A. Consider the following reaction: 2SO2 (g) + O2 (g) → 2SO3 (g) If the initial rate of change for sulfur dioxide is −2.00 M/min, what is the initial rate of change of oxygen?
a. −4.00 M/min
b. −1.00 M/min
c. 4.00 M/min
d. 1.00 M/min
B. Consider the following reaction: N2 (g) + 3Cl2 (g) → 2NCl3 (g) If the rate of reaction is 0.750 M/s, what is the rate of change of chlorine?
a. 0.250 M/s
b. 2.250 M/s
c. −0.250 M/s
d. −2.250 M/s
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A. Consider the following reaction: 2SO2 (g) + O2 (g) → 2SO3 (g) If the initial...
Consider the decomposition of sulfur trioxide gas into sulfur dioxide and oxygen 2SO3(g)<- ->2SO2(g) +O2(g) a flask of SO3 is filled to 0.960 M and allowed to decompose. at equilibrium the concentration of SO2 is 0.320 M what is Kc?
Sulfur dioxide and oxygen react to form sulfur trioxide, like
this: 2SO2(g)+O2(g)→2SO3(g)
Also, a chemist finds that at a certain temperature the
equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide
has the following composition:
Calculate the value of the equilibrium constant Kp for this
reaction. Round your answer to 2 significant digits.
compound pressure at equilibrium SO2 58.3 atm 02 84.7 atm SO3 66.3 atm
Consider the reaction: 2SO2(g) + O2(g)2SO3(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.11 moles of SO2(g) react at standard conditions. S°system = J/K
Consider the reaction 2SO2(g) + O2(g)2SO3(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.11 moles of SO2(g) react at standard conditions. S°surroundings = J/K
Consider the following equilibrium reaction. 2SO2(g)+O2(g)↽−−⇀2SO3(g)Δ?=−198 kJ/mol Which characteristics of this reaction will be affected by a change in temperature? I. value of equilibrium constant II. equilibrium concentrations Or both
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.07×10-2 moles of SO2(g) and 7.94×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.86×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
Consider the reaction: 2SO2(g)+O2(g)→2SO3(g) a) If 287.8 mL of SO2 reacts with 166.6 mL of O2 (both measured at 323 K and 67 mbar ), what is the limiting reactant? b) What is the theoretical yield of SO3? c) If 180.2 mL of SO3 is collected (measured at 323 K and 67 mbar ), what is the percent yield for the reaction?
Consider this reaction at equilibrium at a total pressure P1: 2SO2(g) + O2(g) 2SO3(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be A) twice P1 B) three times P1 C) 3.5 P1 D) less than twice P1 E) unchanged The answer is D, but would someone solve this question step-by-step?
Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) If 274.2 mL of SO2 is allowed to react with 159.0 mL of O2 (both measured at 322 K and 54.4 mmHg Part A: What is the theoretical yield of SO3? Part B: If 180.2 mL of SO3 is collected (measured at 322 K and 54.4 mmHg ), what is the percent yield for the reaction?