Practice ProblemCONCEPTUALIZE
Consider a chemical reaction represented by the equation
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Aleks 360 2 Semester Access Card For Chemistry
- Carbon 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_forwardThe reaction shown below has an equilibrium constant value of Kp=5.50 at a certain temperature.CO (g) + Cl₂ (g) ⇄ COCl₂ (g) Kp = 5.50A container is pressurized with CO and Cl₂ until the pressure of CO is 0.450 atm and the pressure of Cl₂ is 0.200 atm. Calculate the pressure of COCl₂ in the container when the system reaches equilibrium.Answer: atm COCl₂arrow_forwardHeating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reactionarrow_forward
- Suppose 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_forwardSolve all part please. Consider the equilibrium reaction N2O4 (g) ⇌ 2 NO2 (g)a. Using appendix C, find H and S for this reaction (you will need this for b,c). delta s= 176.6J delta H=5802kJb. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PNO2 = PN2O4 = 1.0 atm.c. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PT = 10.0 atm and PNO2 = 2 PN2O4.arrow_forward2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g) You have 0.4 moles C2H2 and 0.2 moles O2 present initially in a 5L flask. You allow the reaction to run until it reaches equilibrium. Which of the following is the correct ICE table for this process? Question 5 options: Conc. C2H4 O2 CO2 H2O Initial 0.4 0.2 0 0 Change -x -x +x +x Equil. 0.4-x 0.2-x x x Conc. C2H4 O2 CO2 H2O Initial 0.08 0.04 0 0 Change -2x -5x +4x +2x Equil. 0.08-2x 0.04-5x 4x 2x Conc. C2H4 O2 CO2 H2O Initial 0.4 0.2 0 0 Change -2x -5x +4x +2x Equil. 0.4-2x 0.2-5x 4x 2x Conc. C2H4 O2 CO2 H2O Initial 0.08 0.04 0 0 Change -20x -20x +20x +20x Equil. 0.08-20x 0.04-20x 20x 20xarrow_forward
- Consider the following reaction: CO (g) + H2O (g) <===> CO2 (g) + H2 (g) a. Write the expression for the equilibrium constant (K) of the reaction b. Calculate the value for K using the following concentrations of each substance at equilibrium: [CO) = 0.55 M [H2O) = 0.44 M [CO2) = 0.25 M [H2) = 0.10 M c. Based on the value you obtained for K, are the products or reactants lower in energy? d. Is the value for ΔH negative or positive? please show workarrow_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_forwardAt a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N2O4 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium? (no scientific notation)N2O4(g) ⇄ 2NO2(g)arrow_forward
- At 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25 × 10−4. If [H2S] = 4.80 × 10−3 M and [H2] = 1.40 × 10−3 M, calculate [S2]. Please write to text formet answerarrow_forwardTopic: The state of the EquilibriumConsider the given reaction. 2BrF5(g) ⇌ Br2(g) + 5F2(g) If the respective equilibrium concentration of BrF5, Br2, and F2 at 250℃ are 0.046 M, 1.2 M, and 0.93 M, what are the values of Kc and Kp?arrow_forwardThe reaction 2 O3 (g) → 3 O2 (g) (∆H° = -300kJ) is in equilibrium at 25°C. Which of the following statements is correct regarding this reaction if the temperature is increased to 50°C? (Choose one of the options) a. The reaction system will shift to the right to re-establish the equilibrium. b. The equilibrium constant of this reaction will decrease. Options: 1.) a only 2.) b only 3.) both a and b are correct. 4.) neither a nor b is correct.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning