Consider the following hypothetical gas-phase reaction: A (g) ⇌ B (g) Kp = 3.40 at 25oC
If a flask initially contains 1.00 atm of each gas, in what direction will the reaction shift in order to reach equilibrium?
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2)
CO(g)+Cl2(g)⇌COCl2(g)CO_{(g)} +Cl_{2(g)} \rightleftharpoons COCl_{2(g)}
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown below:
The graph below shows the concentration of reactants and products for an unknown chemical reaction.
Which of the following statements are correct
i. Q < K at point A
For the reaction N2H4(g) ⇌ N2(g) + 2 H2(g), Kc = 0.026 at 200 K. If we place 2.0 M of N2H4(g), 0.80 M of H2(g), and 3.5 M of N2(g) in a closed vessel, in which way will the reaction proceed to reach equilibrium?
A graduate student sets up an equilibrium demonstration by placing NO2 and N2O4 in flask. These species are in equilibrium with eachother as shown below. Initially the reaction quotient, Q is equal to 3.5, we know that for this reaction K = 1.1 We would predict that,
2 NO2(g)⇌N2O4(g)2\ NO_{2(g)}\rightleftharpoons N_2O_{4(g)}
Equilibrium: Reaction quotient
The system: H2(g) + X2(g) : 2 HX(g) has a value of 24.4 for Kc. A system being studied in a 3.00 liter reactor was charged with 0.150 moles of H2, 0.150 moles of X2, and 0.600 moles of HX. A catalyst was introduced using a remote unit. Which statement below describes the situation
Consider the following reaction to answer the next two questions:
4Cr(s)+3CCl4(g)⇄4CrCl3(g)+3C(s)        ΔH=26.9kJ4Cr(s)+3CCl_4(g) \rightleftarrows 4CrCl_3(g) +3C(s)\ \ \ \ \ \ \ \ \Delta H=26.9kJ
Which of the following statements regarding the reaction quotient Qc and the equilibrium constant Kc is true?
Equilibrium: Reaction quotient
For the equilibrium process N2O4 (g) ⇌ 2 NO2 (g), Kc = 0.212 at 100oC. If a reaction is initiated with 0.70 mol of N2O4 and 0.35 mol of NO2 in a 1.0 liter container that is heated to 100oC. At equilibrium, how will the amounts of N2O4 and NO2 compare with the initial amounts?
Equilibrium: Reaction quotient
A reaction vessel is prepared by putting 0.2 mol of H2S (g) and 0.05 mol of NH3 (g) into a sealed 1.0 L vessel containing 0.05 mol of ammonium hydrosulfide. Based on the reaction given below, will there be a change in the amounts of ammonium hydrosulfide in the flask after waiting for some time?
𝑁𝐻4𝐻𝑆(𝑠)⇌𝐻2𝑆(𝑔)+𝑁𝐻3(𝑔)𝐾𝐶=0.11𝑁𝐻_4𝐻𝑆 (𝑠) ⇌𝐻_2𝑆 (𝑔)+𝑁𝐻_3 (𝑔) \qquad𝐾_𝐶=0.11
Equilibrium: Using The Reaction Quotient
Silver chloride will react with acetic acid to form the complex ion silver acetate. A reaction mixture is prepared by adding 0.25 g of AgCl to a 1.25 L solution that already contains 4.6×10‐6 M Ag(CH3COO)(aq), 2.3×10‐3 M Cl-, 1.1×10‐8 M H+, and 0.010 M CH3COOH. Based on this information, which of the statements below is true?
AgCl(s)+CH3COOH(aq)⇌Ag(CH3COO)(aq)+Cl−(aq)+H+(aq)K=5.87×10−16AgCl(s)+CH_3 COOH(aq)⇌Ag(CH_3 COO)(aq)+Cl^- (aq)+H^+ (aq)\qquad K = 5.87×10^{-16}
After allowing this solution to rest for some time:
Equilibrium: Calculating Equilibrium Concentrations
Iodine chloride (ICl) can decompose, forming iodine and chlorine gases. If a reaction vessel is prepared by filling a 5.00 L container with 0.500 mol each of ICl, I2, and Cl2.
2ICl(g)⇌I2(g)+Cl2(g)KC=0.110 (at 25°C)2ICl(g)⇌I_2 (g)+Cl_2 (g)\qquad K_C = 0.110\ (at \ 25°C)
a) In which direction will the reaction proceed (towards products or reactants)? Show how you determined your answer.
Consider the reaction: A+2B⇌C+DA+2B\rightleftharpoons C+D
At a particular temperature this reaction is reactant-favoured at equilibrium. If for the current concentrations the forward reaction is favoured, which of the following statements is true?
Chemical Equilibria
Consider this balanced chemical reaction and the molecular representation for both of the next two questions: 2AB(g)⇌A2(g)+B2(g)2AB(g)⇌A_2(g)+B_2(g)
For the following isomerization reaction between butane and isobutane, which statement best describes the system at time 2?
Equilibrium: Reaction Quotient
At 425 °C, Kp = 4.18 x 10-9 for the reaction:
2HBr(g)↔H2(g)+Br2(g)2HBr_{(g)}\leftrightarrow H_{2(g)}+Br_{2(g)}
In one experiment 0.20 atm of HBr, 0.100 atm of H2 and 0.010 atm of Br2 are placed in a container. Is the reaction at equilibrium? If not, in which direction will it proceed?