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Crazy boy [7]
2 years ago
14

С

Chemistry
1 answer:
algol [13]2 years ago
6 0

The percent composition  of this compound :

Mg = 72.182%

N = 27.818%

<h3> Further explanation </h3>

Given

9.03 g  Mg

3.48 g  N

Required

The percent composition

Solution

Proust stated the Comparative Law that compounds are formed from elements with the same Mass Comparison so that the compound has a fixed composition of elements

Total mass of the compound :

= 9.03 g + 3.48 g

= 12.51 g

The percent composition :

Mg : 9.03/ 12.51 g x 100% = 72.182%

N : 3.48 / 12.51 g x 100% = 27.818%

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The answer to your question is below

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a. How many grams of Cl2 are needed to react with 20.00 g of P4? ___68.7 g___________

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                         20     ----------    x

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b. You have 15.00 g. of P4 and 22.00 g. of Cl2, identify the limiting reactant and calculate the grams of PCl3 that can be produced as well as the grams of excess reactant remaining. LR____________ grams PCl3 _________ grams excess reactant ___________

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I will use P4 to find the limiting reactant

                 

                     x = (15 x 426) / 124 = 51.5   The limiting reactant is Chlorine

                                                                  because we need 51.5 g and we only have 22g

Excess reactant

                 x = (22 x 124) / 426 = 6.4 g of P4

           Excess P4 = 15 g - 6.4 = 8.6 g of P4 in excess

Grams of PCl3 produced

                              426 g of Cl2 ----------------  550 g of PCl3

                                 22g of Cl2 ------------- -     x

            x = (22 x 550) / 426 = 28.4 g of PCl3

c. If the actual amount of PCl3 recovered is 16.25 g., what is the percent yield? ______________

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d. Given 28.00 g. of P4 and 106.30 g. of Cl2, identify the limiting reactant and calculate how many grams of the excess reactant will remain after the reaction. LR ______________ grams excess reactant

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x = (28 x 426) / 124

x = 96.2 g of Cl2 and we have 106.3 so Chlorine is the excess reactant and P4 is the limiting reactant.

Excess reactant = 106.3  - 96.2 = 10.1 g of Cl2 in excess

                   

                 

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