2SO2 + O2 ----> 2SO3 + Energy
Decreasing the
volume - moles of SO3 will increase as decreasing pressure
will shift the reaction towards SO3.
Adding oxygen to
equilibrium mixture - moles of SO3 will increase as O2 is a
reactant, increasing reactant will proceed with the reaction
towards the product.
Raising the temperature of
the system - being an exothermic reaction increase in
temperature will reduce the moles of SO3 produced.
Decreasing the pressure of
the system - Decreasing the pressure is accompanied by
volume ncrease. Tyhen it will proceed towards the higfher number of
moles. So, moles of SO3 will reduce.
Adding a catalyst -
moles of SO3 will not change on the addition of catalyst but
equilibrium will be formed earlier.
2SO2 + O2 ----> 2SO3 + Energy
Decreasing the
volume - The rate of forwarding reaction will increase as
the decreasing volume will shift the reaction towards the lesser
number of moles, thus SO3 production will be
higher.
Adding oxygen to
equilibrium mixture - It is one of the reactants, so adding
O2 will increase the rate of the forward reaction.
Raising the temperature of
the system - As it is an exothermic reaction, adding
temperature will decrease the forward rate of reaction.
Decreasing the pressure of
the system - Decreasing pressure is accompanied by inceasein
volume, so it will proceed towards the higher number of moles. So
rate of forward reaction will reduce and backward reaction will
rise.
Adding a catalyst -
Adding a catalyst will increase the rate of forward reaction as
well as the backward reaction.
1. Consider the following reaction at equilibrium. 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) a. What will happen if the pressure increased? b. What will happen if the concentration of FeS2(s) is decreased? 2) The following reaction is exothermic: What direction will the equilibrium shift if the following changes are made? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) a) Raising the temperature b) Adding SO3 c) Removing O2 d) Decreasing the volume
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
1. a) Predict the effect of the following changes on the reaction in which SO3 decomposes to form SO2 and O2. 2 SO3(g) → 2 SO2 (g) + O2 (g) delta Ho = 197.78 kJ (1) Increasing the temperature of the reaction. (2) Increasing the pressure on the reaction. (3) Adding more O2 when the reaction is at equilibrium. (4) Removing O2 from the system when the reaction is at equilibrium. b) A person exposed to high levels of carbon...
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2(g) 02(8)2 S03(g) O A) Adding SO3 O B) Increase volume O c) Increase the temperature OD) Adding catalyst 0 E) Increase pressure
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
Using Le Chatelier's Principle, What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the reaction? 2SO3(g) ⇌ 2SO2(g) + O2(g) in each of the following cases: 1. Oxygen is added to reaction container. 2. The pressure is increased by decreasing the volume of the reaction container. 3. In the rigid container (i.e. constant volume), the pressure is increased by adding argon gas. 4. The temperature of the reaction container is decreased (Note:...
Sulfur trioxide is formed from sulfur dioxide and oxygen according to the reaction formula 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) with the equilibrium constant 2.5 × 1010 at the temperature 5.0 × 102 K. A reaction vessel with a volume of 0.25 L contains from start 0.030 moles of SO2 (g) and 0.050 moles of O2 (g). a) Calculate the partial pressure SO3 (g) after equilibrium is reached at 5.0 × 102 K. b) Will more...
Consider the following system at equilibrium where K. = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 SO2 (g) + O2(g) 2 S03 (g) The production of Soz (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. decreasing the temperature. 2. increasing the pressure (by changing the volume). 3. decreasing the volume. 4. adding SO3 5. removing 02
Please answer all four of these questions and explain WHY. I don't understand any of this. Thank you! Consider the following reaction: 2 SO2(g)O2(g)2 SO3(g) If 1.55 moles of SO2 and 1.55 moles of O2 are added to an empty sealed container: What is the rate of the reverse reaction BEFORE any SO3 has been formed? Greater than zero, and greater than the rate of the forward reaction. What is the rate of the reverse reaction an instant AFTER some...
28. For the reaction 2 SO2(g) + O2(g) → 2 S03(), a. Determine the expression for the rate of the reaction with respect to each of the reactants and products. b. When SO3 is increasing at a rate of 0.0071 M/s, how fast is 02 decreasing? How fast is SO2 A decreasing?