Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+ Cl2(g)

A sample of 43.1g MnO2 is added to a solution containing 42.9g HCl.

a. What is the limiting agent?
b. What is the theoretical yield of Cl2?
c. If the yield of the reaction is 72.9%, what is the actual yield of chlorine?

A. HCl is the limiting reactant.

B. Theoretical yield of Cl₂ is 20.9 g.

C. Actual yield of Cl₂ = 15.2 g.

Explanation:

The balanced equation for the reaction is given below:

4HCl + MnO₂ –> MnCl₂ + 2H₂O + Cl₂

Next, we shall determine the masses of HCl and MnO₂ that reacted and the mass of Cl₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of HCl = 1 + 35.5

= 36.5 g/mol

Mass of HCl from the balanced equation = 4 × 36.5 = 146 g

Molar mass of MnO₂ = 55 + (2×16)

= 55 + 32

= 87 g/mol

Mass of MnO₂ from the balanced equation = 1 × 87 = 87 g

Molar mass of Cl₂ = 2 × 35.5

= 71 g/mol

Mass of Cl₂ from the balanced equation = 1 × 71 = 71 g

SUMMARY:

From the balanced equation above,

146 g of HCl reacted with 87 g of MnO₂ to produce 71 g of Cl₂.

A. Determination of the limiting reactant.

From the balanced equation above,

146 g of HCl reacted with 87 g of MnO₂.

Therefore, 42.9 g of HCl will react with = (42.9 × 87)/146 = 25.6 g of MnO₂.

From the calculation made above, we can see clearly that only 25.6 g out of 43.1 g of MnO₂ given was needed to react completely with 42.9 g of HCl.

Therefore, HCl is the limiting reactant.

B. Determination of theoretical yield of Cl₂.

Here, the limiting reactant will be used.

From the balanced equation above,

146 g of HCl reacted to produce 71 g of Cl₂.

Therefore, 42.9 g of HCl will react to produce = (42.9 × 71)/146 = 20.9 g of Cl₂.

Thus, the theoretical yield of Cl₂ is 20.9 g.

C. Determination of the actual yield of Cl₂.

Theoretical yield of Cl₂ = 20.9 g

Percentage yield of Cl₂ = 72.9%

Actual yield of Cl₂ =?

Percentage yield = Actual yield / Theoretical yield × 100

72.9% = Actual yield / 20.9

Cross multiply

Actual yield = 72.9% × 20.9

Actual yield = 72.9/100 × 20.9

Actual yield = 0.729 × 20.9

Actual yield of Cl₂ = 15.2 g

answer: option (4) is the correct answer.

explanation:

areas which are at low altitudes and near the equator tend to receive direct sunlight from the sun. hence, heat energy or radiations from the sun make these areas warmer and they have warmest water.

whereas areas which are at high altitudes and away from the equator do no receive direct sunlight. hence, no direct contact from the sun makes these regions colder and thus, they have colder water.

thus, we can conclude that the statement areas at low latitudes near the equator have the warmest water because they receive the most direct sunlight best explains the relationship between an area's geography and the temperature of its surface water.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: