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Please fill out the answer table for questions (1-5) on page 2. 1. Consider the reaction...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u IIULS reaction: CÓ (g) + 3 H (g) + CH4 (g) + H2O (G) 1. At 25°C, Keq=4.0. What must be the Co] at equilibrium If the equilibrium concentrations of [H.]= 2.0M. (CH) = 5.0M, and (HO) = 3.OM? Answer: 0.469 M The ICE table is a way to keep track of what is happening in the reaction vessel. The initial concentrations if given...
please answer all. thank u Equm U ving reaction for Questions 1 - 3 and answer the questions based upon th sed upon...
please answer all. thank u
Equm U ving reaction for Questions 1 - 3 and answer the questions based upon th sed upon this Consider the following reaction reaction: co (g) + 3 H, (g) + CH (9) + H2O (g) 1. At 25°C. Kega 4.0. What must be Kes 4.0. What must be the coat equilibrium If the rulibrium concentrations on HJE 2.0M, (CH) = 5.OM, and [HO] - 3.OM? Answer: 0.469 M a way to keep track of...
Consider the following reaction at equilibrium. What will happen if SO2 is added to the reaction?...
Consider the following reaction at equilibrium. What will happen if SO2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) A.) The equilibrium will change in the direction of the products. B.) The equilibrium constant will increase. C.) The equilibrium will change in the direction of the reactants. D.) The equilibrium constant will decrease. E.) No change in equilibrium is observed.
Consider the following reaction at equilibrium. What will happen if O2 is added to the reaction?...
Consider the following reaction at equilibrium. What will happen if O2 is added to the reaction? 4FeS2(s) + 11O2(g) <--> 2Fe2O3(s) + 8SO2(g) A) The equilibrium constant will increase. B) The equilibrium will change in the direction of the reactants. C)The equilibrium will change in the direction of the products. D)No change in equilibrium is observed. E)The equilibrium constant will decrease. 2- Identify the change that will always shift the equilibrium to the right. 2SO2(g) + O2(g) ⇋ 2SO3(g) A)...
1) The reaction below is exothermic 2SO2 (g) + O2(g) = 2803(g) + heat Le Châtelier's...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
not sire if im right or wrong? Consider the following reaction at equilibrium. What will happen...
not sire if im right or wrong?
Consider the following reaction at equilibrium. What will happen if Fes, is removed from the reaction? 4 FeS (s) + 11 O2(g) = 2 Fe,0,(s) + 8 SO,(9) looo The equilibrium constant will increase. The equilibrium will change in the direction of the reactants. The equilibrium will change in the direction of the products. No change in equilibrium is observed. The equilibrium constant will decrease.
Question 5 0/1 point The equilibrium constant for the gas phase reaction N2 (g) + 3H2(g)...
Question 5 0/1 point The equilibrium constant for the gas phase reaction N2 (g) + 3H2(g) + 2NH3 (B) is Keq - 4,34 x 10-3 at 300 °C. At equilibrium, Question 5 The equilibrium constant for the gas phase reaction N2 (8) + 3H2 (g) – 2N63 (g) is keq = 4.34 x 10-3 at 300 °C. At equilibrium, products predominate only reactants are present roughly equal amounts of products and reactants are present only products are present reactants predominate
A reaction that has a positive AH and a positive AS will be spontaneous at high...
A reaction that has a positive AH and a positive AS will be spontaneous at high temperatures spontaneous at low temperatures spontaneous at all temperatures nonspontaneous at all temperatures QUESTION 6 Which of the following statements is FALSE? Keg for a reaction written in reverse is the reciprocal of the key for the forward reaction A reaction quotient (Q) larger than Keq means that the reaction will shift toward reactants Chemical equilibrium indicates that reactants and products are present in...
1) the photosynthetic conversion of co2 to o2 can be represented by 6co2 + 6h2o <>c6h12o6+6o2...
1) the photosynthetic conversion of co2 to o2 can be represented by 6co2 + 6h2o <>c6h12o6+6o2 what is the equilibrium expression for this reaction? 2) what is the state of the system if I2=1.0 M and I=1.0×10^-3 M I2 <>2I. kc=3.8×10^-5 a. the system is at equilibrium b. the system is at a steady state c. the system is not at equilibrium and will produce more reactants d. the system is not at equilibrium and will produce more products 3)...
Chemistry QB14.32 Level 2 х Question The reaction 2 C[math]_{2}[/math]H[math]_{6}[/math](g) + 5 O[math]_{2}[/math](g) [math]\leftrightharpoons[/math] 4 CO(g)...
Chemistry QB14.32 Level 2
х Question The reaction 2 C[math]_{2}[/math]H[math]_{6}[/math](g) + 5 O[math]_{2}[/math](g) [math]\leftrightharpoons[/math] 4 CO(g) + 6 H[math]_{2}[/math]O(g) has [math]\Delta[/math]H[math]^{0}_{rxn}[/ma<0. Determine for each indicated change whether the reactant(s) or product(s) concentrations will [math]\textbf[increase}[/math] or [math]\textbf{not change}[/math] when the reaction reestablishes equilibrium. Your answers must be [math]\textbf{reactants}[/math], [math]\textbf{products}[/math], or [math]\textbf(not change}[/math). Increase the C[math]_{2}[/math]H[math]_{6}[/math] partial pressure. Increase the O[math]_{2}/math] concentration Decrease the CO partial pressure. Add 2.0 moles of H[math]_{2}[/math]o. Decrease the reaction vessel volume. Add a catalyst to the...
Consider the following reaction for Questions 1.3 and answer the questions based upon this GU u IIULS reaction: CÓ (g) + 3 H (g) + CH4 (g) + H2O (G) 1. At 25°C, Keq=4.0. What must be the Co] at equilibrium If the equilibrium concentrations of [H.]= 2.0M. (CH) = 5.0M, and (HO) = 3.OM? Answer: 0.469 M The ICE table is a way to keep track of what is happening in the reaction vessel. The initial concentrations if given...
please answer all. thank u
Equm U ving reaction for Questions 1 - 3 and answer the questions based upon th sed upon this Consider the following reaction reaction: co (g) + 3 H, (g) + CH (9) + H2O (g) 1. At 25°C. Kega 4.0. What must be Kes 4.0. What must be the coat equilibrium If the rulibrium concentrations on HJE 2.0M, (CH) = 5.OM, and [HO] - 3.OM? Answer: 0.469 M a way to keep track of...
not sire if im right or wrong?
Consider the following reaction at equilibrium. What will happen if Fes, is removed from the reaction? 4 FeS (s) + 11 O2(g) = 2 Fe,0,(s) + 8 SO,(9) looo The equilibrium constant will increase. The equilibrium will change in the direction of the reactants. The equilibrium will change in the direction of the products. No change in equilibrium is observed. The equilibrium constant will decrease.
Question 5 0/1 point The equilibrium constant for the gas phase reaction N2 (g) + 3H2(g) + 2NH3 (B) is Keq - 4,34 x 10-3 at 300 °C. At equilibrium, Question 5 The equilibrium constant for the gas phase reaction N2 (8) + 3H2 (g) – 2N63 (g) is keq = 4.34 x 10-3 at 300 °C. At equilibrium, products predominate only reactants are present roughly equal amounts of products and reactants are present only products are present reactants predominate
A reaction that has a positive AH and a positive AS will be spontaneous at high temperatures spontaneous at low temperatures spontaneous at all temperatures nonspontaneous at all temperatures QUESTION 6 Which of the following statements is FALSE? Keg for a reaction written in reverse is the reciprocal of the key for the forward reaction A reaction quotient (Q) larger than Keq means that the reaction will shift toward reactants Chemical equilibrium indicates that reactants and products are present in...
Chemistry QB14.32 Level 2
х Question The reaction 2 C[math]_{2}[/math]H[math]_{6}[/math](g) + 5 O[math]_{2}[/math](g) [math]\leftrightharpoons[/math] 4 CO(g) + 6 H[math]_{2}[/math]O(g) has [math]\Delta[/math]H[math]^{0}_{rxn}[/ma<0. Determine for each indicated change whether the reactant(s) or product(s) concentrations will [math]\textbf[increase}[/math] or [math]\textbf{not change}[/math] when the reaction reestablishes equilibrium. Your answers must be [math]\textbf{reactants}[/math], [math]\textbf{products}[/math], or [math]\textbf(not change}[/math). Increase the C[math]_{2}[/math]H[math]_{6}[/math] partial pressure. Increase the O[math]_{2}/math] concentration Decrease the CO partial pressure. Add 2.0 moles of H[math]_{2}[/math]o. Decrease the reaction vessel volume. Add a catalyst to the...
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