Volume of 1 mole of any gas under STP = 22.4 L,
so
0.15 mol*22.4 L/1 mol = 3.36 L of H2
Answer:
The answer to your question is False.
Explanation:
Data
1 mole of NH₄NO₃
0.75 moles of N₂O
Percent yield = 25%
Chemical reaction
NH₄NO₃ ⇒ N₂O + 2H₂O
Process
1.- Determine the theoretical yield
1 mol NH₄NO₃ ------------- 1 mol of N₂O
2.- Calculate the percent yield
Percent yield = Actual yield / Theoretical yield x 100
-Substitution
Percent yield = 0.75 / 1 x 100
-Simplification
Percent yield = 0.75 x 100
-Result
Percent yield = 75%
Conclusion
False, the actual percent yield is 75%
Answer:
1.50 g
Explanation:
The heat absorbed by the aluminum in this case is:
q = m x C x ΔT m= q/ (C x ΔT)
q= 9.86 J
C = 0.90 J/g-K
ΔT = ( 30.5 ºC - 23.2 ºC ) = 7.3 ºC = 7.3 K (this is a range of temperature)
m = 9.86 J / ( 0.90 J/g-K ) x 7.3 K ) = 1.50 g
Answer:
the correct answer is option 'b': More than
Explanation:
The 2 situations are represented in the attached figures below
When an object is placed in air it is acted upon by force of gravity of earth which is measured as weight of the object.
While as when any object is submerged partially or completely in any fluid the fluid exerts a force in upward direction and this force is known as force of buoyancy and it's magnitude is given by Archimedes law as equal to the weight of the fluid that the body displaces, hence the effective force in the downward direction direction thus the apparent weight of the object in water decreases.
Answer:
Explanation:
At constant pressure and temperature, the mole ratio of the gases is equal to their volume ratio (a consequence of Avogadro's law).
Hence, the <em>complete combustion reaction</em> that has a ratio of 100 ml of gaseous hydrocarbon to 300 ml of oxygen, is that whose mole ratio is 1 mol hydrocarbon : 3 mol of oxygen.
Then, you must write the balanced chemical equations for the complete combustion of the four hydrocarbons in the list of choices, and conclude which has such mole ratio (1 mol hydrocarbon : 3 mol oxygen).
A complete combustion reaction of a hydrocarbon is the reaction with oxygen that produces CO₂ and H₂O, along with the release of heat and light.
<u>a. C₂H₄:</u>
- C₂H₄ (g) + 3O₂ (g) → 2CO₂(g) + 2H₂O (g)
Precisely, for this reaction the mole ratio is 1 mol C₂H₄: 2 mol O₂, hence, this is the right choice.
The following analysis just shows that the other options are not right.
<u>b. C₂H₂:</u>
- 2C₂H₂ (g) + 5O₂ (g) → 4CO₂(g) + 2H₂O (g)
The mole ratio for this reaction is 2 mol C₂H₂ :5 mol O₂.
<u>с. С₃Н₈</u>
- C₃H₈ (g) + 5O₂ (g) → 3CO₂(g) + 4H₂O (g)
The mole ratio is 1 mol C₃H₈ : 5 mol O₂
<u>d. C₂H₆</u>
- 2C₂H₆ (g) +7 O₂ (g) → 4CO₂(g) + 6H₂O (g)
The mole ratio is 2 mol C₂H₆ : 7 mol O₂
