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4 years ago

How many moles of coF3 are produced when 1.25 moles of 3co reacts

Chemistry

2 answers:

oee [108]4 years ago

7 0

Answer:

1.25 moles

Explanation:

First, we need to balance the equation. Essentially, this means making sure we have the same number of each atom on each side.

On the left side, we currently have:

- 1 Co atom

- 2 F aomts

On the right side, we have:

- 1 Co atom

- 3 F atoms

To balance it, add a 2 to Co on the left, 3 to F2 on the left, and 2 to CoF3 on the right:

$2Co+3F_2$ → $2CoF_3$

Now, we have 1.25 moles of Co, and since the ratio between Co and CoF3 is 1:1, we also have 1.25 moles of CoF3.

Thus, the answer is 1.25 moles.

Sloan [31]4 years ago

3 0

Answer:

1.25 moles

Explanation:

Balancing the equation:

2Co + 3F2 --> 2CoF3

Co : CoF3

2 : 2

1.25 : X

X/1.25 = 2/2

X/1.25 = 1

X = 1.25 moles

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sukhopar [10]

Answer:

a element

Explanation:

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3 years ago

An ionic bond forms between sodium chorine when the sodium atoms _______ electrons.

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4 0

4 years ago

The ________ orbital is degenerate with 5py in a many-electron atom.

arsen [322]

The ________ orbital is degenerate with 5py in a many-electron atom.

<h2>5px is the correct answer</h2>

5 0

3 years ago

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds silver nitrate solution to a sample of the

anyanavicka [17]

Answer:

c. precipitation

Explanation:

Let's consider the following balanced net ionic equation.

Cl⁻(aq) + AgNO₃(ag) ⇒ AgCl(s) + NO₃⁻ (ag)

What kind of reaction is this?

a. acid-base. No, because the reactants are not acids and bases.

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3 0

3 years ago

The estimated heat of vaporization of diethyl ether using the Chen's rule is A. 29.7 KJ/mol B. 33.5 KJ/mol C. 26.4 KJ/mol D. 36.

Brums [2.3K]

Answer:

C. 26.4 kJ/mol

Explanation:

The Chen's rule for the calculation of heat of vaporization is shown below:

$\Delta H_v=RT_b\left [ \frac{3.974\left ( \frac{T_b}{T_c} \right )-3.958+1.555lnP_c}{1.07-\left ( \frac{T_b}{T_c} \right )} \right ]$

Where,

$\Delta H_v$ is the Heat of vaoprization (J/mol)

$T_b$ is the normal boiling point of the gas (K)

$T_c$ is the Critical temperature of the gas (K)

$P_c$ is the Critical pressure of the gas (bar)

R is the gas constant (8.314 J/Kmol)

For diethyl ether:

$T_b=307.4\ K$

$T_c=466.7\ K$

$P_c=36.4\ bar$

Applying the above equation to find heat of vaporization as:

$\Delta H_v=8.314\times307.4 \left [ \frac{3.974\left ( \frac{307.4}{466.7} \right )-3.958+1.555ln36.4}{1.07-\left ( \frac{307.4}{466.7} \right )} \right ]$

$\Delta H_v=26400 J/mol$

The conversion of J into kJ is shown below:

1 J = 10⁻³ kJ

Thus,

$\Delta H_v=26.4 kJ/mol$

<u>Option C is correct</u>

6 0

4 years ago