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°C, what mass 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°C, what mass 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°C, what mass of KMnO₄(s)should be decomposed? Assume the decomposition of KMnO₄(s)goes to completion.

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