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Question 1 --> 2NH3 Determine the correct mole ratios based on the following reaction: N2 +...
Question 3 Based on the following reaction. If you have 14.0g of H2, how many grams of NH3 could you produce? N2 + 3H2 --> 2NH3 O 52.5g NH3 O 78.7g NH3 O 472g NH3 O 17.0g NH3
For the reaction 3H2(g) + N2(g) =2NH3(8), Keq = 0.297 at 700K. If [H2] = [N2] - [NH3) = 1.62 Mat 700K, which one of the following is correct? (NH3) increases as the system approaches equilibrium. [H2] and [N2] increase as the system approaches equilibrium. [N]) and (NH3) increase as the system approaches equilibrium. [H2) and (NH3) decrease as the system moves toward equilibrium.
Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H) Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in a decrease in the concentration of NH3 (8) a decrease in the concentration of H2(g) an increase in the value of the equilibrium constant a lower partial pressure of N2 removal of all of the H2(g)
Nitrogen and hydrogen can react to form ammonia. N2(g)+3H2(g)→2NH3(g) 1. Choose ratios showing the relationships between moles of each of the reactants and products in the reaction. Multiple choice, which one? A. 2 mol N2 : 2 mol H2 : 3 mol NH3 B.1 mol N2 : 1/3 mol H2 : 1/2 mol NH3 C. 1 mol N2 : 1 mol H2 : 1 mol NH3 D. 1 mol N2 : 3 mol H2 : 2 mol NH3 2. How...
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.
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.
3. For the reaction, N2 + 3H2 → 2NH3 What is the maximum number of moles of NH3 which could be formed from 12.26 mol of N2 and 2.11 mol of H2?
QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
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: 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?