Exhibit 14-6 Consider the Reaction at Equilibrium Below and Its

question 4

Multiple Choice

Exhibit 14-6 Consider the reaction at equilibrium below and its corresponding equilibrium constant to answer the following question(s) .
2 NO₂ (g) 2 NO (g) + O₂(g) K p = 4.48*10^{- 13}
A pressure of 0.45 atm of NO₂ is introduced into a container and allowed to come to equilibrium. Complete the ICE equilibrium table shown below to get started. Partial pressure S₂NO₂² NO O₂Initial 0.45 M Change At equilibrium
-Refer to Exhibit 14-6. What relationship listed below can be used to solve for x in this table and ultimately the equilibrium partial pressures of each substance?

• A) x/(0.45 + 2x) = 4.48×10 ^{- 13}
• B) 2x³/(0.45 - 2x)² = 4.48×10 ^{- 13}
• C) 4x²/(0.45 - 2x)² = 4.48×10 ^{- 13}
• D) 4x³/(0.45 - 2x)² = 4.48×10 ^{- 13}
• E) 4x³/(0.45 + 2x) = 4.48×10 ^{- 13}

Comprehend the accounting treatment of normal and abnormal spoilage in cost accounting.

Grasp the concept of equivalent units and how they are used in process costing, including differences between weighted average and FIFO methods.

Understand the rationale behind using predetermined overhead rates in costing.

Identify the characteristics of products that dictate the selection of a specific costing system.

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