Question

3. Phosphorus burn in air to produce a phosphorus oxide in the following reaction: \[ 4 \mathrm{P}_{(\mathrm{s})}+5 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{P}_{4} \mathrm{O}_{10(\mathrm{~s})} \] a) What mass of phosphorus will be needed to produce 3.25 mol of \( \mathrm{P}_{4} \mathrm{O}_{10} \) ? ( 2 marks) b) If 0.489 mol of phosphorus burn, what mass of oxygen is used? What mass of \( \mathrm{P}_{4} \mathrm{O}_{10} \) is produced? (2 marks)

          3. Phosphorus burn in air to produce a phosphorus oxide in the following reaction:
\[
4 \mathrm{P}_{(\mathrm{s})}+5 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{P}_{4} \mathrm{O}_{10(\mathrm{~s})}
\]
a) What mass of phosphorus will be needed to produce 3.25 mol of \( \mathrm{P}_{4} \mathrm{O}_{10} \) ? ( 2 marks)
b) If 0.489 mol of phosphorus burn, what mass of oxygen is used? What mass of \( \mathrm{P}_{4} \mathrm{O}_{10} \) is produced? (2 marks)

3. Phosphorus burn in air to produce a phosphorus oxide in the following reaction:

4 P(s)+5 O2( g)→P4O10( s)

a) What mass of phosphorus will be needed to produce 3.25 mol of P4O10 ? ( 2 marks)
b) If 0.489 mol of phosphorus burn, what mass of oxygen is used? What mass of P4O10 is produced? (2 marks)

Added by Renee C.

Chemistry Principles and Reactions

William L. Masterton, Cecile N. Hurley 8th Edition

Chapter 3

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Solved by Expert Ishu S

Step 1

The balanced equation is: \[ 4 \mathrm{P}_{(\mathrm{s})} + 5 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{P}_{4} \mathrm{O}_{10(\mathrm{~s})} \] Show more…

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3. Phosphorus burn in air to produce a phosphorus oxide in the following reaction: \[ 4 \mathrm{P}_{(\mathrm{s})}+5 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{P}_{4} \mathrm{O}_{10(\mathrm{~s})} \] a) What mass of phosphorus will be needed to produce 3.25 mol of \( \mathrm{P}_{4} \mathrm{O}_{10} \) ? ( 2 marks) b) If 0.489 mol of phosphorus burn, what mass of oxygen is used? What mass of \( \mathrm{P}_{4} \mathrm{O}_{10} \) is produced? (2 marks)