How many grams of Zn(NO3) are in 3.67 miles?

How many miles are in 68 grams of copper 2 hydroxide, Cu (OH)2

BabaBlast [244]

Molar mass Cu(OH)₂ = 97.561 g/mol

1 mol --------- 97.561 g
? mol ---------- 68 g

moles = 68 * 1 / 97.561

moles = 68 / 97.561

= 0.6969 moles

hope this helps!

8 0

3 years ago

A 20. 0-liter flask contains a mixture of argon at 0. 72 atmosphere and oxygen at 1. 65 atmospheres. What is the total pressure

exis [7]

The total pressure of the system is equivalent to the sum of all the pressure of the individual gases. The total pressure of the flask is 2.37 atm.

<h3>What is total pressure?</h3>

According to Dalton's law, the total pressure of the system will be equivalent to the total of the pressures exerted by the individual gases present in the system.

The total pressure of gases is given as,

$\rm P = P_{1} +P_{2}+ P_{3}.....P_{n}$

Given,

The pressure of argon gas = 0.72 atm
The pressure of oxygen = 1.65 atm
Total pressure = P

Substituting values in the above equation:

$\begin{aligned}\rm P &= 0.72 + 1.65\\\\&=2.37\;\rm atm\end{aligned}$

Therefore, 2.37 atm is the total pressure of the flask.

Learn more about total pressure here:

brainly.com/question/11150092

5 0

3 years ago

How many moles are there in 2.00 x 10^19 molecules of CCl4

HACTEHA [7]

Answer: 0.0000332mol

Explanation: 1mole of CCl4 contains 6.02x10^23 molecules.

Therefore, X mol of CCl4 will contain 2 x 10^19 molecules i.e

Xmol of CCl4 = 2 x 10^19/ 6.02x10^23 = 0.0000332mol

7 0

3 years ago

A sample of calcium phosphate was found to have a mass of 125.3 g. How many molecules were contained in the sample?

Viktor [21]

The answer for the following problem is mentioned below.

Therefore number of molecules(N) present in the calcium phosphate sample are 19.3 × 10^23 molecules.

Explanation:

Given:

mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 125.3 grams

We know;

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = (40×3) + 3 (31 +(4×16))

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 120 + 3(95)

molar mass of calcium phosphate ( $Ca_{3}(PO_{4} )_{2}$ ) = 120 +285 = 405 grams

We also know;

No of molecules at STP conditions( $N_{A}$ ) = 6.023 × 10^23 molecules

To solve:

no of molecules present in the sample(N)

We know;

$\frac{m}{M} =\frac{N} }{}$ N÷ $N_{A}$

$\frac{405}{125.3}$ = $\frac{N}{6.023*10^23}$

N =(405×6.023 × 10^23) ÷ 125.3

N = 19.3 × 10^23 molecules

Therefore number of molecules(N) present in the calcium phosphate sample are 19.3 × 10^23 molecules

3 0

3 years ago

Draw the best Lewis structure for NH3 by filling in the bonds, lone pairs, and formal charges. (Assign bonds, lone pairs, radica

kiruha [24]

Answer : The Lewis-dot structure of $NH_3$ is shown below.

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

The given molecule is, $NH_3$

As we know that hydrogen has '1' valence electron and nitrogen has '5' valence electrons.

Therefore, the total number of valence electrons in $NH_3$ = 5 + 3(1) = 8

According to Lewis-dot structure, there are 6 number of bonding electrons and 2 number of non-bonding electrons.

Now we have to determine the formal charge for each atom.

Formula for formal charge :

$\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}$

$\text{Formal charge on N}=5-2-\frac{6}{2}=0$

$\text{Formal charge on }H_1=1-0-\frac{2}{2}=0$

$\text{Formal charge on }H_2=1-0-\frac{2}{2}=0$

$\text{Formal charge on }H_3=1-0-\frac{2}{2}=0$

Hence, the Lewis-dot structure of $NH_3$ is shown below.

3 0

3 years ago