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Consider this reaction: N2(g) + 3H2(g) - 2NH3(g). Based on initial conditions, a student predicts that...
Question 19 of 2 Question 19 Consider this reaction: N2(g) + 3H2(g) + 2NH3(g). Based on initial conditions, a student predicts that the direction of the reaction proceeds to the left. How would you write the change of NH3 in your ICE table? 4 points +x O-X 2x O-2x +3x 0 -3x Questi Question 24 & points Compare the acid strength between two molecules by completing each of the two sentences below. Use the drop down. HBrO is a than...
Consider this reaction: 3H2(g) + N2(g) --> 2NH3(g) First, if 5.00 g of H2 is reacted with 21.0 g of N2 determine the identity of the limiting reactant. Second, what theoretical mass of product NH3 would be produced?
Consider the following reaction at equilibrium: (AH° = +92.4kJ) 2NH3(g) = N2(g) + 3H2(0) Le Chateliers Principle predicts that the moles of H2(g) in the reaction container will increase with Select one: O a. an increase in the volume of the reaction (constant T) O b. some removal of NH3(g) from the reaction vessel (constant V and T) O c. addition of some N2(g) to the reaction vessel (constant V and T) O d. an increase in total pressure by...
A student ran the following reaction in the laboratory at 745 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 3.44x10-2 moles of N2(g) and 5.80x10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 7.82x10-4M. Calculate the equilibrium constant, K., she obtained for this reaction. K=
Consider the chemical reaction 2NH3(g) ó N2(g) + 3H2(g). The equilibrium is to be established in a 50.0 L container at 1,000 K, where Kc = 4.0 × 10-2. Initially, 6.10 x 105 moles of NH3(g) are present. Calculate the amount of H2 presentat equilibrium. [H2] =_____
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...
Consider this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5 x 10^4 at 127 degrees celsius, what is the equilibrium constant, Kp at the same temperature?
The ΔHΔH for the reaction N2(g)+3H2(g)N2(g)+3H2(g) →→ 2NH3(g)2NH3(g) is −123.77kJmol−1−123.77kJmol−1 at 1000 K. The heat capacities of the reactants and products are CP,m=CP,m= 3.502 RR, 3.466 RR, and 4.217 RR for N2(g)N2(g), H2(g)H2(g), and NH3(g)NH3(g), respectively. Calculate ΔHfΔHf of NH3(g)NH3(g) at 500 KK from this information. Assume that the heat capacities are independent of temperature. Express your answer to four significant figures and include the appropriate units.
For the reaction 2NH3(g)<->N2(g)+3H2(g), Kc=0.0076 at a particular temperature. If 0.025 M NH3, 0.50M N2, and 0.015 M H2 are mixed in a reaction vessel, is the reaction at equilibrium? If not, in what direction will the reaction shift to reach equilibrium?
N2(g) + 3H2(g) →2NH3(g) If there is 15.17 g N2 and excess H2 present, the reaction yields 14.7 g NH3. Calculate the percent yield for the reaction.