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olga2289 [7]
3 years ago
9

Look at the following hypothetical reaction: A + 4B - C + 3D. Assume that the equation is balanced. Which of the following mole

ratios will produce the most product?
a) A/B

b) A/4B

c) 3A/4B

d) 4A/B
Chemistry
2 answers:
ra1l [238]3 years ago
7 0
Answer is: <span>b) A/4B.
Chemical reaction: A + 4B </span>→ C + 3D.
from chemical reaction: n(A) : n(B) = 1 : 4.
a) if 1A reacts with 1B, there is not enough B (need 3B more).
c) if 3A react with 4B, there is not enough B (need 8B more).
d) if 4A react with 1B, there is not enough B (need 15B more). 

yuradex [85]3 years ago
5 0

The correct answer is b. Since the equation is balance we can establish that A and B react in the ration 1:4. So in order for the reactants to produce more product there must exist a limiting reactant that gets used up once the ratio of reactants is 1:4 or greater than this value. The first pair of reactants gives us a 1:1 ratio, which means

a.mol A \times \frac{mol C}{mol A} = mol\ C\\\\mol B \times \frac{mol C}{4mol B} = 0.25 mol\ C.

Here B is the limiting reactant and it get used up before we can go above our treshold ratio.

b. mol A \times \frac{mol C}{mol A} = mol C\\\\4mol B \times \frac{mol C}{4mol\ B} = mol\ C

The reactants react in the ratio 1:4 which gives 1 mol of C

c. 3mol A \times \frac{mol C}{mol A} = 3mol\ C\\\\4mol B \times  \frac{mol C}{4mol B} = 1 mol C

The 3:4 ratio makes B be the limiting reactant which means even though we have 3 moles of A, after 1 mol A has reacted all the 4 moles of B will be used up.

d, 4mol A \times \frac{molC }{mol A} = 4mol\ C\\\\mol\ B \times \frac{mol C}{ mol B} = 1 mol C

Here there is not enough moles of B to get more product.


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A 25.00 ml solution of sulfuric acid H2SO4 is titrated to phenolphthalein end point with 27.00 ml of 1.700 M KOH
Nastasia [14]
<h3>Answer:</h3>

0.918 M

<h3>Explanation:</h3>

Assuming the question requires we calculate the Molarity of sulfuric acid:

We are given:

  • Volume of the acid, H₂SO₄ = 25.00 ml
  • Volume of the base, KOH = 27.00 mL
  • Molarity of the base, KOH is 1.70 M

We can calculate the molarity of the acid using the following steps;

<h3>Step 1: Write the chemical equation for the reaction.</h3>

The reaction is an example of a neutralization reaction where a base reacts with an acid to form salt and water.

Therefore, the balanced equation will be;

H₂SO₄(aq) + 2KOH(aq) → K₂SO₄(aq) + 2H₂O(l)

<h3>Step 2: Determine the moles of the base, KOH </h3>

When given molarity and the volume of a solution, the number of moles can be calculated by multiplying molarity with volume.

Number of moles = Molarity × Volume

                             = 1.700 M × 0.027 L

                              = 0.0459 moles

Thus, moles of KOH used is 0.0459 moles

<h3>Step 3: Determine the number of moles of the Acid, H₂SO₄</h3>

From the reaction, 1 mole of the acid reacts with 2 moles of KOH

Therefore, the mole ratio of H₂SO₄ to KOH is 1 : 2

Thus, moles of H₂SO₄ = Moles of KOH ÷ 2

                                     = 0.0459 moles ÷ 2

                                     = 0.02295 moles

<h3>Step 4: Calculate the molarity of the Acid </h3>

Molarity is the concentration of a solution in moles per liter

Molarity = Moles ÷ Volume

Molarity of the acid = 0.02295 moles ÷ 0.025 L

                                = 0.918 M

Thus, the molarity of the acid, H₂SO₄ is 0.918 M

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