Practice ProblemBUILD
Which of the following equilibrium expressions corresponds to a
(a)
(b)
(c)
(d)
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- Consider the following equilibrium: 2HF(g)⇌H2(g)+F2(g) At equilibrium, the concentration of hydrogen fluoride gas, hydrogen gas, and fluorine gas are 2.04 mol/L, 2.47 mol/L, and 1.89 mol/L. What is the value of the equilibrium constant? Answer to 3 decimal places.arrow_forwardGiven that K c of the reaction below is 2.2 × 10-3 at a certain temperature, which of the following statements is correct? 2ICl (g) ⇄ I2 (g) + Cl2 (g) View Available Hint(s) Given that K c of the reaction below is 2.2 × 10-3 at a certain temperature, which of the following statements is correct? 2ICl (g) ⇄ I2 (g) + Cl2 (g) A. At this temperature, the products are favored and equilibrium lies to the left. B. At this temperature, the reactants are favored and the equilibrium lies to the right. C. At this temperature, the products are favored and the equilibrium lies to the right. D. At this temperature, the reactants are favored and the equilibrium lies to the left.arrow_forwardSuppose you are given the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas B, the value of K: Select one: a. increases, because by adding A more products are made, increasing the product to reactant ratio b. does not change, as long as the temperature is constant c. depends on whether the reaction is endothermic or exothermic d. does not change, because A does not figure into the product to reactant ratio e. decreases, because A is a reactant so the product to reactant ratio decreasesarrow_forward
- The following reaction is at equilibrium: CH4 + 2 Cl2 ⇌ CH2Cl2 + 2 HCl If the partial pressures are: CH4 = 0.250 bar, Cl2 = 0.150 bar, and CH2Cl2 = 0.175 bar at equilibrium, what is the partial pressure of HCl at equilibrium if the K is 2.30? Question options: 0.356 0.272 0.007 0.391arrow_forwardReaction of nitrogen and hydrogen in the presence of a catalyst produces ammonia: N2 + 3H2 2NH3 , rHo = -92 kJ mol-1 . What would increase equilibrium concentration of the product in the mixture? A) Increase pressure, keep temperature constant B)Increase temperature, keep pressure constant C) Decrease pressure, keep temperature constant D) Information is insufficient for answerarrow_forwardThe following system was set up and allowed to come to equilibrium: 2 NO2(g) ⇌ N2O4 At equilibrium, the concentration of nitrogen dioxide was 2.45 mol/L, and the value of the equilibrium constant for the reaction at that temperature is 0.835. What was the concentration of the dinitrogen tetraoxide? Answer in mol/L to 3 decimal places.arrow_forward
- Given the following reaction:XBO3(s) <--> XO(s) + BO2(g) If the concentration of BO2 at equilibrium was 2.0 M, what is the equilibrium constant (K)? Group of answer choices 1.0 M 0.50 M 2.0 M Not enough information is givenarrow_forwardWhat’s the equilibrium constant (K), for the following equation, if you have at equilibrium 0.25 mol/L of NH3 , 1.516 mol/L of H2 and 0.505 mol/L of N2 when it comes to equilibrium? 2 NH3(g)à 3 H2(g)+ N2(g) Table NH3 H2 N2 Initial 1.261 M 0 M 0 M Change -2x +3x +x Equilibrium 0.25 M 1.516M 0.505Marrow_forwardFor the equilibrium: COCl2(g) ↔ CO(g) + Cl2(g) , the equilibrium constant is 2X10-5 If the initial concentration of COCl2 is 21.5X10-3M, calculate the concentration of CO at equilibrium. Answer may be in decimal form (e.g. 0.00325) or exponent form (e.g. 3.25E-3).arrow_forward
- For the following reaction, If the equilibrium concentrations are B = 1.8 M and C = 0.92 and Kc = 1.8 what is the equilibrium concentrwtion of the A report answer in two significant figuresarrow_forwardCarbon monoxide and hydrogen react according to the following equation: CO (g) + H2 (g) CH4 (g) + H2O (g) When 1.00 mol of CO and 3.00 moles of H2 are placed in a 10.0 L container at 927 ° C (1200 K) and allowed to reach equilibrium, the mixture is found to have 0.363 moles of H2O What is the molar composition (that is, how many moles) of H2 are present in the equilibrium mixture? Answer:arrow_forwardWhich of the following does not represent a homogeneous equilibrium? [Select all that apply] Group of answer choices N2O4 (g) ⇄ 2 NO2 (g) N2 (g) + 3 H2 (g) ⇄ 2 NH3 (g) CaCO3 (s) ⇄ CaO (s) + CO2 (g) H2 (g) + I2 (g) ⇄ 2 HI (g) Co (s) + 2H+ (aq) ⇄ Co2+ (aq) + H2 (g)arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning