Write the balanced equation and determine the moles of O2 produced from 4.289 g KClO3 using gas stoichiometry. Lastly, use ideal gas equation to determine the volume of O2 from the # of moles O2 produced
The initial and unbalanced equation of decomposition of KClO3 will appear as:
KClO3 → O2 + KCl
When KClO3(s) (molar mass = 122.55 g mol–1 ) is heated at high temperature, it decomposes to give KCl(aq) (molar mass = 74.55 g mol–1 ) and O2(g) (molar mass = 32.00 g mol–1 ) as products. If 4.289 g of KClO3 are heated, how many liters of oxygen gas (measured at 22.4 oC and 754.0 torr) are produced?
A. 1.283 L
B. 0.9626 L
C. 0.8555 L
D. 1.668 L
E. 1.925 L
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