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3 years ago

4Fe(s) + 3O2(g) ⟶ 2Fe2O3(g)

Chemistry

2 answers:

oee [108]3 years ago

8 0

Answer:

Iron. Fe

Explanation:

klio [65]3 years ago

5 0

Answer:

list down it..❤️❤️✌️✌️

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A sample of nitric acid has a mass of 8.2g. It is dissolved in 1L of water. A 25mL aliquot of this acid is titrated with NaOH. T

AveGali [126]

Answer:

18.075 mL of NaOH solution was added to achieve neutralization

Explanation:

First, let's formulate the chemical reaction between nitric acid and sodium hydroxide:

NaOH + HNO3 → NaNO3 + H2O

From this balanced equation we know that 1 mole of NaOH reacts with 1 mole of HNO3 to achieve neutralization. Let's calculate how many moles we have in the 25 mL aliquot to be titrated:

63.01 g of HNO3 ----- 1 mole

8.2 g of HNO3 ----- x = (8.2 g × 1 mole)/63.01 g = 0.13014 moles of HNO3

So far we added 8.2 grams of nitric acid (0.13014 moles) in 1 L of water.

1000 mL solution ---- 0.13014 moles of HNO3

25 mL (aliquot) ---- x = (25 mL× 0.13014 moles)/1000 mL = 0.0032535 moles

So, we now know that in the 25 mL aliquot to be titrated we have 0.0032535 moles of HNO3. As we stated before, 1 mole of NaOH will react with 1 mole of HNO3, hence 0.0032535 moles of HNO3 have to react with 0.0032535 moles of NaOH to achieve neutralization. Let's calculate then, in which volume of the given NaOH solution we have 0.0032535 moles:

0.18 moles of NaOH ----- 1000 mL Solution

0.0032535 moles---- x=(0.0032535moles×1000 mL)/0.18 moles = 18.075mL

As we can see, we need 18.075 mL of a 0.18 M NaOH solution to titrate a 25 mL aliquot of the prepared HNO3 solution.

4 0

3 years ago

Which of the following is an example of a chemical change? A. Boiling water B. Burning paper C. Dissolving sugar in water D. Mel

SpyIntel [72]

It’s B.burning paper

8 0

4 years ago

Read 2 more answers

What is the job of an environmental engineer?

xz_007 [3.2K]

Answer:

To keep the evinermental machinces working

Explanation:

6 0

3 years ago

Which of the following buffer systems would you use if you wanted to prepare a solution having a pH of approximately 9.5?Which o

zalisa [80]

Answer:

b. 0,08M NH₄⁺ / 0,12M NH₃

Explanation:

The buffers are:

a. 0,08M H₂PO₄⁻ / 0,12M HPO₄²⁻

b. 0,08M NH₄⁺ / 0,12M NH₃

It is possible to find out the pH of a buffer using Henderson-Hasselbalch formula:

pH = pka + log₁₀ [A⁻] / [HA] (1)

Where A⁻ is the conjugate base of the weak acid, HA.

a. For the system H₂PO₄⁻ / HPO₄²⁻ pka is 7,198. Replacing in (1)

pH = 7,198 + log₁₀ [0,12] / [0,08]

pH = 7,37

That means this buffer system don't have a pH of approximately 9,5

b. For the system NH₄⁺ / NH₃ pka is 9,3. Replacing in (1)

pH = 9,3 + log₁₀ [0,12] / [0,08]

pH = 9,50

That means this buffer system is the buffer you need to use.

I hope it helps!

7 0

3 years ago

Which of the following is NOT a physical property?

ICE Princess25 [194]

Answer:

reactivity is NOT a physical property

5 0

3 years ago