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3 years ago

What does two bonded flurione atoms form?

1 answer:

8 0

2 Fluorine atoms covalently bonded with each other, each sharing an equal number of a single, one valence electron to achieve a stable octet, would form a diatonic fluorine gas. It is a diatomic molecule, a molecule consisting of 2 atoms that are the same, in this case fluorine.

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Will mark BRAINLIEST!

Nataliya [291]

Answer:

Explanation:

2 NO2(g) ⇄ N2O4(g)

Adding Argon to this reaction will have NO effect. Catalysts nor inert gases have an affect on equilibrium conditions.

Only changes in concentration, temperature conditions and pressure-volume conditions (unless both sides have equal molar volumes) will affect the equilibria.

NH4OH(aq) ⇄ NH3(g) + H2O(l)

Removing ammonia from reaction equilibrium causes the reaction to shift right to replace removed ammonia. => Think of the reaction as being on a seesaw => removing ammonia from the product side tilts the seesaw left causing the NH₄OH to decompose and deliver more NH₃ and H₂O to the product side to increase weight on that side and level the seesaw. :-)

5 0

3 years ago

2. If the reaction of 5.75 moles of sodium with excess hydrofluoric acid is able to produce 2.49 mol H2, what is the percent yie

GuDViN [60]

Answer:

86.5%

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

2Na + 2HF –> 2NaF + H2

Next, we shall determine the theoretical yield of the hydrogen gas, H2. This is illustrated:

From the balanced equation above,

2 moles of Na reacted to produce 1 mole of H2.

Therefore, 5.75 moles of Na will react to produce = (5.75 x 1)/2 = 2.88 moles of H2.

Therefore, the theoretical yield of Hydrogen gas, H2 is 2.88 moles.

Finally, we shall determine the percentage yield of Hydrogen gas, H2. This can be obtained as follow:

Actual yield of H2 = 2.49 moes

Theoretical yield of H2 = 2.88 moles

Percentage yield of H2 =.?

Percentage yield = Actual yield /Theoretical yield x 100

Percentage yield = 2.49/2.88 x 100

Percentage yield = 86.5%

Therefore, the percentage yield of Hydrogen gas, H2 is 86.5%.

6 0

3 years ago

Convert 5.15 meters to inches

sukhopar [10]

Answer:

202.76 inches

Explanation:

1 meter = 39.37 inches

5.15 × 39.37 = 202.7559,when rounded it's 202.76

5 0

3 years ago

Why is it important to predict consequences when decision-making?

zavuch27 [327]

The correct answer is b

3 0

3 years ago

How many grams of CO2 are produced from 6.7 L of O2 gas at STP?

Tasya [4]

<h3>Answer:</h3>

13 g CO₂

<h3>General Formulas and Concepts:</h3>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Moles
STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

<u>Stoichiometry</u>

Using Dimensional Analysis

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<h3>Explanation:</h3>

<u>Step 1: Define</u>

<em>Identify variables</em>

[Given] 6.7 L O₂

[Solve] g O₂

<u>Step 2: Identify Conversions</u>

[STP] 22.4 L = 1 mol

[PT] Molar Mass of O: 16.00 g/mol

[PT] Molar Mass of C: 12.01 g/mol

Molar Mass of CO₂: 12.01 + 2(16.00) = 44.01 g/mol

<u>Step 3: Convert</u>

[DA] Set up: $\displaystyle 6.7 \ L \ O_2(\frac{1 \ mol \ O_2}{22.4 \ L \ O_2})(\frac{44.01 \ g \ O_2}{1 \ mol \ O_2})$
[DA] Divide/Multiply [Cancel out units]: $\displaystyle 13.1637 \ g \ O_2$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

13.1637 g CO₂ ≈ 13 g CO₂

5 0

3 years ago