CHEMISTRY HIGH SCHOOL

The mass of a nitrogen atom is 14 u. What is the mass, in grams, of 2 mol of N ?

Answers

Answer 1

Answer:

Answer:

28 grams

Explanation:

Molar mass of Nitrogen = 14 u

Mass = Mole * Molar Mass

= 2 * 14

= 28 g

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Which element has both metallic and nonmetallic properties?
(1) Rb (3) Si
(2) Rn (4) Sr

Answers

Element which has both metallic and non-metallic properties is silicon as it is a metalloid.

What are metalloids?

Metalloids are defined as the elements which possess properties of both metals as well as non-metals.These elements are present only in the p-block of the periodic table.

In the p-block of the periodic table, these are the elements which separate the metals from the non metals by forming a zig-zag line between them.

These elements have 4 electrons in their valence shell which indicates that they can neither loose nor accept electrons rather share them between the 2 atoms.

As the elements are present between metals and non-metals they resemble both categories of elements in terms of their properties.They usually possess metallic appearances but are brittle.

Chemically, the behave as non-metals and have a characteristic property of forming alloys.They can form amphoteric or weakly acidic oxides.

Learn more about metalloids,here:

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Well, since they have both metallic and nonmetallic properties, it should be called Semiconductor. And this element would be Si, Silicon.

How many liters of chlorine gas can react with 56.0 grams of calcium metal at standard temperature and pressure? Show all of the work used to find your answer.Ca + Cl2 CaCl2

Answers

The balanced chemical reaction is:

Ca + Cl2 = CaCl2

We are given the amount of calcium metal to be used for this reaction. This will be the starting point for the calculations.

56 g Ca ( 1 mol Ca / 40.08 g Ca) (1 mol Cl2 / 1 mol Ca) ( 22.414 L Cl2 / 1 mol Cl2 ) = 31.32 L Cl2 gas produced from the reaction

Answer:

31.36 L of chlorine gas will react with 56 g of calcium.

Explanation:

$Ca + Cl_2\rightarrow CaCl_2$

Mass of calcium = 56 g

Moles of calcium gas = $(56 g)/(40 g/mol)=1.4 moles$

According to reaction, 1 mole of calcium react with 1 mole of chlorine gas.

Then 1.4 mol of calcium wiull react with :

$(1)/(1)* 1.4 = 1.4 mol$ chlorine gas

At standard temperature and pressure. 1 mol of gas occupies 22.4 L of volume.

Then 4.1 moles of chlorine gas will occupy :

$22.4 L\tmes 4.1 =31.36 L$

31.36 L of chlorine gas will react with 56 g of calcium.

What is the oxidation state of each element in the species Mn(ClO4)3?

Answers

The oxidation state of the compound Mn (ClO4)3 is to be determined in this problem. For oxygen, the charge is 2-, the total considering its number of atoms is -24. Mn has a charge of +3. TO compute for Mn, we must achieve zero charge overall hence 3+3x-24=0 where x is the Cl charge. Cl charge, x is +7.

Answer:

Mn: 3+

Cl: 7+

O: 2-

Explanation:

1) Compound given: Mn [ClO₄]₃

2) Initially you only know the oxidation state of O, since it is always 2-, except when it form peroxides, which is not the case.

3) So, you do not know the oxidation states neither of the Mn nor of the Cl, and you need some more information.

You might start from the ion [ClO₄] but you do not know its charge.

This ion comes from one of the oxoacids formed by Cl. Those are four different acids. These are them:

i) Oxidation state 1+: Cl₂O + H₂O → H₂Cl₂O₂ = HClO ⇒ ion ClO⁻

ii) Oxidation state 3+: Cl₂O₃ + H₂O → H₂Cl₂O₄ = HClO₂ ⇒ ion ClO₂⁻

iii) Oxidation state 5+: Cl₂O5 + H₂O → H₂Cl₂O₆ = HClO₃ ⇒ ion ClO₃⁻

iv) Oxidation state 7+: Cl₂O₇ + H₂O → H₂Cl₂O₈ = HClO₄ ⇒ ion ClO₄⁻

Finally, we have that our ion is ClO₄⁻ and the oxidation state of Cl is 7+.

4) Now you just have to find the oxidation state of Mn, for which you make a balance of charges:

Mn [ClO₄]₃

Since, the ion ClO₄⁻ has 1 negative charge, and there are 3 ions the total negative charge is 3-. Since the compound is neutral, you conclude that Mn has oxidation state 3+.

That according to this balance: 1(3+) + 3(1-) + 3 - 3 = 0.

5) Summarizing, the oxidation states are:

Mn: 3+

Cl: 7+

O: 2-

D Serum Levels Of 4 Mcg/mL, Calculate The Dose, In Milligrams, For A 120-lb Patient That May Be Expected To Result In A Blood Serum Gentamicin Level Of 4.5 Mcg/mL. This problem has been solved! See the answer If the administration of gentamicin at a dose of 1.75 mg/kg is determined to result in peak blood serum levels of 4 mcg/mL, calculate the dose, in milligrams, for a 120-lb patient that may be expected to result in a blood serum gentamicin level of 4.5 mcg/mL.

Answers

Answer:

The patient requires a dose of 107.2 mg of gentamicin

Explanation:

A dosage of 1.75 mg per Kilogram body weight results in blood serum levels of 4.5 mcg/mL

This means that; 1.75 mg/ kg = 4.0 mcg/mL

Therefore, dosage of gentamicin in mg/kg that will result in 4.5 mcg/mL blood serum level = (1.75 mg/Kg * 4.5 mcg/mL) / 4.0 mcg/mL

Dosageof gentamicin = 1.97 mg/Kg

1-lb = 0.453592 Kg

Weight of 120-lb patient in Kg = 120 * 0.453592 = 54.43 Kg

Dose in mg required by patient = 1.97 mg/Kg * 54.43 Kg = 107.2 mg

Therefore, the 120-lb patient requires a dose of 107.2 mg of gentamicin to result in a blood serum level of 4.5 mcg/mL

Predict the products in the following reaction:AgNO3(aq) + Na2CrO4(aq) →

A. AgCrO4(s) + Na2NO3(aq)

B. Ag2CrO4(s) + NaNO3(aq)

C. Ag(CrO4)2(s) + Na2NO3(aq)

D. Ag(CrO4)3(s) + Na(NO3)2(aq)

Answers

I think the correct answer from the choices listed above is option B. The products of the reaction made by silver nitrate and sodium chromate are silver chromate and silver nitrate. The chemical reaction should be written as:

2AgNO3(aq) + Na2CrO4(aq) → Ag2CrO4(s) + 2NaNO3(aq)

The products obtained when 2 AgNO₃ + Na₂CrO₄ reacts is Ag₂CrO₄ + 2 NaNO₃.