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3 years ago

When 1.5 grams of magnesium burns, how many grams of magnesium oxide will be formed?

1 answer:

6 0

The balanced chemical reaction for this would be written as:

2Mg + O2 = 2MgO

We use this reaction and the amount of the reactant given to calculate for the amount of magnesium oxide that is produced. We do as follows:

1.5 g Mg (1 mol / 24.31 g) ( 2 mol MgO / 2 mol Mg ) (40.30 g /1 mol ) = 2.49 g MgO produced

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In the compound iodine heptafluoride: (hints: write out the molecular formula of this compound before answering the question. Al

Aloiza [94]

In the compound iodine heptafluoride: (hints: write out the molecular formula of this compound before answering the question. Also be sure you clearly understand the concepts of charge, oxidation numbers, how to determine charge and oxidation numbers, and - most important of all! - the similarities and the differences between charges and oxidation numbers)

<u>Each fluorine atom has a charge of 1</u>

<h3>What is iodine heptafluoride?</h3>

The interhalogen compound iodine heptafluoride, often known as iodine(VII) fluoride or iodine fluoride, has the chemical formula IF7. As anticipated by VSEPR theory, it exhibits a unique pentagonal bipyramidal structure. The molecule is capable of undergoing the Bartell process, a pseudorotational rearrangement that is similar to the Berry mechanism but for a heptacoordinated system. It produces colorless crystals that melt at 4.5 °C and have a very narrow liquid range with a boiling point of 4.77 °C. The dense mist has an unpleasant, musty smell. The molecule is symmetrical with D5h. suggestion

To learn more about iodine heptafluoride from the given link:

brainly.com/question/28200374

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7 0

1 year ago

Determine the empirical formula of a compound containing 24.74% potassium, 34.74% manganese, and 40.50% oxygen. What is the name

AlexFokin [52]

The answer would be KMnO4, please let me know if you would like me to explain how i got this

4 0

3 years ago

Determine the molarity of 1.2 mol KCl in 1.1 L of a solution?

victus00 [196]

Answer:

1.1 M

General Formulas and Concepts:

Molarity = moles of solute / liters of solution

Explanation:

<u>Step 1: Define variables</u>

1.2 mol KCL

1.1 L of solution

M = unknown

<u>Step 2: Solve for Molarity</u>

Substitute: M = 1.2 mol/1.1 L
Evaluate: M = 1.09091

<u>Step 3: Check</u>

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

1.09091 M ≈ 1.1 M

7 0

2 years ago

A 25.0 g sample of metal at

Nadya [2.5K]

The change in temperature of the metal is 6.1°C. Details about change in temperature can be found below.

<h3>How to calculate change in temperature?</h3>

The change in temperature of a substance can be calculated by subtracting the initial temperature of the substance from the final temperature.

According to this question, a 25.0 g sample of metal at 16.0 °C is warmed to 22.1 °C by 259J of energy.

This means that the change in temperature of the metal can be calculated as:

∆T = 22.1°C - 16°C

∆T = 6.1°C

Therefore, the change in temperature of the metal is 6.1°C.

Learn more about change in temperature at: brainly.com/question/19051558

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7 0

1 year ago

2.24g of iron combine with 0.96g of oxygen to form an oxide of iron. Determine the formula of this oxide of iron and use it to c

irakobra [83]

Answer:

See Explanation

Explanation:

Let us find the number of moles of each element

For iron = 2.24g/56 = 0.04 moles

For oxygen = 0.96 g/16 = 0.06 moles

Then we divide by the lowest ratio;

0.04/0.04 and 0.06/0.04

1 and 2

We Thus obtain 1 : 1.5

Multiplying through by 2 we have; 2 : 3

The formula of the oxide formed is Fe2O3

The balanced equation is;

4Fe + 3O2 ------> 2Fe2O3

6 0

3 years ago