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RideAnS [48]
3 years ago
7

16. Relevant information is knowledge that relates to the question. True or false

Chemistry
1 answer:
Serggg [28]3 years ago
3 0

Answer:

True

Explanation:

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Which of the following is true of gases?
sweet-ann [11.9K]
The most logical answer is d
3 0
3 years ago
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Compound X has a molar mass of 266.64 g/mol and the following composition: aluminum 20.24% chlorine 79.76% Write the molecular f
N76 [4]

Answer:

Explanation:

Assume we have 100g of this substance. That means we would have 20.24g of Cl and 79.76g of Al. Now we can find how many moles of each we have:

\frac{79.76 \:g}{35.45 \: g/mol} = 2.25 mol of chlorine

\frac{20.24 \: g}{26.98 \: g/mol} = 0.750 mol of Al.

To form a integer ratio, do 2.25/0.75 = 2.99999 ~= 3.

So the ratio is essentially Al : Cl => 1 : 3. To the compound is possibly AlCl_3.

However, it says it has a molar mass of 266.64 g/mol, and since AlCl3 has a molar mass of 133.32, it must be Al_2Cl_6.

Actually this molecule isn't exactly AlCl3 (which is ionic). Al2Cl6 forms a banana bond where Cl acts as a hapto-2 ligand. But that's a bit advanced. All you need to know is X = Al2Cl6

5 0
3 years ago
An isotope of an element has a mass number of 129 and it has 74 neutrons. How many
Viktor [21]

Answer:

Explanation:

tiene 74 protones

6 0
3 years ago
Which types of atomic orbitals of the central atom mix to form hybrid orbitals in:<br> (c) PF₅;
zloy xaker [14]

The atomic orbitals of the central atom mix to form hybrid orbitals are one s and three p.

<h3>Which atomic orbitals are used to form hybrid orbitals?</h3>

Pauling supposed that in the presence of four hydrogen atoms, the s and p orbitals form four equivalent combinations which he called hybrid orbitals.

<h3>How many bonds does PF5?</h3>

Phosphorus pentafluoride has 5 regions of electron density around the central phosphorus atom (5 bonds, no lone pairs).

The resulting shape is a trigonal bipyramidal in which three fluorine atoms occupy equatorial and two occupy axial positions.

Learn more about PF5 here:

<h3>brainly.com/question/1565926</h3><h3 /><h3>#SPJ4</h3>
5 0
2 years ago
A sample of gas contains 0.1900 mol of CO(g) and 0.1900 mol of NO(g) and occupies a volume of 22.0 L. The following reaction tak
worty [1.4K]

Answer:

V₂ = 16.5 L

Explanation:

To solve this problem we use <em>Avogadro's law, </em>which applies when temperature and pressure remain constant:

V₁/n₁ = V₂/n₂

In this case, V₁ is 22.0 L, n₁ is [mol CO + mol NO], V₂ is our unknown, and n₂ is [mol CO₂ + mol N₂].

  • n₁ = mol CO + mol NO = 0.1900 + 0.1900 = 0.3800 mol

<em>We use the reaction to calculate n₂</em>:

2CO(g) + 2NO(g) → 2CO₂(g) + N₂(g)

  • mol CO₂:

0.1900 mol CO * \frac{2molCO_{2}}{2molCO} = 0.1900 mol CO₂

  • mol N₂:

0.1900 mol NO * \frac{1molN_{2}}{2molNO} = 0.095 mol N₂

  • n₂ = mol CO₂ + mol N₂ = 0.1900 + 0.095 = 0.2850 mol

Calculating V₂:

22.0 L / 0.3800 mol = V₂ / 0.2850 mol

V₂ = 16.5 L

3 0
4 years ago
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