Consider the decomposition of hydrazine as shown below. N₂H₄(g) 2H₂(g) + N₂(g)
At a certain temperature, K_p = 2.5 *10³. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium.

Question

Consider the decomposition of hydrazine as shown below. N₂H₄(g)

Consider the decomposition of hydrazine as shown below. N<sub>2</sub>H<sub>4</sub>(g) 2H<sub>2</sub>(g) + N<sub>2</sub>(g) At a certain temperature, K<sub>p</sub> = 2.5 *10<sup>3</sup>. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium. A) 76 atm B) 5776 atm C) 54 atm D) 127 atm E) none of these

2H₂(g) + N₂(g)
At a certain temperature, K_p = 2.5 *10³. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium.

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The Answer of Consider the decomposition of hydrazine as shown below. N₂H₄(g) 2H₂(g) + N₂(g) At a certain temperature, K_p = 2.5 *10³. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium.

Consider the Decomposition of Hydrazine as Shown Below