Would
N2 + 3h2 -> 2NH3 + 22Kcal
be considered endothermic or exothermic? and why?
The reaction is said to be exothermic if energy is produced is the reaction.
The reaction is said to be endothermic if energy is required for the reaction.
The given reaction is
N2 + 3 H2 --------> 2 NH3 + 22 kcal
In the above reaction, 22 kcal energy is present on product side. That is 22 kcal is produced in the reaction.
Hence this reaction is exothermic
Would N2 + 3h2 -> 2NH3 + 22Kcal be considered endothermic or exothermic? and why?
pts) The synthesis of ammonia from nitrogen and hydrogen is exothermic N2(g) + 3H2(g) → 2NH3(g) + Heat )If heat is removed, will the forward rate of the reaction increase or decrease? Why? ) If nitrogen gas is added, will the forward rate of the reaction increase or decrease? Why? If the volume of the reaction container is increased, how will this affect the rate of the forward reaction? Why? )
For the following exothermic reaction 3H2(g) + N2(g) ↔ 2NH3(g) + heat. In which direction does equilibrium shift if the temperature of the reaction vessel is raised. Select one: a. Reaction shifts towards products. b. There is no effect. c. reaction shifts towards reactants
Initially in a reaction, N2 + 3H2 = 2NH3, N2 has a concentration of 0.4M, 3H2 has a concentration of 0.4M and 2NH3 has a concentration of 0.3. Calculate the equilibrium concentrations of each substance if Kp is 8.65*10^10 at a temperature of 298k.
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
Consider the reaction: N2(g) + 3H2(g) <---> 2NH3(g) The Gibbs free energy of formation ((delta)Gfo) for ammonia is -16.5 kJ/mol and the reaction is exothermic. Calculate the (delta)Gorxn and the equilibrium constant for the reaction and clearly state whether K increases or decreases with temperature.
If the system 3H2(g) + N2(g) ⇄ 2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached. True or False
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.
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?
Want 2CH4 + 2NH3 ----> 2HCN + 6H2 From: N2+3H2 --->2NH3 DeltaH: -91.8KJ 2H2+C--->CH4 DeltaH: -74.9 KJ 2C+H2+N2----> 2HCN DeltaH: 270.3 KJ
N2(g) + 3H2(g) → 2NH3(g). If 10.0 mol of N2 are added to 10.0mol H2 A. How many moles of NH3 are produced? B. What is the limiting reactant?