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ss7ja [257]
3 years ago
15

What is the % by volume of 50mL of ethylene glycol dissolved in 950mL of H2O?

Chemistry
1 answer:
MariettaO [177]3 years ago
5 0

Answer:

5.0 %

Explanation:

Given data

  • Volume of ethylene glycol (solute): 50 mL
  • Volume of water (solvent): 950 mL

Step 1: Calculate the volume of solution

If we assume that <em>the volumes are additive</em>, the volume of the solution is equal to the sum of the volume of the solute and the solvent.

V = 50 mL + 950 mL = 1000 mL

Step 2: Calculate the percent by volume

We will use the following expression.

\% v/v = \frac{volume\ of\ solute}{volume\ of\ solution} \times 100 \%  = \frac{50mL}{1000mL} \times 100 \% = 5.0\%

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In the reaction C + O2 → CO2, 18 g of carbon react with oxygen to produce 72 g of carbon dioxide. What mass of oxygen would be n
melamori03 [73]

Answer:

54 g

Explanation:

Given data:

Mass of carbon = 18 g

Mass of CO₂ = 72 g

Mass of oxygen needed = ?

Solution:

Chemical reaction:

C + O₂     →       CO₂

according to law of conservation mass, mass can neither be created nor destroyed in a chemical equation.

This law was given by French chemist  Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.

In given photosynthesis reaction:

6CO₂ + 6H₂O + energy → C₆H₁₂O₆ + 6O₂

there are six carbon atoms, eighteen oxygen atoms and twelve hydrogen atoms on the both side of equation so this reaction followed the law of conservation of mass.

In a similar way,

C   +    O₂     →       CO₂

18 g +   X      = 72

X = 72 -18

X = 54 g

Thus, 54 g of O₂ are required.

3 0
2 years ago
Read 2 more answers
A helium balloon is filled on the ground where the atmospheric pressure is 768 torr. The volume of the balloon is 8.00 m3. When
Anvisha [2.4K]

Answer:

The correct option is: <u>B. 366 torr</u>

Explanation:

Given: <u>On the ground</u>- Initial Volume: V₁ = 8.00 m³, Initial Atmospheric Pressure: P₁= 768 torr;

<u>At 4200 m height</u>- Final Volume: V₂ = 16.80 m³, Final Atmospheric Pressure: P₂ = ?

Amount of gas: n, and Temperature: T = constant

<u>According to the Boyle's Law</u>, for a given amount of gas at constant temperature:         P₁ V₁ = P₂ V₂

⇒  P₂ = P₁ V₁ ÷ V₂

⇒  P₂ = [(768 torr) × (8.00 m³)] ÷ (16.80 m³)

⇒  P₂ = 365.71 torr ≈ 366 torr

<u>Therefore, the final air pressure at 4200 m height: P₂ = 366 torr.</u>

6 0
3 years ago
12. How is the melting point of a substance related to its freezing point? Both indicate the temperature at which the solid and
krok68 [10]
Both indicate the temperature at which the solid and liquid states of a substance are in equilibrium would be your answer.

This is beacause the melting point of a substance is the same as the freezing point of a substance. At this particular temp, the substance can be either a solid or a liquid. 

hope this helps!
8 0
3 years ago
Read 2 more answers
Si se tiene 1mol de NO . cuantas moleculas de NO hay
kumpel [21]

if you have 1mol of NO. how many molecules of NO are there

Answer:

6.02 x 10²³ molecules

Explanation:

Given parameters:

Number of moles of NO = 1 mole

Unknown:

Number of molecules in NO;

Solution:

A mole of compound contains the Avogadro's number of particles.

  1 mole of a substance contains 6.02 x 10²³ molecules

So, 1 mole of NO contained 6.02 x 10²³ molecules

3 0
2 years ago
One of the hydrates of MnSO4 is manganese(II) sulfate tetrahydrate . A 71.6 gram sample of MnSO4 4 H2O was heated thoroughly in
Dennis_Churaev [7]

Answer:

48.32 g of anhydrous MnSO4.

Explanation:

Equation of dehydration reaction:

MnSO4 •4H2O --> MnSO4 + 4H2O

Molar mass = 55 + 32 + (4*16) + 4((1*2) + 16)

= 223 g/mol

Mass of MnSO4 • 4H2O = 71.6 g

Number of moles = mass/molar mass

= 71.6/223

= 0.32 mol.

By stoichiometry, since 1 mole of MnSO4 •4H2O is dehydrated to give 1 mole of anhydrous MnSO4

Number of moles of MnSO4 = 0.32 mol.

Molar mass = 55 + 32 + (4*16)

= 151 g/mol.

Mass = 151 * 0.32

= 48.32 g of anhydrous MnSO4.

3 0
2 years ago
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