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Zinaida [17]
2 years ago
14

How many moles of Hydrogen gas will be produced if you start with 2.5 moles of Magnesium and an excess of Hydrochloric Acid give

n the following balanced chemical reaction:
Mg + 2HCl → MgCl2 + H2

Group of answer choices

A. 1.25 moles

B. 5.0 Moles

C. 7.5 moles

D. 2.5 moles
Chemistry
1 answer:
nadezda [96]2 years ago
7 0

Taking into account the reaction stoichiometry, 1.25 grams of H₂ (option A) are formed if you start with 2.5 moles of Magnesium and an excess of Hydrochloric Acid.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

Mg + 2 HCl  → MgCl₂ + H₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • Mg: 1 mole
  • HCl: 2 moles
  • MgCl₂: 1 mole
  • H₂: 1 mole

<h3>Mass of hydrogen formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 2 moles of Mg form 1 mole of H₂, 2.5 moles of Mg form how many moles of H₂?

moles of H_{2} =\frac{2.5 moles of Mgx1 mole of H_{2} }{2 moles of Mg}

<u><em>moles of H₂= 1.25 moles</em></u>

Finally, 1.25 grams of H₂ (option A) are formed if you start with 2.5 moles of Magnesium and an excess of Hydrochloric Acid.

Learn more about the reaction stoichiometry:

brainly.com/question/24741074

brainly.com/question/24653699

#SPJ1

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A compound is composed of 58.8% c, 9.8% h, and 31.4% o, and the molar mass is 102 g/mol. what is the molecular formula for this
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The solution would be like this for this specific problem:

 

<span>Moles of carbon = 58.8 / 12 = 4.9 </span><span>
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</span><span>I hope this helps and if you have any further questions, please don’t hesitate to ask again.</span>
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1) When 2.38g of magnesium is added to 25.0cm of 2.27 M hydrochloric acid, hydrogen gas is released.
Andrej [43]

Answer:

a. HCl.

b. 0.057 g.

c. 1.69 g.

d. 77 %.

Explanation:

Hello!

In this case, since the reaction between magnesium and hydrochloric acid is:

Mg+2HCl\rightarrow MgCl_2+H_2

Whereas there is 1:2 mole ratio between them.

a) Here, we can identify the limiting reactant as that yielded the fewest moles of hydrogen gas product via the 1:1 and 2:1 mole ratios:

n_{H_2}^{by\  HCl}=0.025L*2.27\frac{molHCl}{1L}*\frac{1molH_2}{2molHCl}  =0.0284molH_2\\\\n_{H_2}^{by\  Mg}=2.38gMg*\frac{1molMg}{24.3gMg}*\frac{1molH_2}{1molMg}=0.0979molH_2

Thus, since hydrochloric yields fewer moles of hydrogen than magnesium, we realize it is the limiting reactant.

b) Here, we use the molar mass of gaseous hydrogen (2.02 g/mol) to compute the mass:

m_{H_2}=0.0284molH_2*\frac{2.02gH_2}{1molH_2}=0.057gH_2

c) Here, we compute the mass of magnesium associated with the yielded 0.0248 moles of hydrogen:

m_{Mg}^{reacted}=0.0284molH_2*\frac{1molMg}{1molH_2}*\frac{24.3gMg}{1molMg}  =0.690gMg

Thus, the mass of excess magnesium turns out:

m_{Mg}^{excess}=2.38g-0.690g=1.69gMg

d) Finally, we compute the percent yield, considering 0.044 g is the actual yield and 0.057 g the theoretical yield:

Y=\frac{0.044g}{0.057g} *100\%\\\\Y=77\%

Best regards!

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