Question

for the equation shown below, use le chatelier’s principle to identify if the changes indicated will cause the reaction to a) shift left, b) shift right, c) have no change, or d) no way to predict a change.

$2n_2 + 3h_2 \
ightleftharpoons 2nh_3 + \text{heat}$

(4 points)

	shift left	shift right	no change	no way to predict a change
taking away hydrogen	$\circ$	$\circ$	$\circ$	$\circ$
increasing the pressure	$\circ$	$\circ$	$\circ$	$\circ$
removing ammonia (nh3)	$\circ$	$\circ$	$\circ$	$\circ$

Explanation:

Step1: Analyze Adding more heat

The reaction \(2N_2 + 3H_2
ightleftharpoons 2NH_3 + \text{heat}\) is exothermic (heat is a product). Adding more heat (product) will shift the equilibrium to the left (to consume the added product). So for "Adding more heat", the shift is left.

Step2: Analyze Taking away hydrogen

Hydrogen (\(H_2\)) is a reactant. Removing a reactant will shift the equilibrium to the left (to produce more of the reactant). So for "Taking away hydrogen", the shift is left.

Step3: Analyze Increasing the pressure

For a gas - phase reaction, pressure is related to the number of moles of gas. The number of moles of gas on the reactant side: \(2 + 3=5\) moles, on the product side: \(2\) moles. Increasing pressure will shift the equilibrium towards the side with fewer moles of gas (product side, \(NH_3\)). So for "Increasing the pressure", the shift is right.

Step4: Analyze Removing ammonia (\(NH_3\))

Ammonia is a product. Removing a product will shift the equilibrium to the right (to produce more of the product). So for "Removing ammonia (\(NH_3\))", the shift is right.

Answer:

• Adding more heat: Shift left
• Taking away hydrogen: Shift left
• Increasing the pressure: Shift Right
• Removing ammonia (\(NH_3\)): Shift Right