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GuDViN [60]
2 years ago
7

Lab: Limiting Reactant and Percent Yield

Chemistry
2 answers:
creativ13 [48]2 years ago
7 0

Answer : If a substance is the limiting reactant, then it limits the formation of products because in the reaction it is present in limited amount.

Explanation :

While observing a chemical reaction, we can tell about whether a reactant is limiting or excess.

Step 1 : first write the chemical reaction and then balanced the chemical equation.

C_2H_4+H_2\rightarrow C_2H_6

Step 2 : convert the given masses into the moles if mass of C_2H_4 is 10.5 g and molar mass of C_2H_4 is 28 g/mole and the mass of hydrogen is 0.40 g and molar mass of hydrogen is 2 g/mole.

\text{moles of }C_{2}H_{4}=\frac{10.5g}{28g/mole}=0.375moles

\text{moles of }H_{2}=\frac{0.40g}{2g/mole}=0.20moles

Step 3 : Now we have to determine the limiting reagent and excess reagent.

\text{ moles of }C_{2}H_{4}\text{ in excess}=0.375-0.20=0.175\text{moles}

Now we conclude that C_{2}H_{4} is the limiting reagent and hydrogen is an excess reagent.

Hypothesis :

Limiting reagent : It is the reagent in the chemical reaction that is totally consumed when the chemical reaction is complete.  Limiting reagent limits the formation of products.

OverLord2011 [107]2 years ago
7 0

Answer:

If a substance is the limiting reactant, then . . .

it will limit the formation of products

because . . .

the reaction is presented at limited

Explanation:

just took the test

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2 years ago
Each 5-ml teaspoon of Extra Strength Maalox Plus contains 450 mg of magnesium hydroxide and 500 mg of aluminum hydroxide. How ma
Art [367]

Answer:

0.0347 moles of hydronium ions

Explanation:

The equation of the neutralization reaction between hydroxide and hydronium ions is given below:

H₃O+ (aq) + OH- (aq) ----> 2 H₂O (l)

From the equation above, 1 mole of hydroxide ions will neutralize one mole hydronium ions.

The moles of hydroxide ions present in 1 teaspoon or 5 mL of antacid product is calculated as follows:

Number of moles = mass / molar mass

Molar mass of Magnesium hydroxide, Mg(OH)₂ = 58 g/mol

Molar mass of aluminium hydroxide, Al(OH)₃ = 78 g/mol

Mass of magnesium hydroxide = 450 g = 0.45 g

Mass of aluminium hydroxide = 500 mg = 0.5 g

Moles of magnesium hydroxide = (0.45/58) moles

Moles of aluminium hydroxide = (0.5/78) moles

Equation of the ionization of magnesium hydroxide and aluminium hydroxide is given below:

Mg(OH)₂ (aq) ----> Mg²+ (aq) + 2 OH- (aq)

Al(OH)₃ (aq) ---> Al³+ (aq) + 3 OH- (aq)

Number of moles of hydroxide ions present in (0.45/58) moles of magnesium hydroxide = 2 × (0.45/58) moles = 0.0155 moles

Number of moles of hydroxide ions present in (0.5/78) moles of aluminium hydroxide = 3 × (0.5/78) moles = 0.0192 moles

Total moles of hydroxide ions = 0.0155 + 0.0192 = 0.0347 moles hydroxide ions

Therefore, 0.0347 moles of hydroxide ions will neutralize 0.0347 moles of hydronium ions.

3 0
3 years ago
An aqueous magnesium chloride solution is made by dissolving 7.15 moles of MgCl2 in sufficient water so that the final volume of
irinina [24]

Answer:

2.86mol/L

Explanation:

Given parameters:

Number of moles of MgCl₂  = 7.15moles

Volume of solution  = 2.50L

Unknown:

Molarity of the MgCl₂ solution = ?

Solution:

The molarity of a solution is the number of moles of solute found in a given volume.

  Molarity  = \frac{number of moles }{volume}  

 Insert the parameters and solve;

   Molarity  = \frac{7.15}{2.5}   = 2.86mol/L

4 0
3 years ago
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