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Question

# Write the balanced equation when phosphorous burns in oxygen to form phosphorous pentoxide.

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Solution

## Balanced chemical equation:“A balanced equation for a chemical reaction is where the number of atoms and charge of each chemical element is equal in both reactants and products.”The reaction between phosphorus and oxygen:When phosphorus is made to burn in oxygen, it results in the formation of phosphorus pentoxide.${\mathrm{P}}_{4}\left(\mathrm{s}\right)+{\mathrm{O}}_{2}\left(\mathrm{g}\right)\stackrel{∆}{\to }{\mathrm{P}}_{2}{\mathrm{O}}_{5}\left(\mathrm{s}\right)\phantom{\rule{0ex}{0ex}}\left(\mathrm{Phosphorous}\right)\left(\mathrm{oxygen}\right)\left(\mathrm{Phosphorous}\mathrm{pentoxide}\right)$ElementReactant sideProduct side$\mathrm{P}$$4$ $2$$\mathrm{O}$$2$$5$Both phosphorus and oxygen are not balanced, by balancing the oxygen on the reactant and product side, the whole equation gets balanced.${\mathrm{P}}_{4}\left(\mathrm{s}\right)+5{\mathrm{O}}_{2}\left(\mathrm{g}\right)\stackrel{\mathrm{heat}}{\to }2{\mathrm{P}}_{2}{\mathrm{O}}_{5}\left(\mathrm{s}\right)\phantom{\rule{0ex}{0ex}}\left(\mathrm{Phosphorous}\right)\left(\mathrm{Oxygen}\right)\left(\mathrm{Phosphorous}\mathrm{pentoxide}\right)$ElementReactant sideProduct side$\mathrm{P}$$4$ $4$$\mathrm{O}$$10$$10$Thus the balanced equation is as follows:${\mathrm{P}}_{4}\left(\mathrm{s}\right)+5{\mathrm{O}}_{2}\left(\mathrm{g}\right)\stackrel{\mathrm{heat}}{\to }2{\mathrm{P}}_{2}{\mathrm{O}}_{5}\left(\mathrm{s}\right)\phantom{\rule{0ex}{0ex}}\left(\mathrm{Phosphorous}\right)\left(\mathrm{Oxygen}\right)\left(\mathrm{Phosphorous}\mathrm{pentoxide}\right)$

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