For the given exothermic reaction, the favorable conditions for the formation of NH3 will be N2...
For the given exothermic reaction, the favorable conditions for the formation of NH3 will be N2 (g) + 3 H2 (g) 2 NH3 (g)
Homework Answers
N2 (g) + 3 H2 (g) -------> 2 NH3 (g) 
H =
-ve for exothermic reaction
The concentration of N2, H2 increases the favor the formation of NH3
At high pressure favor the formation of NH3
The formation of NH3 is forward reaction. It is exothermic reaction. The exothermic reaction takes place at low temperature.
The low temperature is favor the formation of NH3
Low temperature is the favorable conditions for the formation of NH3 will be N2 (g) + 3 H2 (g) 2 NH3 (g)
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For the given exothermic reaction, the favorable conditions for
the formation of NH3 will be N2...
1) a) For the following reaction, the rate of formation of NH3 is 0.020 M/min. N2(g)...
1) a) For the following reaction, the rate of formation of NH3 is 0.020 M/min. N2(g) + 3 H2 (g) → 2 NH3(g) Find the rate of reaction b) For the following reaction, the rate of formation of NH3 is 0.020 M/min. N2(g) + 3 H2 (g) → 2 NH3(g) Find the change in concentration of H2 in the same time interval.
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The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2...
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Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C The value of Kp for this reaction is a. less than ko O b.greater than kc O c equal than ke Consider the reaction: N2 (g)+3 H2 (g)=2 NH3 (g)Kc = 0.0043T = 300 °C Part 1. Given the initial conditions below, which statement is true? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M O a. Q is greater...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following...
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...
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 temp...
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
A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium...
A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.61 M, [H2] = 1.26 M, and [NH3] = 0.30 M. Calculate the equilibrium constant, Kc, if the reaction is represented as ( 1 2 ) N2(g) + ( 3 2 ) H2(g) ⇌ NH3(g)
1. The simplest ammonia formation is from nitrogen and hydrogen. Consider the reversible reaction N2(g) + 3H2(g) → 2NH3(g) The standard enthaply and Gibbs free energy of formation one mole NH3 is ∆H◦...
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5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
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