A convenient way to produce very high purity oxygen in the laboratory is to decompose KMnO₄(s) at high temperature according to the following chemical equation: 2KMnO₄(s) $\rarr$ K₂MnO₄(s) + MnO₂(s) + O₂(g)
If 2.50 L of O₂(g) is needed at 1.00 atm and 20.^$\circ$C, what mass (in grams) of KMnO₄(s) should be decomposed
Assume the decomposition of KMnO₄(s) goes to completion.

Question

A convenient way to produce very high purity oxygen in the laboratory is to decompose KMnO₄(s) at high temperature according to the following chemical equation: 2KMnO₄(s)

\rarr

K₂MnO₄(s) + MnO₂(s) + O₂(g)
If 2.50 L of O₂(g) is needed at 1.00 atm and 20.^$\circ$C, what mass (in grams) of KMnO₄(s) should be decomposed
Assume the decomposition of KMnO₄(s) goes to completion.

Quizplus · Accepted Answer

The Answer of A convenient way to produce very high purity oxygen in the laboratory is to decompose KMnO₄(s) at high temperature according to the following chemical equation: 2KMnO₄(s) $\rarr$K₂MnO₄(s) + MnO₂(s) + O₂(g) If 2.50 L of O₂(g) is needed at 1.00 atm and 20.^$\circ$C, what mass (in grams) of KMnO₄(s) should be decomposed Assume the decomposition of KMnO₄(s) goes to completion. A) 35.8 g B) 34.8 g C) 33.8 g D) 32.8 g E) None of the above

A Convenient Way to Produce Very High Purity Oxygen in the Laboratory