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3 years ago

Last week at a tax free sale, Ms. Kuhn bought 4 shirts for $15.95 each and 2 new belts

Chemistry

1 answer:

erastovalidia [21]3 years ago

3 0

Answer:

$18.30

Explanation:

The change is the amount left over after the selling price has been matched by the buyer.

Let us find the total cost of what of Ms. Kuhn bought;

For the shirt;

Cost = 4 shirts for $15.95 each = 4(15.95) = $63.8

2 new belts for $8.95 each = 2(8.95) = $17.9

Total cost = $63.8 + $17.9 = $81.7

The amount of change left = $100 - $81.7 = $18.3

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Lemonade is an example of a compound because the particles retain their original chemical properties and identity.

Ksenya-84 [330]

Answer:

False

Explanation:

Compounds are chemically combined

lemonade is not

If the squeezed lemonade is made by squeezing lemons to extract the juice and mixing it with water and sugar, it would be a homogenous mixture.

If it contains a pulp than it would be heterogeneous

4 0

4 years ago

Consider the reaction for the combustion of benzene: 2 C6H6(g) 15 O2(g) ---> 12 CO2(g) 6 H2O(l) What mass of H2O is produced

irakobra [83]

Answer: Mass of water produced is 17.3 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For benzene:

Given mass of benzene = 25.0 g

Molar mass of benzene= 78 g/mol

Putting values in equation 1, we get:

$\text{Moles of benzene}=\frac{25.0g}{78g/mol}=0.32mol$

The chemical equation for the reaction follows:

$2C_6H_6(g)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(l)$

As, oxygen is an excess reagent. Thus benzene is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of benzene produces 6 moles of water

So, 0.32 moles of benzene will produce = $\frac{6}{2}\times 0.32=0.96moles$ of water

Now, calculating the mass of water from equation 1, we get:

Molar mass of water= 18 g/mol

Moles of water = 0.96moles

Putting values in equation 1, we get:

$0.96mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=17.3g$

Thus mass of water produced is 17.3 grams

3 0

3 years ago

What mass of naturally occurring uranium is closer to 238 u , 235 u or 234 u?

Liono4ka [1.6K]

Uranium (92U) is a naturally occurring radioactive element that has no stable isotopes but two primordial isotopes (uranium-238 and uranium-235) that have long half-life and are found in appreciable quantity in the Earth's crust, along with the decay product uranium-234.

7 0

3 years ago

Anything in red is the question

solmaris [256]

Answer:

19. C₂H₂, HF, and H₂O₂ are molecular compounds

20. The formula is CuSO₄. 5H₂O

Explanation:

Question 19.

The three the chemical formulae in red, C₂H₂, HF, and H₂O₂, represent compounds because a compound is the chemical union of two or more atoms of different kind.

The chemical union is done either by ionic bonds or covalent bonds.

C, H, F, and O are all non-metal elements. Non-metals combine each other through covalent bonds, which is the bond in which electrons are shared to complete the valence shell. Ionic bonds are formed by the electrostatic atraction between ions of different charge and is typical of the bond between a metal and a non-metal.

Thus, all the bonds are covalent and the compounds are molecular compounds.

Question 20.

You can determine the chemical formula using the molar masses of both Copper(II) sulfate and water.

Molar mass of copper(II) sulfate: 159.609 g/mol
Molar mass of water: 18.015 g/mol

Call n the number of water molecules in the molecular formula:

CuSO₄ . nH₂O

The ratio of water to copper(II) sulfate is:

n × molar mass of water / molar mass of the compound

n × 18.015 / (n × 18.015 + 159.609) = 36%

18.015n = 0.36(18.015n + 159.609)

18.015n = 6.4854n + 57.45924

11.5296n = 57.45924

n = 4.9836 ≈ 5

Therefore, the formula of the hydrate contains 5 molecules of water and it is CuSO₄.5H₂O.

8 0

3 years ago

Each of the following is a sign of economic freedom EXCEPT:

MAVERICK [17]

Answer:

Explanation:

7 0

3 years ago