Consider a situation in which 235 g of P4 are exposed to 272 g of O2.
What is the percent yield if the actual yield from this reaction is 318 g ?
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Consider a situation in which 235 g of P4 are exposed to 272 g of O2....
Consider a situation in which 235 g of P4 are exposed to 272 g of O2. In Part A, you found the amount of product (3.80 mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the amount of product (3.40 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. Express...
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Consider a situation in which 186 g of P4 are exposed to 208 g of O2. a) What is the maximum amount in moles of P2O5 that can theoretically be made from 186 g of P4 and excess oxygen? b) What is the maximum amount in moles of P2O5 that can theoretically be made from 208 g of O2 and excess phosphorus? How do I solve these? I forgot the equations Thanks in advance
P4+5O2→2P2O5 Consider a situation in which 112 g of P4 are exposed to 112 g of O2. Part A What is the maximum amount in moles of P2O5 that can theoretically be made from 112 g of P4 and excess oxygen? Part B What is the maximum amount in moles of P2O5 that can theoretically be made from 112 g of O2 and excess phosphorus?
P4(s)+10Cl2(g)→4PCl5(g) Now consider a situation in which 29.0 g of P4 is added to 55.0 g of Cl2, and a chemical reaction occurs. To identify the limiting reactant, you will need to perform two separate calculations: 1. Calculate the number of moles of PCl5 that can be produced from 29.0 g of P4 (and excess Cl2). 2. Calculate the number of moles of PCl5 that can be produced from 55.0 g of Cl2 (and excess P4). 3. Then, compare the...
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