In Part A, you found the amount of product (1.80 mol P2O5) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the amount of product (1.40 mol P2O5) formed from the given amount of oxygen and excess phosphorus. Now, determine how many moles of P2O5 are produced from the given amounts of phosphorus and oxygen.

Question

Li

Chemistry

8 December, 02:48

In Part A, you found the amount of product (1.80 mol P2O5) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the amount of product (1.40 mol P2O5) formed from the given amount of oxygen and excess phosphorus. Now, determine how many moles of P2O5 are produced from the given amounts of phosphorus and oxygen.

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Answers (1)

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Ronin Sloan · Answer 1

First step is to balance the reaction equation. Hence we get P4 + 5 O2 = > 2 P2O5

Second, we calculate the amounts we start with

P4: 112 g = 112 g / 124 g/mol - 0.903 mol

O2: 112 g = 112 g / 32 g/mol = 3.5 mol

Lastly, we calculate the amount of P2O5 produced.

2.5 mol of O2 will react with 0.7 mol of P2O5 to produce 1.4 mol of P2O5.

This is 1.4 * (31*2 + 16*5) = 198.8 g