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Choose four ways in which the yield of ammonia in the reaction below can be improved...
Nitrogen gas and hydrogen gas can ve converted into ammonia gas as shown in the reaction equation listed below. Answer each of the questions listed below regarding this reaction. 1. Nitrogen gas and hydrogen gas can be converted into ammonia gas as shown in the reaction equation listed below. Answer each of the questions listed below regarding this reaction. N2(g) + 3 H2(g) = 2 NH3(g) AH = -92.2 kJ/mole and K = 2.6 x 108 This reaction is an...
The decomposition of ammonia gas is endothermic, AH = 92 kJ/mol. 2 NH3() = N2(g) + 3H2(g) What change to an equilibrium mixture of this reaction will result in the formation of more hydrogen gas? The addition of a catalyst. An decrease in temperature. An increase in volume. A decrease in the concentration of ammonia.
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced? decreasing the volume adding N2 increasing the volume adding H2 2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced? decreasing the temperature adding H2 increasing the temperature adding N2 3. What is the effect of a...
Which of the following would increase the yield of the products of the following endothermic reaction? 2H2O(g) + 2Cl2(g) 4HCl(g) + O2(g) ΔH > 0 Question 14 options: 1) Decreasing the temperature of the reaction 2) Adding HCl to the reaction vessel 3) Decreasing the volume of the container 4) Removing Cl2(g) from the reaction vessel 5) Increasing the volume of the container
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...
The dissociation of PCl5(g) to PCl3(g) and Cl2(g) is an endothermic reaction. PCl5(g) PCl3(g) + Cl2(g) What is the effect on the position of equilibrium of each of the following changes? a) Compressing the gaseous mixture _________________________________ b) Decreasing the temperature _________________________________ c) Adding Cl2(g) to the equilibrium mixture __________________________________ d) Removing PCl5 (g) from the equilibrium mixture __________________________________
Question 1 Glucose metabolism can be represented by the following chemical reaction: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l) H for the reaction is -2837 kJ/mole. Is this reaction endothermic or exothermic? Write an expression for the equilibrium constant for this reaction. Given that the value of the equilibrium constant is very large, would you expect this reaction to be fast or slow? Explain the effect on equilibrium of Increasing temperature Increasing pressure by decreasing the volume Decreasing concentration of oxygen Increasing the concentration of...
For the equilibrium system below, which of the following would result in an increase in the quantity of PCls(g)? 10. removing some Cl2(8) injecting some He gas d. a. increasing temperature b. increasing the size of the container c. decreasing temperature e. Consider this equilibrium N2(8)+3H2(NHs(8)+94 k] If some nitrogen gas were injected into this system at constant temperature and pressure the system would most likely experience which of the following? a. an increase in [hydrogen) b. a decrease in...
Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N204 is colorless. At High Temperature the red color is strong. || At Low Temperature the gas has less color. If we represent the equilibrium as: 2 NO2(g) = N204(9) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the...
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 1.6 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.56 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.