3 years ago

ASAP! I have 20 min to finish this i need help

Chemistry

1 answer:

rodikova [14]3 years ago

7 0

The real answer is B

You might be interested in

In a laboratory experiment, John uses a mesh to separate soil particles from water. Which technique of separation is he using?

m_a_m_a [10]

Correct answer -->filtration

8 0

3 years ago

How many moles of electrons is required to deposit 5.6g of iron from a solution of iron (2) tetraoxosulphate(6)

yuradex [85]

Answer:

0.20 mol

Explanation:

Let's consider the reduction of iron from an aqueous solution of iron (II).

Fe²⁺ + 2 e⁻ ⇒ Fe

The molar mass of Fe is 55.85 g/mol. The moles corresponding to 5.6 g of Fe are:

5.6 g × 1 mol/55.85 g = 0.10 mol

2 moles of electrons are required to deposit 1 mole of Fe. The moles of electrons required to deposit 0.10 moles of Fe are

0.10 mol Fe × 2 mol e⁻/1 mol Fe = 0.20 mol e⁻

7 0

3 years ago

If you dissolve 50.0 grams of potassium bromide in 100.0g of water what is the mass percent of the resultant solution?

tatiyna

Mass percent= grams solute/ grams of solution x 100

Mass Percent= (50/ 150)x100= 33.3%

7 0

2 years ago

What is the mass of 8.12 × 10^23 molecules of CO2 gas? (Atomic mass of carbon = 12.011 u; oxygen = 15.999 u.)

amid [387]

Answer:

$m=59.3gCO_2$

Explanation:

Hello,

In this case, the first step is to compute the molar mass of carbon dioxide as shown below, considering it has one carbon atom and two oxygen atoms:

$M=12.011g/mol+2*15.999g/mol\\\\M=44.009g/mol$

It is important to notice it is the mass in one mole of such compound. Afterwards, we need to use the Avogadro's number to compute the how many moles are in the given molecules of carbon dioxide as shown below:

$mol=8.12x10^{23}molec*\frac{1mol}{6.022x10^{23}molec} =1.35mol$

Finally, the mass by using the molar mass:

$m=1.35mol*\frac{44.009g}{1mol} \\\\m=59.3gCO_2$

Best regards.

4 0

2 years ago

An alloy is made up of more than one type of what?

pychu [463]

More than one type of metallic elements.

4 0

3 years ago