![QUESTION 11 BE [CLO-5] The following equilibria were attained at 823 K 1. COO (s) + H2 (g) Co(s) + H20 (g) Kc1 = 67 2. Co (s)](http://img.homeworklib.com/questions/33a8fe50-d77e-11ea-97cb-13eceaadd3e8.png?x-oss-process=image/resize,w_560)
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QUESTION 11 BE [CLO-5] The following equilibria were attained at 823 K 1. COO (s) +...
Question: 1 For the following exothermic reaction system at equilibrium: CO2(g)H2(g) H20(g)CO(g) Choose the changes that...
Question: 1 For the following exothermic reaction system at equilibrium: CO2(g)H2(g) H20(g)CO(g) Choose the changes that will increase the value of K Add a catalyst (constant T) Remove H2(g) (constant T) Add CO2(g) (constant T) Decrease the temperature Increase the temperature Decrease the volume (constant T) Add H20(g) (constant T) Submit Show Hints MAIN QUESTION
Thank you Question 5: (1 point) At 390 K, the equilibrium constant, K., for the reaction...
Thank you
Question 5: (1 point) At 390 K, the equilibrium constant, K., for the reaction below is 1.8 x 10-?. PCIs (g) - PC1; (g) + Cl2 (g) Assume a quantity of PCIs (g) is placed in a rigid 10 L vessel and the system is allowed to reach equilibrium at a constant temperature of 390 K. Identify whether each of the following statements is true or false. At equilibrium, if the vessel contains I mole of PCs (g)...
answ 10. 11, 12 xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Wh...
answ 10. 11, 12
xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Which of the of the following changes in condition will cause the equilibrium to shift to the right? (3 pts) (A) add Fe (B) removeCO ( C M CO (D) raise the temperature . Calculate the equilibrium copcentrations of land lat 700 K in a vessel that contains initial concentration of HI -0.36 M. The equilibrium...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO s)+ SO2(8)+ 02(g CH,COO (aq) + H20 (aq) C H,COOH(aq) + H2O(I) 2) The reaction 2HBr(g) H2(g)+ Br2(g) has a Ke value of 1.05 at 25°C. If [HBr] = 0.177 M, [H] 0.223 M and [Br] =0.111 M, in which direction will the system shift?
question #14 13. Which of the following will cause the value of the rate constant, k,...
question #14
13. Which of the following will cause the value of the rate constant, k, for the reaction (A + 2B → C) to increase? a) increasing concentration of A b) increasing concentration of B c) increasing concentration of C d) increasing temperature e) all will cause the value of the rate constant to increase 4. The equilibrium constant, Kc, for the reaction (H2O(g) + CO(g) → H2(g) + CO2(g)) is 1.20 X 10'. What is the equilibrium constant...
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) +...
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
1. For the following balance: 2 HF (g) H2 (g) + F2 (g) 73Kcal Indicate what...
1. For the following balance: 2 HF (g) H2 (g) + F2 (g) 73Kcal Indicate what will happen with each of the following changes: a) Decrease in HF concentratiorn b) Increase in temperature c) Decrease in pressure d) Increase in H2 concentration ej Increase in the concentration of F2 2. At 130 oc the sodium bicarbonate, NaHCO3, decomposes partially according to the following equilibrium: 2 NaHCO3 (s) sNa2CO3 (s) + CO2 (g)+ H20 (g) Ko= 6.25. 100 g of NaHCO3...
3.(12pts) The reaction Cl(aq) + HS(a) determined DRL S)+(aq) +2 Cl(aq) has the experimentally rate k[Cl2][H2S]...
3.(12pts) The reaction Cl(aq) + HS(a) determined DRL S)+(aq) +2 Cl(aq) has the experimentally rate k[Cl2][H2S] Which of the following mechanisms is(are) consistent with the experimental results. Mech I Mech 11, Mech III Cl2 +H2S >H CI CI+HS (slow) CI+ + HS. …>H+ + Cl. + S H2S = HS. + H+ HSCl2 2CI +S+H (fast) (fast equil) (slow) H2S HS+H (fast equil) (fast equil) (slow) 4. (10 pts) Write the equilibrium constant Ke expression for the following 4 KO:(s)...
3. Please use the rules for manipulating K above to answer the following questions. a) At...
3. Please use the rules for manipulating K above to answer the following questions. a) At 303 Kelvin, the equilibrium constant for the gas phase reaction of N, and Hą to form NH, is 2.8 x 10 What is the equilibrium constant for the decomposition of ammonia at the same temperature to produce hydrogen and nitrogen? Kreverse = Kforward 2.8x10-9 = 357142857.1 3.5x10 b) At 1000 Kelvin, the reaction Na(g) + 3H2(g) + 2NH3(g) has a kc value of 2.4...
1. Define the following terms: a. Activation Energy b. Exothermic Reaction 2. Explain what Le Chatelier's...
1. Define the following terms: a. Activation Energy b. Exothermic Reaction 2. Explain what Le Chatelier's Principle states False True False 3. According to Collision Theory, surface area is directly related to reaction rate True 4. According to Collision Theory, reaction temperature is indirectly related to reaction rate 5. Determine the equilibrium constant K for the following reaction: H+ (aq) + OH(aq) = H20 (1) Keg 6. Determine the value of Key for the reaction CH4 (g) + 2H S(g)...
Question: 1 For the following exothermic reaction system at equilibrium: CO2(g)H2(g) H20(g)CO(g) Choose the changes that will increase the value of K Add a catalyst (constant T) Remove H2(g) (constant T) Add CO2(g) (constant T) Decrease the temperature Increase the temperature Decrease the volume (constant T) Add H20(g) (constant T) Submit Show Hints MAIN QUESTION
Thank you
Question 5: (1 point) At 390 K, the equilibrium constant, K., for the reaction below is 1.8 x 10-?. PCIs (g) - PC1; (g) + Cl2 (g) Assume a quantity of PCIs (g) is placed in a rigid 10 L vessel and the system is allowed to reach equilibrium at a constant temperature of 390 K. Identify whether each of the following statements is true or false. At equilibrium, if the vessel contains I mole of PCs (g)...
answ 10. 11, 12
xide ones are reduced to installe r e reaction with carbon monoxide Fe(s) + CO (8) Fe(s) + CO2 () Which of the of the following changes in condition will cause the equilibrium to shift to the right? (3 pts) (A) add Fe (B) removeCO ( C M CO (D) raise the temperature . Calculate the equilibrium copcentrations of land lat 700 K in a vessel that contains initial concentration of HI -0.36 M. The equilibrium...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO s)+ SO2(8)+ 02(g CH,COO (aq) + H20 (aq) C H,COOH(aq) + H2O(I) 2) The reaction 2HBr(g) H2(g)+ Br2(g) has a Ke value of 1.05 at 25°C. If [HBr] = 0.177 M, [H] 0.223 M and [Br] =0.111 M, in which direction will the system shift?
question #14
13. Which of the following will cause the value of the rate constant, k, for the reaction (A + 2B → C) to increase? a) increasing concentration of A b) increasing concentration of B c) increasing concentration of C d) increasing temperature e) all will cause the value of the rate constant to increase 4. The equilibrium constant, Kc, for the reaction (H2O(g) + CO(g) → H2(g) + CO2(g)) is 1.20 X 10'. What is the equilibrium constant...
Write the expressions for Kp for the following reactions: 1. a) 2NH3(g) + Co2(g) N2CH40(s) + H20 (I) b) CuO (s) + H2(g) Cu(l)+H20 (g) 2. At room temperature, a 1.5 L flask contains 3.0 moles of Cl, 0.5 mole of NOCI, and 4.0x10 mole of NO. Calculate Ke at this temperature for the following reaction: 2NO (g) + Cl2(g) 2NOCİ (g) 0.00245 M, does this represent a system at M, [No] 0.2 M and [Ch] If [NOCI] 2.0x 10...
1. For the following balance: 2 HF (g) H2 (g) + F2 (g) 73Kcal Indicate what will happen with each of the following changes: a) Decrease in HF concentratiorn b) Increase in temperature c) Decrease in pressure d) Increase in H2 concentration ej Increase in the concentration of F2 2. At 130 oc the sodium bicarbonate, NaHCO3, decomposes partially according to the following equilibrium: 2 NaHCO3 (s) sNa2CO3 (s) + CO2 (g)+ H20 (g) Ko= 6.25. 100 g of NaHCO3...
3.(12pts) The reaction Cl(aq) + HS(a) determined DRL S)+(aq) +2 Cl(aq) has the experimentally rate k[Cl2][H2S] Which of the following mechanisms is(are) consistent with the experimental results. Mech I Mech 11, Mech III Cl2 +H2S >H CI CI+HS (slow) CI+ + HS. …>H+ + Cl. + S H2S = HS. + H+ HSCl2 2CI +S+H (fast) (fast equil) (slow) H2S HS+H (fast equil) (fast equil) (slow) 4. (10 pts) Write the equilibrium constant Ke expression for the following 4 KO:(s)...
3. Please use the rules for manipulating K above to answer the following questions. a) At 303 Kelvin, the equilibrium constant for the gas phase reaction of N, and Hą to form NH, is 2.8 x 10 What is the equilibrium constant for the decomposition of ammonia at the same temperature to produce hydrogen and nitrogen? Kreverse = Kforward 2.8x10-9 = 357142857.1 3.5x10 b) At 1000 Kelvin, the reaction Na(g) + 3H2(g) + 2NH3(g) has a kc value of 2.4...
1. Define the following terms: a. Activation Energy b. Exothermic Reaction 2. Explain what Le Chatelier's Principle states False True False 3. According to Collision Theory, surface area is directly related to reaction rate True 4. According to Collision Theory, reaction temperature is indirectly related to reaction rate 5. Determine the equilibrium constant K for the following reaction: H+ (aq) + OH(aq) = H20 (1) Keg 6. Determine the value of Key for the reaction CH4 (g) + 2H S(g)...
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