When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) Imported Asset MgCl2 (aq) + H2 (g), if 72.9 g of Mg and 146.0 g of HCl are allowed to react, identify the limiting reagent.
Mg
HCl
MgCl2
H2
QUESTION 8
When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) Imported Asset MgCl2 (aq) + H2 (g), if 48.6 g of Mg and 150.0 g of HCl are allowed to react, identify the limiting reagent.
Mg
HCl
MgCl2
H2
QUESTION 9
The number of moles of the reagent in excess can be used to calculate the moles of the products of the reaction.
TRUE
FALSE
QUESTION 10
Ammonia gas is formed from nitrogen gas and hydrogen gas according to the following equation: N2 (g) + 3H2 (g) Imported Asset 2NH3 (g). If 112 grams of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 120 grams of ammonia, what is the percent yield of this reaction?
44.1%
66.2%
88.3%
96.4%
QUESTION 11
Ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation: N2 (g) + 3H2 (g) Imported Asset 2NH3 (g). If 84.0 g of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 85.0 g of ammonia, what is the percent yield of this reaction?
42.2%
65.0%
70.3%
83.3%
QUESTION 12
Ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation, N2 (g) + 3H2 (g) Imported Asset 2NH3 (g). If 140 grams of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 155 grams of ammonia, what is the percent yield of this reaction?
45.5%
67.0%
82.4%
91.2%
3 points Save Answer
QUESTION 13
The actual yield is usually less than the predicted (theoretical) yield.
TRUE
FALSE
2 points Save Answer
QUESTION 14
The theoretical yield for a chemical reaction can not be calculated until the reaction is completed.
TRUE
FALSE
When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) Imported Asset MgCl2 (aq) + H2 (g), if 72.9 g of Mg and 146.0 g of HCl are allowed to react, identify the limiting reagent.
Mg
HCl
MgCl2
H2
I assume imported asset means arrow. You can write an arrow a little easier like this. --> or ==> or >>>.
Mg + 2HCl ==> MgCl2 + H2
mols Mg = grams/atomic mass = 72.9/24.3 = 3
mols HCl = 146/35.5 = 4.12
If Mg is the limiting reagent (LR) all of it will be used. How much HCl is needed? That will be
mols HCl needed = 3 mol Mg x (2 mols HCl/1 mol Mg) = 6 mols HCl. You don't have that much HCl; therefore, Mg can't be the LR which means HCl must be the LR. I always like to check that to see that I didn't make an error. So now we ask ourselves if HCl is the LR, all of it will be used. How much Mg is needed? That's
4.12 mols HCl x (1 mol Mg/2 mols HCl) = 4.12 x 1/2 = 2.06 mols Mg needed. Do you have that much Mg. Yes, so HCl is the LR, all of it will be used, and some of the Mg will be used but some will be left unreacted. Mg is the reagent in excess.
Listen here! Yall should solve this question right without having any problems! Because I need this for myself...
To identify the limiting reagent in a chemical reaction, we need to compare the number of moles of each reactant and determine which reactant is completely consumed first.
In QUESTION 8, we have 48.6 g of Mg and 150.0 g of HCl.
To find the number of moles of each reactant, we use the molar mass of the substances:
- Mg: molar mass = 24.31 g/mol
- HCl: molar mass = 36.46 g/mol
Number of moles of Mg = 48.6 g / 24.31 g/mol = 2 moles of Mg
Number of moles of HCl = 150.0 g / 36.46 g/mol = 4.112 moles of HCl
Now, we compare the ratio of moles of Mg to HCl in the balanced equation, which is 1:2. We can see that we have 2 moles of Mg and 4.112 moles of HCl, so the HCl is in excess. Therefore, the limiting reagent is Mg.
The answer to QUESTION 8 is: The limiting reagent is Mg.
In QUESTION 9, the statement says "The number of moles of the reagent in excess can be used to calculate the moles of the products of the reaction." This statement is TRUE. When the limiting reagent is consumed completely, any excess reactant remaining can be used to calculate the moles of the products.
The answer to QUESTION 9 is: TRUE.
To calculate the percent yield of a reaction, we compare the actual yield to the theoretical yield.
In QUESTION 10, we have 112 grams of nitrogen gas reacting to produce 120 grams of ammonia. The molar mass of nitrogen gas is 28.02 g/mol, and the molar mass of ammonia is 17.03 g/mol.
Number of moles of nitrogen = 112 g / 28.02 g/mol = 3.996 moles of nitrogen
The balanced equation tells us that 1 mole of nitrogen reacts to form 2 moles of ammonia, so the theoretical yield of ammonia is 2 * 3.996 = 7.992 moles.
The molar mass of ammonia is 17.03 g/mol, so the theoretical yield in grams is 7.992 moles * 17.03 g/mol = 136.35 grams.
The percent yield is calculated by dividing the actual yield (120 grams) by the theoretical yield (136.35 grams) and multiplying by 100:
Percent yield = (actual yield / theoretical yield) * 100
Percent yield = (120 g / 136.35 g) * 100 = 88.15%
The answer to QUESTION 10 is: 88.3%
Similarly, in QUESTION 11 and QUESTION 12, we follow the same steps to calculate the percent yield.
For QUESTION 11:
Actual yield = 85.0 grams of ammonia
Theoretical yield = 2 * 84.0 g/mol = 168 grams
Percent yield = (85.0 g / 168 g) * 100 = 50.60%
The answer to QUESTION 11 is: 50.6%
For QUESTION 12:
Actual yield = 155 grams of ammonia
Theoretical yield = 2 * 140 g/mol = 280 grams
Percent yield = (155 g / 280 g) * 100 = 55.36%
The answer to QUESTION 12 is: 55.4%
In QUESTION 13, the statement says "The actual yield is usually less than the predicted (theoretical) yield." This statement is TRUE. The actual yield represents the amount of product that is obtained during a reaction, which is often less than the theoretical yield due to experimental limitations and other factors.
The answer to QUESTION 13 is: TRUE.
In QUESTION 14, the statement says "The theoretical yield for a chemical reaction can not be calculated until the reaction is completed." This statement is FALSE. Theoretical yield can be calculated based on stoichiometry and the amount of limiting reagent present before the reaction takes place. It represents the maximum amount of product that can be obtained in an ideal reaction.
The answer to QUESTION 14 is: FALSE.
Question 8 is the same kind as the first one you posted. Work it the same way.
For the others, posting multiple questions with one posts USUALLY results in nothing being answered because it takes too much time for a single post. You might consider posting these as single posts; however, I SUGGEST YOU SHOW HOW YOU THINK EACH SHOULD BE SOLVED OR TELL US EXACTLY WHAT YOU DON'T UNDERSTAND.