What is the excess reactant for the following reaction given we have 3.4 moles o

Question

What is the excess reactant for the following reaction given we have 3.4 moles of ca(No_3) _2 and 2.4 moles of Li_3 PO_4? Reaction: 3Ca(NO_3) _2 + 2Li_3 PO_4 rightarrow 6LiNO_3 + Ca_3 (PO_4) _2 A)Li_3 PO_4 B)Ca(NO_3)_2 C) Ca_3 (PO_4)_2 D) LiNO_3 The elements with the highest electronegativity values tend to be found in the: A) center of the periodic table. B) lower right-side of the periodic table. C) upper left-side of the periodic table. D) upper right-side of the periodic table. E) lower left-side of the periodic table. Which of the following elements has the electron configuration of 3s^2 3p^3 in its outermost shell? A) Al B) Si C) P D) S

Explanation / Answer

1) The reactants which are not used completely when the reaction is over, are called excess reactants. From the above reaction stoichiometry, we know that 3 moles of Ca(NO3)2 require to react completely with 2 moles of Li3PO4. But we have 3.4moles Ca(NO3)2 and 2.4moles of Li3PO4 Therefore moles of Li3PO4 req to consume 3.4moles Ca(NO3)2 = 3.4X2/3 =2.26moles

But we have 2.4 moles. Thus excess reactant is Li3PO4

In a periodic table, electronegativity increases from bottom left hand corner to the upper right hand corner of the periodic table. Therefore answer is ( D.)

The outermost shell electronic configuration 3s2, 3p5 indicate that the element has total 15 electrons. Phosphorus has 15 electrons (atomic number of P is 15).Therefore answer is P.

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