Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g)
Part B What is the theoretical yield of SO3? nSO3 =
Part C If 175.8 mL of SO3 is collected (measured at 327 K and
48.7 mmHg ), what is the percent yield for the reaction? Express
your answer using four significant figures.
Consider the following reaction at 388 K
2SO2 (g) + O2 (g) <==> 2SO3 (g)
At equilibrium the reaction mixture contains 1.28 atm of O2 and
6.78 atm of SO3. The
equilibrium constant, KP, at this temperature is 46.7. Calculate
the equilibrium partial
pressure of SO2.
Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) 290.2 mL
of SO2 is allowed to react with 151.8 mL of O2 (both measured at
318 K and 47.9 mmHg ), what is the limiting reactant? What is the
theoretical yield of SO3? If 170.7 mL of SO3 is collected (measured
at 318 K and 47.9 mmHg ), what is the percent yield for the
reaction?
Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g)
Part A If 276.0 mL of SO2 is allowed to react with 161.4 mL of
O2 (both measured at 327 K and 48.7 mmHg ), what is the limiting
reactant?
Part B What is the theoretical yield of SO3? nSO3 =
Part C If 175.8 mL of SO3 is collected (measured at 327 K and
48.7 mmHg ), what is the percent yield for the reaction? Express
your answer using four significant figures.
The following reaction wax examined at 250 C
2SO3(g) <--------- ------------->
2SO2(g) + O2(g)
At a particular temperature , 14.5 mole SO3 is placed in to a
2.0 L container and dissociates according to the reaction above. At
equilibrium 3.0 mole of SO2 is present. Calculate Kc for this
reaction
-A student ran the following reaction in the laboratory at
1143 K:
2SO2(g) +
O2(g)
2SO3(g)
When she introduced 8.19×10-2 moles of
SO2(g) and
8.56×10-2 moles of
O2(g) into a 1.00 liter container, she
found the equilibrium concentration of
O2(g) to be
6.08×10-2 M.
Calculate the equilibrium constant, Kc, she obtained for
this reaction.
Kc =____________
-A student ran the following reaction in the laboratory at
363 K:
CH4(g) +
CCl4(g)
2CH2Cl2(g)
When she introduced 4.64×10-2 moles of
CH4(g) and...
ALL WITH EXPLANATIONS please :)
12. Consider the following reaction:
2SO2(g) + O2(g) ⇄ 2SO3(g) +E
Which of the following will not shift the equilibrium to the
right?
A. Adding
more O2
B. Adding
a catalyst
C. Increasing
the pressure
D. Lowing
the temperature
13. Consider
the following equilibrium system: CaCO3(s) ⇄
CaO(s) + CO2(g)
Which
one of the following changes would cause the above system to shift
left?
A. Add
more CaO
B. Remove
CaCO3
C. Increase
pressure
D. Remove
CO2
14. Consider
the following equilibrium:
SO2Cl2(g) + energy ⇄ SO2(g) + Cl2(g)
When
the temperature is decreased, the equilibrium shifts
A. Left...
At a certain temperature, 0.900 mol SO3 is placed in a 5.00 L
container.
2SO3(g)−⇀↽−2SO2(g)+O2(g)
At equilibrium, 0.110 mol O2 is present. Calculate Kc.
2SO2(g) + O2(g) <--> 2SO3(g)
A sealed reaction vessel is charged with 5.0 atm SO2 and 2.5 M
atm at 500 degrees Celsius. The reaction is allowed to
equilibriate. At equilibrium 3.0 atm of SO3 is produced. What is
the equilibrium concentration of each species. What is Kc for this
reaction? Show all work.
The following reaction can occur at 298K under
appropriate conditions.
2SO2(g) +O2(g)-----> 2SO3(g)
An equilibrium mixture contain O2(g) and SO3(g) at partial pressure
of 0.50atm and 2.0atm respectively. Using data available in
Appendix 4 of your textbook, determine the equilibrium partial
pressure of SO2 in the mixture. Will this reaction be most favored
at a high or at a low temperature, assuming standard conditions?
Justify your reasoning
Substance.
delta
H°
S°
SO2(g)
-297.
248
SO3(g)
-396.
257
O2(g)
0.
205