Equilibrium Stoichiometry

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• When a sample of NO(g) (11.75 mol) is placed in 440.0 L reaction vessel at 882.0 K and allowed to come to equilibrium the mixture contains 79.86 grams of N2(g). What is the concentration (mol/L) of N2(g)?
• A 23.0 g sample of I2(g) is sealed in a gas bottle having a volume of 500 mL. Some of the molecular I2(g) dissociates into iodine atoms and after a short time the following equilibrium is established. I2(g-->2I(g) For this system, Kc= 3.80 x 10^-5. What mass of I2(g) will be in the bottle when equilibrium is established?
• A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the partial pressure of nitrogen in the mixture.
• A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the value of the equilibrium constant, Kp for the system at 800C?
• A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the Gibbs free energy change, delta G, for the reaction at 800C?
• A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What will be the sign of the change in entropy, delta S, for the reaction?
• What is the stoichiometric equation corresponding to the equilibrium mass action expression given below?
• PCl3(g) + Cl2(g) <---> PCl5(g) Kc = 0.18 In an initial mixture of 0.300M PCl3 (g), 0.400M Cl2 (g), what are the equilibrium concentrations of all gases?
• Consider the equilibrium: 2N2O (g) + O2 (g) = 4NO (g) 3.00 moles of NO (g) are introduced into a 1.00 liter evacuated flask. When the system comes to equilibrium, 1.00 moles of N2O (g) has formed. What are the equilibrium concentrations of each substance? What is Kc for the reaction?
• Considering the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) If a solution is made containing initial [SO2Cl2]= 0.021M, at equilibrium, [Cl2]= 1.3×10−2M. What are the equilibrium concentrations of SO2Cl2 and SO2?
• At some temperature, a 100-L reaction vessel contains a mixture that is initially 1.0 mol Co and 2.0 mol H2. The vessel also contains a catalyst so that the following equilibrium is attained: CO(g) + 2H2(g) <--> CH3OH(g) At equilibrium, the mixture contains 0.100 mol CH3OH. In a later experiment in the same vessel, you start with 1.0 mol CH3OH. How much methanol is there at equilibrium?
• At 25°C in a closed system, ammonium hydrogen sulfide exists as the following equilibrium. NH4HS(s)<--->NH3(g) + H2S(g) When a sample of pure NH4HS(s) is placed in an evacuated reaction vessel and allowed to come to equilibrium at 25°C, total pressure is 0.660 atm. What is the value of Kp?
• A mixture initially contains A, B, and C in the following concentrations: [A]=0.550 M, [B]=1.05 M, [C]=.550 M. The following reaction occurs and equilibrium is established: A+2B <-> C At equilibrium, [A]=.390 M and [C]=0.710 M. What is the value of the equilibrium constant, Kc?
• Considering the following reaction: CO(g) + 2 H2(g) --> CH3OH(g) Suppose that the initial concentrations of the reactants are [CO] = 0.500 M and [H2] = 1.00 M. Assuming that there is no product at the beginning of the reaction and that at equilibrium [CO] = 0.15 M, what is the equilibrium constant at this new temperature?
• Considering H2(g) + I2(g) ↔ 2HI and temperature = 731K, 1.20 mol of H2 and 1.20 mol of I2 are placed in a 1.00 L vessel. What is the equilibrium concentration of I2 in the gaseous mixture? The equilibrium constant is K = 49.0
• Hydrogen sulfide decomposes according to the following reaction, for which Kc=9.30E-8 at 700 degrees Celsius. 2 H2S(g) --> 2 H2(g) + S2(g) If 0.29 moles of H2S is placed in a 3.0-L container, What is the equilibrium concentration of H2(g) at 700 degrees Celsius?
• Considering H2(g) + I2(g) ↔ 2HI and a temperature of 731K; 2.40 mol of H2 and 2.40 mol of I2 are placed in a 1.00 L vessel. What is the equilibrium concentration of H2 in the gaseous mixture? The equilibrium constant is K = 49.0
• Question #438d8
• In an experiment, 0.200 mol H2 and 0.100 mol I2 were placed in a 1.00 L vessel where the following equilibrium was established: H2 + I2 <-----> 2HI For this reaction, Kc = 49.5, What were the equilibrium concentration for H2, I2 and HI?
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• 1. For the reaction, #PCl_(3(g))+Cl_(2(g)) rightleftharpoons PCl_(5(g))#, #K_c = 96.2 # at 400 K. If the initial concentrations are 0.22 mol/L of #PCl_3# and 0.42 mol/L of #Cl_2#, what are the equilibrium concentrations of all species?
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• For the reaction #NH_4HS_((s)) rightleftharpoons NH_(3(g)) + H_2S_((g))#, #K_c = 1.2*10^(-4)# at 491K. What concentration of #NH_3# will be present at equilibrium if a sample of #NH_4HS# is placed in a vessel at 491K?
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• Using the following reaction: C10H15ON(aq) +H20(l) = C10H15ONH+ (aq) + OH- (aq), a 0.035M solution of ephedrine has a pH of 11.33, how would you calculate the equilibrium concentrations of C10H15ON(aq), C10H15ONH+ (aq),and OH- (aq)?
• What are the products to #C_2H_6(g) + O_2(g)#?
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• Question #19cd0
• In a 10 litre evacuated chamber, 0.5 mole of H2 and 0.5 mole I2 gases are reacted to produce HI gas at 445°.the equilibrium constant at this temperature is 50. How many moles of iodine remain unreacted at equilibrium?
• At 27°C ,1atm, 20% of N2O4 dissociated into NO2. Determine the partial pressure of each gas at equilibrium and the equilibrium constant Kp at this temperature(assume that the number of mole of N2O4 before dissociation is 1 mole)?
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• When 46g of I2 and 1g of H2 are heated to equilibrium at 450°C ,the equilibrium mixture contains 1.9g I2. How many moles of each gas present at equilibrium?Determine Kc and Kp for this reaction at the same temperature?
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• Calculate the mass of ethyl acetate formed at 25 C from 1.66 moles of acetic acid and 2.17 moles of ethyl alcohol ? . Kc = 4
• Question #9bbc5
• If we have #"24.9 L"# of liquid ethanol, with a density of #"789 g/L"# at a certain temperature, how many mols do we have?
• Using Raoult's law... and knowing that #A# and #B# form an ideal binary mixture but #R# and #S# have negative deviation...?
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• A mixture of 2.50mol H2, 1.5 mol CS2, 1.5 mol CH4 and 2mol H2S is placed in a 5.0L reaction vessel. When equilibrium is achieved, the concentration of CH4 has become 0.25M. Whay are the number of moles of CS2 at equilibrium?
• A #0.240*mol# quantity of dinitrogen gave #7.8*mol# of ammonia. Does this make sense chemically?
• 3.1 mol of #sf(Fe^(3+)# is mixed with 3.2 mol of #sf(SCN^-)# and allowed to reach equilibrium, after which 3 mol of #sf([Fe(SCN)]^(2+))# is formed. What is the value of #sf(K_c)# ?
• What is the equilibrium equation in chemistry? Is it different from the regular equation?
• What is Kp? What goes on in a Kp equation?
• How do you balance this equation? #Fe(NO_3)_3 + KSCN -> Fe(NO_3)_3 + KSCN#
• What is the chemical equation for the ionization of benzoic acid?
• How do you write the balanced acid equation and the dissociation expression Ka for following compounds in water? a) #H_3PO_4# b) #HClO_2# c) #CH_3COOH# d) #HCO_3^-# e) #HSO_4^-#
• How do you find the equilibrium constant for the reverse reaction of this problem?
• In the following equation: if you add #CH_4# to the mixture which direction does it shift? If you remove #H_2# what direction does it shift? Which way does it shift if you add a catalyst?
• How do you write the chemical equation for the acid-ionization equilibrium of acetic acid in water?
• The dissociation of ethanoic acid is an equilibrium process which is represented by the equation: #HC_2H_3O_2  H^+ + C_2H_3O_2^-# How will this equilibrium be affected if a base (OH-) is added?
• What is #K_(eq)# for the reaction #2SO_3(g) #⇌ #2SO_2(g)# + # O_2 (g)#?
• Can someone explain on how they derived to the answer of 20.0L?
• Is the answer to this question 221 J? If not, can someone explain it to me?
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• 2 moles PCl5 are heated in a 2L flask.At equilibrium 40% PCl5 dissociates . what is the equilibrium constant for this reaction?
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• Calculate the concentration of each species at equilibrium?
• Equilibrium constant question?
• What is the value of Kc here?
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• Question #19979
• What is the net ionic equation for the reaction between hydroiodic acid, and potassium hydroxide?
• Question #fdae0
• Suppose #"2.83 g"# of ammonium chloride solid is placed into a closed, evacuated rigid container, and allowed to decompose at a certain temperature. If 40% of it decomposed into ammonia and hydrogen chloride gas, what is #K_c# for this reaction?
• How does the equilibrium evolve if the pressure of reactants or products are altered?
• What principle states that mass is neither gained or lost during a chemical reaction?
• At #25^@ "C"#, for the reaction #"N"_2"O"_4(g) rightleftharpoons 2"NO"_2(g)#, the equilibrium constant is #K_c = 5.85xx10^(-3)#. #"20.0 g"# of #"N"_2"O"_4# were added to a #"5.00-L"# container. What is the molar concentration of #"NO"_2# at equilibrium?
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• Given the reaction...#SO_2(g) + NO_2(g) rightleftharpoons SO_3(g) + NO(g)#...for which #K_"eq"=3.75#, what will be the equilibrium concentrations of products and reactants?
• Question #26e77
• How can one tell a reaction has reached equilibrium?
• How can one tell a reaction has reached equilibrium?
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• What is the concentration of ammonium ion in a solution of #NH_3(aq)# that is nominally #0.157*mol*L^-1#?