All categories

2 years ago

I will mark brainliest

Chemistry

1 answer:

nikitadnepr [17]2 years ago

6 0

$S_8 +120_2$ → $8SO_3$ has been balanced correctly.

<h3>What is a balanced chemical equation?</h3>

A balanced equation is an equation for a chemical reaction in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products.

$S_8 +120_2$ → $8SO_3$ has been balanced correctly and the rest are not balanced.

Learn more about balanced chemical equations here:

brainly.com/question/15052184

#SPJ1

You might be interested in

Which environmental conditions contribute most to the spread of bacteria?

Nostrana [21]

Answer: D

Explanation: Bacteria thrives in warm and moist environments.

6 0

3 years ago

Calculate the pH if the [H^+] = 9.71 ×<br> 10^-8

oksano4ka [1.4K]

Answer:

pH = 7.01

Explanation:

The pH can be calculated using the formula:

pH = -log[H⁺]

In this formula, [H⁺] represents the concentration of H⁺. Since you have been given this value, you can easily find the pH.

pH = -log[H⁺]

pH = -log[9.71 x 10⁻⁸]

pH = 7.01

4 0

2 years ago

Read 2 more answers

How can you separate a mixture containing two different liquids? filtration evaporation distillation magnetic attraction

maxonik [38]

Distillation I believe.....

7 0

4 years ago

What is the correct name

Inessa05 [86]

Answer:

The Answer is 2-methylpentane

Or the third one down.

Explanation:

5 0

3 years ago

Read 2 more answers

What is the pH of a buffer solution upon mixing 15.0 mL of 0.40 M HCl and 20.0 mL of 0.50 M NH? Kb (NH3) = 1.8 x 10 E. 7.00 A. 9

vladimir2022 [97]

<u>Answer:</u> The pH of resulting solution is 9.08

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$ ........(1)

<u>For HCl:</u>

Molarity of HCl = 0.40 M

Volume of solution = 15.0 mL

Putting values in equation 1, we get:

$0.40M=\frac{\text{Moles of HCl}\times 1000}{15.0mL}\\\\\text{Moles of HCl}=0.006mol$

<u>For ammonia:</u>

Molarity of ammonia = 0.50 M

Volume of solution = 20.0 mL

Putting values in equation 1, we get:

$0.50M=\frac{\text{Moles of ammonia}\times 1000}{20.0mL}\\\\\text{Moles of ammonia}=0.01mol$

The chemical reaction for hydrochloric acid and ammonia follows the equation:

$HCl+NH_3\rightarrow NH_4Cl$

Initial: 0.006 0.01

Final: - 0.004 0.006

Volume of solution = 15.0 + 20.0 = 35.0 mL = 0.035 L (Conversion factor: 1 L = 1000 mL)

To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

$pOH=pK_b+\log(\frac{[salt]}{[base]})$

$pOH=pK_b+\log(\frac{[NH_4Cl]}{[NH_3]})$

We are given:

$pK_b$ = negative logarithm of base dissociation constant of ammonia = $-\log (1.8\times 10^{-5})=4.74$

$[NH_4Cl]=\frac{0.006}{0.035}$

$[NH_3]=\frac{0.004}{0.035}$

pOH = ?

Putting values in above equation, we get:

$pOH=4.74+\log(\frac{0.006/0.035}{0.004/0.035})\\\\pOH=4.92$

To calculate pH of the solution, we use the equation:

$pH+pOH=14\\pH=14-4.92=9.08$

Hence, the pH of the solution is 9.08

3 0

4 years ago