Consider the following reaction: a + 4b ➔ 3c + 2d if 5.0 mol of a reacts with 12.0 mol of b to form 6.0 mo! of c, the percent yield of the reaction is:

The % yiel of the reaction is 66.67%

Explanation:

Step 1: Data given

Number of moles of A = 5.0 mol

Number of moles of B = 12.0 mol

Number of moles of C formed = 6.0 = actual yield

Step 2: The balanced equation

A + 4B ➔ 3C + 2D

Step 3: Calculate the limiting reactant

B is the limiting reactant. It will completely be consumed ( 12.0 moles)

A is in excess. There will react 12/4 = 3.0 mol

There will remain 5.0 - 3.0 = 2.0 moles

Step 4: Calculate moles of C produced = theoretical yield

For 1 mol of A we need 4 moles of  B to produce 3 moles of C

For12.0 moles of B we'll have 9 moles of C produced.

Step 5: Calculate % yield

% yield = actual yield / theoretical yield

% yield = (6.0 mol / 9.0 mol)* 100%

% yield = 66.67 %

The % yiel of the reaction is 66.67%

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explanation:

they are both synthetic elements

explanation:

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