Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:
2NF₃(g)
N₂(g) + 3F₂(g)
When 2.54 mol of NF₃ is placed in a 6.00-L container and allowed to come to equilibrium at 800 K,the mixture is found to contain 0.0434 mol of N₂.What is the value of K_p at this temperature? (R = 0.0821 L · atm · mol^-1 · K^-1)

Question

Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:
2NF₃(g)

Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF<sub>3</sub>(g) N<sub>2</sub>(g) + 3F<sub>2</sub>(g) When 2.54 mol of NF<sub>3</sub> is placed in a 6.00-L container and allowed to come to equilibrium at 800 K,the mixture is found to contain 0.0434 mol of N<sub>2</sub>.What is the value of K<sub>p</sub> at this temperature? (R = 0.0821 L · atm · mol<sup>-1</sup> · K<sup>-1</sup>) A) 1.54 × 10<sup>-5</sup> B) 1.91 × 10<sup>-3</sup> C) 1.78 × 10<sup>-3</sup> D) 1.59 × 10<sup>-5</sup> E) 4.43 × 10<sup>-7</sup>

N₂(g) + 3F₂(g)
When 2.54 mol of NF₃ is placed in a 6.00-L container and allowed to come to equilibrium at 800 K,the mixture is found to contain 0.0434 mol of N₂.What is the value of K_p at this temperature? (R = 0.0821 L · atm · mol^-1 · K^-1)

Quizplus · Accepted Answer

The Answer is B

Nitrogen Trifluoride Decomposes to Form Nitrogen and Fluorine Gases According