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3 years ago

In this redox reaction, identify the reducing agent. 2Li + F2 2LiF

2 answers:

8 0

As what we see in the chemical reaction that is given, we can conclude that the Lithium must be the reducing agent since it is the one that is oxidised. In addition to that, a redox reaction or simply known as the oxidation-reduction reaction usually operates when electrons get transferred between species.

kvv77 [185]3 years ago

6 0

I simply refer to the correct answer:
brainly.com/question/1621662

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How manymoles of each ion are present in 175 mL of 0.147 M Fe2(SO4)3?

lilavasa [31]

Answer: 0.0257 moles of $Fe^{3+}$ and 0.0257 moles of $SO_4^{2-}$

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

$Molarity=\frac{moles}{\text {Volume in L}}$

moles of $Fe_2(SO_4)_3=Molarity\times {\text {Volume in L}}=0.147\times 0.175L=0.0257moles$

The balanced reaction for dissociation will be:

$Fe_2(SO_4)_3\rightarrow Fe^{3+}+SO_4^{2-}$

According to stoichiometry:

1 mole of $Fe_2(SO_4)_3$ gives 1 mole of $Fe^{3+}$ and 1 mole of $SO_4^{2-}$

Thus there will be 0.0257 moles of $Fe^{3+}$ and 0.0257 moles of $SO_4^{2-}$

8 0

3 years ago

A cough syrup contains 5.0% ethyl alcohol, c2h5oh, by mass. if the density of the solution is 0.9928 g/ml, determine the molarit

WARRIOR [948]

To answer the question above, let us a basis of the 1000 mL or 1 L.
volume = (0.9928 g/mL)(1000mL) = 992.8 g
Then, determine the mass of the alcohol by multiplying the total mass by the decimal equivalent of 5%.
mass of alcohol = 0.05(992.8 g) = 49.64 g
Then, determine the number of moles of ethyl alcohol by dividing the mass of alcohol by the molar mass (46 g/mol).
n = 49.64 g/ (46 g/mol) = 1.08 mol
Then, divide the number of moles by the volume (our basis is 1 L)
molarity = 1.08 mol/ 1 L = 1.08 M

5 0

3 years ago

What is the energy of a wave with wavelength of 4.2 x 10-7 m. (Hint: Calculate for frequency first.)

erik [133]

Answer:

Option B. 4.74×10¯¹⁹ J.

Explanation:

The following data were obtained from the question:

Wavelength (λ) = 4.2×10¯⁷ m

Energy (E) =.?

Next, we shall determine the frequency of the wave. This can be obtained as follow:

Wavelength (λ) = 4.2×10¯⁷ m

Velocity (v) = constant = 3×10⁸ m/s

Frequency (f) =.?

v = λf

3×10⁸ = 4.2×10¯⁷ × f

Divide both side by 4.2×10¯⁷

f = 3×10⁸ / 4.2×10¯⁷

f = 7.143×10¹⁴ s¯¹

Therefore, the frequency of the wave is 7.143×10¹⁴ s¯¹.

Finally, we shall determine the energy of the wave using the following formula

E = hf

Where

E is the energy.

h is the Planck's constant

f is the frequency

Thus, the enery of the wave can be obtained as follow:

Frequency (f) = 7.143×10¹⁴ s¯¹.

Planck's constant = 6.63×10¯³⁴ Js

Energy (E) =..?

E = hf

E = 6.63×10¯³⁴ × 7.14×10¹⁴

E = 4.74×10¯¹⁹ J

Therefore, the energy of the wave is 4.74×10¯¹⁹ J.

5 0

3 years ago

What volume of 0.100 M HCl will react completely with 50.00 mL of 0.200 M NaOH?

skelet666 [1.2K]

Equation of reaction
Hcl+NaoH-->Nacl+H2O
1:1
Using the formula CaVa/CbVb=na/nb
Ca(Concentation of acid)= 0.100M
Cb(Concentration of base)=0.200M
Va=?
VB=50.00ml
na=1
nb=1
from the formula
Va= CbVbna/Canb
Va= 0.2*50*1/0.1*1
=10/0.1=100ml
Therefore volume of acid = 100ml

7 0

3 years ago

The compound known as diethyl ether, commonly referred to as ether, contains carbon, hydrogen, and oxygen. A 1.376 g sample of e

hoa [83]

Answer:

The answer to your question is: C₄H₁₀O

Explanation:

Data

CxHyOz

mass sample : 1.376 g

mass CO₂ = 3.268 g

mass H₂O = 1.672 g

Process

Reaction

CxHyOz + O₂ ⇒ CO₂ + H₂O

1.- Calculate the moles and mass of carbon

Molecular mass CO₂ = 44g

44 g of CO₂ -------------- 12 g of C

3.268 g of CO₂ -------- x

x = (3.268 x 12) / 44

x = 0.891 g of Carbon

12 g of carbon ----------- 1 mol

0.891 g of C ---------- x

x = (0.891 x 1) / 12

x = 0.0743 moles of carbon

2.- Calculate the moles and mass of hydrogen

18 g of water --------------- 2 g of H

1.672 g of H₂O ------------ x

x = (1.672 x 2) / 18

x = 0.186 g of hydrogen

1 g of hydrogen ------------ 1 mol of H

0.186 g of H ------------ x

x = (0.186 x 1) / 1

x = 0.186 moles of H

3.- Calculate the mass of Oxygen and its moles

Mass of Oxygen = 1.376 - 0.891 - 0.186

= 0.299 g of O₂

Moles of Oxygen

16 g of Oxygen ---------------- 1 mol

0.299 g of O ----------------- x

x = (0.299 x 1) / 16

x = 0.019 moles of Oxygen

4.- Divide by the lowest number of moles

Carbon 0.0743/ 0.019 = 3.9 ≈ 4.0

Hydrogen 0.186/ 0.019 = 9.7 = 10

Oxygen 0.019/ 0.019 = 1

5.- Write the empirical formula

C₄H₁₀O

4 0

3 years ago