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When 3.00 g of hydrogen reacts with 4.00 g of oxygen, 4.00 g of water is formed.

(a) What is the limiting reactant?
(b) What is the theoretical yield?
(c) What is the percent yield?
Question 11 options:

a)

(a) oxygen

(b) 4.51 g

(c) 88.7 %


b)

(a) hydrogen

(b) 4.51 g

(c) 88.7 %


c)

(a) oxygen

(b) 4.05 g

(c)13.0 %


d)

(a) hydrogen

(b) 4.05 g

(c) 13.0 %

Respuesta :

Answer:

Answer A  

Explanation:

2 H2  +  O2  = 2 H2O  

  knowing the mole weights of these elements shows O2 is the limiting reactant in this situation.

4 g oxygen is  4 /31.998  = .125 mole O2

  We should get two times these moles of water = .250 moles

         weight = .250 (1.008 * 2  + 15.999) =  4.50 gm H20   (theoretical)

   ....but we only got 4 gm

4/4.50  =  88.8%  

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