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What would adding nitrogen do to the reaction? A) shift right B) shift left C) increased...
For the exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + HEAT, which of the following changes could be carried out to cause the reaction to shift to the right? Adding H2 Adding NH3 Increasing the temperature Removing N2
1) Which reaction will shift to the left in response to a decrease in volume? A) 2 SO3 (8) 2 SO2(g) + O2(8) B) N2(g) + 3H2(g) + 2NH3(g) C) 2H1 (8) H2(g) + 12 (8) D) 4 Fe (8) +32(g) 2 Fe2O3 (s) E) H2 (8) + Cl2(g) 2 HCl (g) Explain 2) Based on Le Châtelier's principle, increasing pressure at constant temperature in the following reaction will not change the concentrations of reactants and products. A) N2 (8)...
19)Ammonia is synthesized from nitrogen and hydrogen in the following reaction: N2(g)+3H2(g)2NH3(g) At 500 °C, the equilibrium constant for this reaction is 0.080. Given that (NHa] - 0.0596 M, [N2]- 0.600 M, and [H2] 0.420 M, find Q and predict how the reaction will proceed. a. Q 0.08, the reaction is at equilibrium b. Q 12.5, the reaction will move to the left c. Q 12.5, the reaction will move to the right d. Q 1.34, the reaction will move...
Question #1: Consider the reaction given, How would the reaction shift? Options are no change, right, or left. Question #2: Determine if the above reaction is endothermic or exothermic based on the following information. Is it endothermic or exothermic? Question #3: Explain your reasoning. Consider 2 NBr3() = N2(8) + 3 Br2() How would the reaction shift if: [N2] is decreased: [Br2] is increased: The amount of N Br3 is doubled: The pressure is decreased by changing the volume: The...
QUESTION 5 Which change to this reaction system would cause the equilibrium to shift to the left? N2(g) + 3H2(g) = 2NH3(g) + heat addition of a catalyst removal of NH3(g) addition of H2 (g) cooling the system decreasing the pressure
Determine the effect on the equilibrium for the reaction below when the pressure of NH3 is increased. N2(g) + 3 H2(g) = 2 NH3(g) AH = -91.8 kJ o a. The reaction will shift to the right. b. There will be no change. c. The reaction will shift to the left. Determine the effect on the equilibrium for the reaction below when the volume of the reaction vessel is increased. N2 (€) + 3H2(g) = 2 NH3(g) AH -91.8 kJ...
Ammonia (NH3) is produced by the reaction of nitrogen and hydrogen according to the chemical equation: N2+ 3H2 → 2NH3. What mass of nitrogen is necessary to react completely with 100.0 g of hydrogen?
Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) + 2NH3(g) Calculate the mass of ammonia produced when 33.0 g of nitrogen react with 11.2 g of hydrogen. Which is the excess reactant and how much of it will be left over when the reaction is complete? o hydrogen nitrogen
please show work? Question 38 (8 points) A 50.0 L reaction vessel contains 2.00 mole nitrogen, 3.00 mole hydrogen and 0.500 mole NH3. The mixture is approaching the following equilibrium: N2(g) + 3H2(g) + 2NH3(9) a) Calculate the reaction quotient Q. b) If the value of Kc is 0.500, predict which direction the reaction will go in order to reach equilibrium(to the right, to the left, or no change). Explain your answer.
Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 32.0 g of nitrogen react with 13.5 g of hydrogen. ___________NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? hydrogen or nitrogen ________ g