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Makovka662 [10]
3 years ago
6

What volume of beaker contains exactly 2.23x10^-2 mol of nitrogen gas at STP?

Chemistry
1 answer:
nikklg [1K]3 years ago
4 0

Answer:

V = 0.5 L

Explanation:

Given data:

Moles of nitrogen = 2.23×10⁻² mol (0.0223 mol)

Temperature = 273 K

Pressure = 1 atm

Volume = ?

Solution:

PV = nRT

V = nRT / P

V = 0.0223 mol × 0.0821 atm. mol⁻¹. L . k⁻¹ × 273 K / 1 atm

V = 0.5 L

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Eva8 [605]

Answer:

Atom, Sub atomic particle, compound, molecule

7 0
2 years ago
Give the percent yield when 162.8 g of CO2 are formed from the reaction of excess amount of
Zepler [3.9K]

Answer:

84.86%

Explanation:

Step 1:

We'll begin by writing a balanced equation for the reaction between C8H18 and O2 to produce CO2. This is illustrated below:

2C8H18 + 25O2 —> 16CO2 + 18H2O

Step 2:

Now, let us calculate the mass of O2 that reacted and the mass of CO2 produced from the balanced equation above. This is illustrated below:

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 25 x 32 = 800g

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Mass of CO2 from the balanced equation = 16 x 44 = 704g

Therefore the mass of O2 that reacted from the balanced equation is 800g

The mass of CO2 produced from the balanced equation is 704g

Step 3:

Determination of the theoretical yield of CO2. This is illustrated below:

From the balanced equation above,

800g of O2 reacted to produced 704g of CO2.

Therefore, 218g of O2 will react to produce = (218 x 704)/800 = 191.84g of CO2.

Therefore, the theoretical yield of CO2 is 191.84g

Step 4:

Determination of the percentage yield of CO2. This is illustrated below:

Actual yield = 162.8g

Theoretical yield = 191.84g

Percentage yield =?

Percentage yield = Actual yieldm/Theoretical yield x100

Percentage yield = 162.8/191.84 x100

Percentage yield = 84.86%

Therefore, the percentage yield of CO2 is 84.86%

6 0
3 years ago
Read 2 more answers
What is the hardest subject u ever taking, mine is chemistry
artcher [175]

Answer:

Mine is language arts brainliest?

Explanation:

7 0
2 years ago
Acetylene (c2h2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. given δh°f[co2(g)] = –393.5
Brums [2.3K]
Answer is: 13181,7 kJ of energy <span>is released when 10.5 moles of acetylene is burned.
</span>Balanced chemical reaction: C₂H₂ + 5/2O₂ → 2CO₂ + H₂O.
<span>ΔHrxn = sum of ΔHf (products of reaction) - sum of ΔHf (reactants).</span><span>
Or ΔHrxn = ∑ΔHf (products of reaction) - ∑ΔHf (reactants).
ΔHrxn - enthalpy change of chemical reaction.
<span>ΔHf - enthalpy of formation of reactants or products.
</span></span>ΔHrxn = (2·(-393,5) + (-241,8)) - 226,6 · kJ/mol.
ΔHrxn = -1255,4 kJ/mol.
Make proportion: 1 mol (C₂H₂) : -1255,4 kJ = 10,5 mol(C₂H₂) : Q.
Q = 13181,7 kJ.
8 0
3 years ago
May someone help me on this
Kamila [148]

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