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2 years ago

Zn-64 = 48.63%

Chemistry

1 answer:

Ann [662]2 years ago

5 0

Answer:

A = 65.46 u

Explanation:

Given that,

The composition of zinc is as follows :

Zn-64 = 48.63%

Zn-66 = 27.90%

Zn-67 = 4.10%

Zn-68 = 18.75%

Zn-70 = .62%

We need to find the average atomic mass of the given element. It can be solved as follows :

$A=\dfrac{48.63\times 64+27.90\times 66+4.1\times 67+18.75\times 68+0.62\times 70}{100}\\A=65.46\ u$

So, the average atomic mass of zinc is 65.46 u.

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A sample of the compound magnesium oxide is synthesized as follows. 60. g of magnesium is burned and produces 100. g of magnesiu

Inga [223]

Answer:

30 g of magnesium would be combined with 20 g of oxygen. The law used solving this problem is the Lavoisier Law of conservation of mass.

Explanation:

If 60 g of magnesium combines with 40 g of oxygen to make 100 g of magnesium oxide, then 30 g of magnesium will combine with 20 g of oxygen to make 50 g of magnesium oxide.

This happens because in a chemical reaction there is no creation or descruction of atoms, only a rearrangement. Therefore, the mass of reactants should be equal to the mass of products.

The following equation represents the proportions of the substances:

Mg + 1/2O₂ → MgO

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3 years ago

A pure gold bar is made up of only particles. A.nickel B.copper C.god D.gold

Minchanka [31]

Answer: gold

Explanation:

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3 years ago

The density of benzene is 0.879g/mL. The volume (with 1 decimal) of 131.9g sample of benzene is how many mL?

timurjin [86]

Answer:

150.1 mL

Explanation:

Step 1: Given data

Density of benzene (ρ): 0.879 g/mL

Mass of the sample of benzene (m): 131.9 g

Volume of the sample of benzene (V): ?

Step 2: Calculate the volume of the sample of benzene

Density is an intrinsic property. It is equal to the quotient between the mass and the volume of the sample of benzene.

ρ = m/V

V = m/ρ

V = 131.9 g/(0.879 g/mL)

V = 150.1 mL

5 0

3 years ago

How do scientists determine locations for drilling for natural gas? Where are many natural gas drill sites located? (Site 2)

Alchen [17]

Explanation:

By drilling several cores miles apart , geologist can correlate the rock units and create an image what exists and where below the surface.

Combining this information with rocks exposed to the surface , which can gives clues about rock orientation below, can be a powerful tool to locating oil and gas .

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2 years ago

If the solubility of sodium chloride is 36 grams per 100 grams of water, which of the following solutions would be considered un

Murrr4er [49]

Answer: If the solubility of sodium chloride is 36 grams per 100 grams of water then 5.8 moles of NaCl dissolved in 1 L of water solution would be considered unsaturated.

Explanation:

A solution which contains the maximum amount of solute is called a saturated solution. Whereas a solution in which more amount of solute is able to dissolve is called an unsaturated solution.

Now, the number of moles present in 36 g of NaCl (molar mass = 58.4 g/mol) is as follows.

$No. of moles = \frac{mass}{molar mass}\\= \frac{36 g}{58.4 g/mol}\\= 0.616 mol$

This shows that solubility of sodium chloride is 36 grams per 100 grams of water means a maximum of 0.616 mol of NaCl will dissolve in 100 mL of water.

So, a solution in which number of moles of NaCl are less than 0.616 mol per 100 mL then the solution formed will be an unsaturated solution.

As 5.8 moles of NaCl dissolved in 1 L (or 1000 mL) of water. So, moles present in 100 mL are calculated as follows.

$Moles = \frac{5.8 mol}{1000 mL} \times 100 mL\\= 0.58 mol$

Moles present in 100 mL of water for 3.25 moles of NaCl dissolved in 500 ml in water are as follows.

$Moles = \frac{3.25 mol}{500 mL} \times 100 mL\\0.65 mol$

Moles present in 100 mL of water for 1.85 moles of NaCl dissolved in 300 ml of water are as follows.

$Moles = \frac{1.85 mol}{300 mL} \times 100 mL\\= 0.616 mol$

Thus, we can conclude that if the solubility of sodium chloride is 36 grams per 100 grams of water then 5.8 moles of NaCl dissolved in 1 L of water solution would be considered unsaturated.

8 0

3 years ago