P4+5O2→2P2O5 Consider a situation in which 112 g of P4 are exposed to 112 g of...

Question

Question

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?

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Consider a situation in which 211 g of P4 are exposed to 240 g of O2....

Consider a situation in which 211 g of P4 are exposed to 240 g of O2. P4+5O2→2P2O5 Maximum number of moles of P2O5 that can theoretically be made from 211 g of P4 and excess oxygen = 3.4 mol Maximum number of moles of P2O5 that can theoretically be made from 240 g of O2 and excess phosphorus = 3 mol Question: What is the percent yield if the actual yield from this reaction is 341 g ? Express your...
Consider a situation in which 186 g of P4 are exposed to 208 g of O2....

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
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...

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. What is the percent yield if the actual yield from this reaction is 318 g ?
Consider a situation in which 161 g of P4 are exposed to 176 g of O2....

Consider a situation in which 161 g of P4 are exposed to 176 g of O2. What is the percent yield if the actual yield from this reaction is 259 g ? Express your answer to three significant figures and include the appropriate units.
A Review | Constants Periodic Table Correct Learning Goal: To calculate theoretical and percent yields, given the masse...

A Review | Constants Periodic Table Correct Learning Goal: To calculate theoretical and percent yields, given the masses of multiple reactants. A balanced chemical reaction gives the mole ratios between reactants and products. For example, one mole of white phosphorus, P4, reacts with five moles of oxygen, O2, to produce two moles of diphosphorus pentoxide, P205: Part B What is the maximum number of moles of P2O5 that can theoretically be made from 144 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...

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...
Calculations involving a limiting reactant Now consider a situation in which 23.0 g of P4 is...

Calculations involving a limiting reactant Now consider a situation in which 23.0 g of P4 is added to 50.0 g of Cl2, and a chemical reaction occurs. To identify the limiting reactant, you will need to perform two separate calculations: Calculate the number of moles of PCl5 that can be produced from 23.0 g of P4 (and excess Cl2). Calculate the number of moles of PCl5 that can be produced from 50.0 g of Cl2 (and excess P4). Then, compare...
The elements phosphorus and oxygen react to give tetraphosphorus pentoxide according to the balanced equation: P4...

The elements phosphorus and oxygen react to give tetraphosphorus pentoxide according to the balanced equation: P4 +5O2 → P4O10 Suppose you have 0.5203 mol P4. (a) How many moles of O2 are needed for complete reaction? (b) What mass of P4O10, in grams, can be produced? (The molar mass of P4O10 is 283.88

For each of the following reactions, calculate the grams of indicated product when 16.4 g of...

For each of the following reactions, calculate the grams of indicated product when 16.4 g of the first reactant and 10.1 g of the second reactant are used. You may want to reference (Pages 253 - 258) Section 7.9 while completing this problem. AlzS3 (s) + 6H2O(1)——2Al(OH)3 (aq) + 3H2S(g) Calculate the mass of H2S. .: HÅR O 2 ? mass of (H2S) = Value Units Submit Submit Request Answer Learning Goal: To calculate theoretical and percent yields, given the...