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enot [183]
3 years ago
14

The _______________ react with the _______________ elements to form different compounds like lithium fluoride (LiF) and sodium c

hloride (NaCl). _______________ have a full valence level and do not combine with other elements.
Chemistry
1 answer:
likoan [24]3 years ago
8 0

Answer: Alkali metals, halogens, noble gases

Explanation:

Ionic compounds are made of ions- charges. In LiF and NaCl, the first element has a +1 and the second element has a charge of -1. Elements that are +1 are alkali metals and elements that are -1 are halogens. Noble gases have full octets in their outermost valence shell, and since they're full it's so stable so it doesn't react with anything.

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When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 20.4 g of carbon were burned in the presence of
Lilit [14]
<h3>Answer:</h3>

74.77 g

<h3>Explanation:</h3>

The equation for the reaction between carbon and Oxygen is given by;

C(s) + O₂(g) → CO₂(g)

We are given;

Mass of carbon 20.4 g

Mass of Oxygen is 66.2 g

Remaining mass of Oxygen after the reaction is 11.8 g

Therefore, Carbon is the rate limiting reagent since Oxygen was in excess.

We are required to calculate the mass of carbon dioxide produced.

<h3>Step 1: Moles of Carbon produced </h3>

Moles = Mass ÷ Molar mass

Molar mass of carbon = 12.01 g/mol

Therefore;

Moles of Carbon = 20.4 g ÷ 12.01 g/mol

                           = 1.699 moles

<h3>Step 2: Moles of carbon dioxide produced </h3>

From the equation, 1 mole of carbon reacts to produce 1 mole of carbon dioxide.

Therefore, the mole ratio of Carbon to carbon dioxide is 1 :1

Thus, moles of carbon dioxide = Moles of carbon

                                                  = 1.699 moles

<h3>Step 3: Mass of carbon dioxide produced </h3>

Mass = Moles × Molar mass

Molar mass of carbon dioxide = 44.01 g/mol

Therefore;

Mass = 1.699 moles × 44.01 g/mol

         = 74.77 g

Therefore, the mass of carbon dioxide gas produced is 74.77 g

6 0
3 years ago
What is the pressure of a gas if the volume is 96.2 L, the temperature is 25°C and there are 1.24 moles?
galben [10]

Answer:

0.315 atm

Explanation:

PV = nRT

P(96.2) = (1.24)(0.08206)(25 + 273)

P = 0.315 atm

6 0
3 years ago
Why are chemical equilibria called dynamic equilibria?
Serga [27]

Answer:

Because molecules are moving so they change from reactants to products and vice versa.

Explanation:

Hello,

In this case, it is widely known that chemical equilibrium is related with such condition at which the rate of consumption of reactants and formation of products tends to zero so their concentrations remain the same over the time. For instance, if we consider the formation of hydrogen chloride at equilibrium:

H_2+Cl_2\rightleftharpoons 2HCl

We can also see that the reactants, hydrogen and chlorine are consumed to form hydrogen chloride and it also goes back to its reactants in a dynamic equilibrium (because they are constantly changing).

Best regards.

4 0
3 years ago
A 1.167 grams sample of hydrated Nickel (II) Chloride is heated until a constant mass is achieved. The constant mass of the samp
svetoff [14.1K]

Answer:

NiCl₂·4H₂O, its name being nickel (II) chloride tetrahydrate.

Explanation:

The constant mass achieved after heating is the mass of anhydrous nickel (II) chloride, NiCl₂. While the mass lost was water.

  • Mass lost = 1.167 g - 0.750 g = 0.417 g

Now we <u>convert 0.750 g of NiCl₂ into moles</u>, using <em>its molar mass</em>:

  • 0.750 g NiCl₂ ÷ 129.6 g/mol = 0.0058 mol NiCl₂

Then we <u>convert 0.417 g of H₂O into moles</u>:

  • 0.417 g H₂O ÷ 18 g/mol = 0.0231 mol H₂O

With the above information we can calculate that the number of H₂O moles is 4 times higher than the number of NiCl₂ moles.

Meaning that <em>the formula of the hydrate is NiCl₂·4H₂O</em>, its name being nickel (II) chloride tetrahydrate.

6 0
3 years ago
Find Number of protons, neutrons and electrons in next atoms:
Dennis_Churaev [7]

Answer:

hi nice person. i need brain points sorry it not answer the question.

Explanation:

7 0
3 years ago
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