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3 years ago

Which of the following is the correct name for MgCI?

Chemistry

1 answer:

kupik [55]3 years ago

7 0

Answer:

C - Magnesium Chloride

Explanation:

The metal in a compounds name is always pronounced, and if the last element is a non-metal, the first half of the element is used and the last part is replaced with "ide"

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Write the balanced chemical equation between H2SO4H2SO4 and KOHKOH in aqueous solution. This is called a neutralization reaction

const2013 [10]

Answer:

0.185M sulfuric acid

Explanation:

Based on the reaction:

H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

1 mole of sulfuric acid reacts with 2 moles of KOH

Initial moles of H₂SO₄ and KOH are:

H₂SO₄: 0.750L ₓ (0.470mol / L) = 0.3525 moles of H₂SO₄

KOH: 0.700L ₓ (0.240mol / L) = 0.168 moles of KOH

The moles of sulfuric acis that react with KOH are:

0.168mol KOH ₓ (1 mole H₂SO₄ / 2 moles KOH) = 0.0840 moles of sulfuric acid.

Thus, moles that remain are:

0.3525moles - 0.0840 moles = 0.2685 moles of sulfuric acid remains

As total volume is 0.700L + 0.750L = 1.450L, concentration is:

0.2685mol / 1.450L = 0.185M sulfuric acid

8 0

2 years ago

The combustion of 40.10 g of a compound which contains only C, H, Cl and O yields 58.57 g of CO2 and 14.98 g of H2O. Another sam

elena-14-01-66 [18.8K]

Answer:

The empirical formula is C4H5ClO2

Explanation:

Step 1: Data given

Mass of the sample = 40.10 grams

Mass of CO2 produced = 58.57 grams

Mass of H2O produced = 14.98 grams

Molar mass CO2 = 44.01 g/mol

Molar mass H2O = 18.02 g/mol

Atomic mass C= 12.01 g/mol

Atomic mass O = 16.0 g/mol

Atomic mass H = 1.01 g/mol

In experiment 2, mass = 75.00 grams and 22.06 grams is Cl

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 58.57 grams / 44.01 g/mol

Moles CO2 = 1.33 moles

Step 3: Calculate moles C

For 1 mol CO2 we have 1 mol CO2

For 1.33 moles CO2 we have 1.33 moles C

Step 4: Calculate mass C

Mass C = 1.33 grams * 12.01 g/mol

Mass C = 15.97 grams

Step 5: Calculate moles H2O

Moles H2O= 14.98 grams /18.02 g/mol

Moles H2O = 0.831 moles

Step 6: Calculate moles H

For 1mol H2O we have 2 moles H

For 0.831 moles H2O we have 2*0.831 = 1.662 moles H

Step7: Calculate mass H

Mass H = 1.662 moles * 1.01 g/mol

Mass H = 1.68 grams

Step 8: Calculate mass %

%C = (15.97 grams / 40.10) * 100 %

%C = 39.8 %

%H = (1.68 / 40.10 ) *100%

%H = 4.2 %

%Cl = (22.06 / 75.00 ) * 100%

%Cl = 29.4 %

%O = 100 % - 39.8% - 4.2 % - 29.4 %

%O = 26.6 %

Step 9: Calculate moles in compound

We assume the compound has a mass of 100 grams

Mass C = 39.8 grams

MAss H = 4.2 grams

MAss Cl = 29.4 grams

Mass O = 26.6 grams

Moles C = 39.8 grams / 12.01 g/mol

Moles C = 3.314 moles

Moles H = 4.2 moles / 1.01 g/mol

Moles H = 4.158 moles

Moles Cl =29.4 grams / 35.45 g/mol

Moles Cl = 0.829 moles

Moles O = 26.6 grams / 16.0 g/mol

Moles O = 1.663 moles

Step 10: calculate the mol ratio

We divide by the smallest amount of moles

C: 3.314 moles / 0.829 moles = 4

H: 4.158 moles / 0.829 moles = 5

Cl: 0.829 moles /0.829 moles = 1

O: 1.663 moles / 0.829 moles = 2

This means For each Cl atom we have 4 C atoms, 5 H atoms and 2 O atoms

The empirical formula is C4H5ClO2

5 0

3 years ago

Warm air holds _____.

Agata [3.3K]

Answer:

less water than cl air

Explanation:

i think

8 0

3 years ago

Write a chemical equation for the reaction that occurs in the following cell: Cu|Cu2+(aq)||Ag+(aq)|Ag. Of the two metals, copper

KatRina [158]

Answer:

Answer is given below.

Explanation:

Anode is that electrode where oxidation occurs. Cathode is that electrode where reduction occurs.

In cell representation, half cell present left to salt-bridge notation $(\parallel )$ is anodic system and another half cell present right to salt-bridge notation $(\parallel )$ is cathodic system.

So anode is Cu and cathode is Ag.

oxidation: $Cu-2e^{-}\rightarrow Cu^{2+}(aq.)$

[reduction: $Ag^{+}+e^{-}\rightarrow Ag$ ] $\times 2$

-----------------------------------------------------------------------------------------------

chemical equation: $Cu+2Ag^{+}(aq.)\rightarrow Cu^{2+}(aq.)+2Ag$

Oxidizing agent is that species which takes electron from another species. Here $Ag^{+}(aq.)$ takes electron from Cu. Hence $Ag^{+}(aq.)$ is the oxidizing agent.

Reducing agent is that species which gives electron to another species. Here Cu gives electron to $Ag^{+}(aq.)$ . Hence Cu is the reducing agent.

6 0

3 years ago

During a chemical reaction, two hydrogen atoms combine with two oxygen atoms. How many hydrogen and oxygen atoms will be present

Reil [10]

Answer:

2 hydrogen and 1 oxygen atoms

Explanation:

3 0

2 years ago