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1. Take the reactions NH3 + 02-NO H20. In an experiment, 3.25g of NH3 are allowed to react with 3.50g of 02.

A. Which reactant is the limiting reagent?

B. How many grams of NO are formed?

C. How much of the excess reactant remains after the reaction?

2. Consider the reaction of C6H6 + Br2 C6H5Br + HBr

A. What is the theoretical yield of C6H5Br if 42.1 g of C6H6 react with 73.0 g Br3?

B. If the actual yield of C6H5Br is 63.6 g, what is the percent yields?​

Sagot :

Princessmaghari993idn

Answer:

1.) Given:

NH3 + O2 -> NO + H2O

3.25 g of NH3 are allowed to react with 3.50 g of O2

To find:

• Which reactant is the limiting reagent

• How many grams of NO are formed

• How much of the excess reactant remains after the reaction

Solution:

A.) On balancing the given equation,

4 NH3 + 5O2 –> 4 NO + 6H2O

Mass of 4 moles of NH3 = 4x(17) = 68g

Mass of 5 moles of O2 = 5x(32) = 160g

3.5/3.25 < 160/68

Hence, the limiting reagent is O2.

B.) O2 NO

160g -> 112g

3.5g -> x

x = 2.45g

Hence, 2.45 grams of NO are formed.

C.) NH3 O2

68g –> 160 g

x –> 3.5 g

x = 1.49 g of NH3

Remaining excess = 3.25–1.49 = 1.76 g

Hence, the remaining excess is 1.76g.

2.) Consider the reaction of C6H6 + Br2 C6H5Br + HBr

A. What is the theoretical yield of C6H5Br if 42.1 g of C6H6 react with 73.0 g Br3?

Answer : 71.6g C6H5Br

B. If the actual yield of C6H5Br is 63.6 g, what is the percent yields?

Answer : 88.8%

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