Weak acids

Electricity is the _of charged<br> particles.<br> A.movement<br> B. collection<br> C.build up

Vitek1552 [10]

Answer:

c

Explanation:

4 0

3 years ago

Q3. A student wanted to make blue copper sulfate crystals from green copper carbonate powder

CaHeK987 [17]

Heat the sulfuric acid solution and adding copper carbonate in it.

<h3>Improvement require in this experiment</h3>

The method could be improved by heating sulfuric acid solution and add copper carbonate into the solution of sulfuric acid. Add the copper carbonate until it is present in excess amount. After that filter the extra amount of copper carbonate so in this way the blue copper sulfate crystals are produced.

Learn more about copper here: brainly.com/question/3157958

5 0

2 years ago

a ______ consumer is a heterotroph that directly eats an autotroph. A primary B. Quaterany C tertiary D secondary

Softa [21]

Primary consumer just remember the “primary” (first) consumer so the one that eats a heterotroph

6 0

3 years ago

Compare the root mean square speeds of O2 and UF6 at 65 degree Celsius

gayaneshka [121]

<h3>Answer:</h3>

The root mean square speeds of O₂ and UF₆ is 513m/s and 155 m/s respectively.

<h3>Solution and Explanation:</h3>

To find how fast molecules or particles of gases move at a particular temperature, the root mean square speed is calculated.
Root mean square speed of a gas is calculated by using the formula;

$Root mean square=\sqrt{ \frac{3RT}{M}$

Where R is the molar gas constant, T is the temperature and M is the molar mass of gas in Kg.

<h3>Step 1: Root mean square speed from O₂</h3>

Molar mass of Oxygen is 32.0 g/mol or 0.032 kg/mol

Temperature = 65 degrees Celsius or 338 K

Molar gas constant = 8.3145 J/k.mol

$Root mean square speed = \sqrt\frac{(3)(8.3145)(338K)}{0.032}$

$= 513.289 m/s$

<h3>Step 2: Root mean square speed of UF₆ </h3>

The molar mass of UF₆ is 352 g/mol or 0.352 kg/mol

$Root mean square speed = \sqrt\frac{(3)(8.3145)(338K)}{0.352}$

$= 154.762m/s$

Therefore; the root mean square speeds of O₂ and UF₆ is 513m/s and 155 m/s respectively.

7 0

3 years ago

Many computer chips are manufactured from silicon, which occurs in nature as SiO2 . When SiO2 is heated to melting, it reacts wi

Ierofanga [76]

Answer:

a. Theoretical yield of Si = <u>72.58 kg</u>

b. Percent Yield =<u> 91.2 %</u>

Explanation:

The chemical reaction involved is: SiO₂ (l) + 2C (s) → Si (l) + 2CO (g)

The stoichiometric ratio = 1 mol SiO₂ ÷ 2 mol C = 0.5 mol SiO₂ ÷ 1 mol C

Given: mass of SiO₂: w₁ = 155.3kg = 155.3 × 10³g, mass of C: w₂ = 79.3kg = 79.3 × 10³g, mass of Si: w₃ = 66.2kg = 66.2 × 10³g (∵ 1 kg =1000g)

Molar mass of SiO₂: m₁ = 60.08 g/mol, atomic mass of C: m₂ = 12.01 g/mol, atomic mass of Si: m₃ = 28.08 g/mol

Number of moles of SiO₂ taken: n₁ = w₁ ÷ m₁ = 155300 g ÷ 60.08 g/mol = 2584.88 mol

Number of moles of C taken: n₂ = w₂ ÷ m₂ = 79300 g ÷ 12.01 g/mol = 6602.83 mol

Actual ratio = n₁ ÷ n₂ = 2584.88 mol SiO₂ ÷ 6602.83 mol C = 0.39 mol SiO₂ ÷ 1 mol C

Since the stoichiometric ratio > actual ratio

<u>Therefore, SiO₂ is the limiting reagent.</u>

<u />

Now, the mass of SiO₂ in 1 mol = number of moles × molar mass = 1 mol × 60.08 g/mol = 60.08 g

the mass of Si in 1 mol = number of moles × molar mass = 1 mol × 28.08 g/mol = 28.08 g

So 28.08 g of Si is produced from 60.08 g SiO₂

Therefore, the amount of Si produced from 155300 g SiO₂ = 155300 g × 28.08 g ÷ 60.08 g = 72583.62 g = 72.58 kg

<u>Therefore, the </u><u>theoretical yield</u><u> of Si = 72.58 kg</u>

<u>Actual yield</u><u> of Si = 66.2 kg</u>

Therefore,<u> </u><u>Percent Yield</u><u> </u>= Actual yield ÷ Theoretical yield × 100 = 66.2 kg ÷ 72.58 kg × 100 =<u> 91.2 %</u>

3 0

3 years ago