What is the atomic number of sulfur?
How many of its s orbitals are filled?
How many of its p orbitals are filled?

Answer: C9H16

Explanation:

molar mass C = 12.011, H = 1.008, O = 15.999, CO2 = 44.01, H2O = 18.00

9.9g CO2 = 0.225 mol, 3.55 g H2O = 0.200 mol

long way

molecules CO2 = 1.355x10^23 —> atoms of C

molecules H2O = 1.204x10^23 —> molecules H2

C:H2 = 1.355/1.204 = 1.125. —> C9H16

short way

molar massesCO2:H2O = 0.225:0.2 = 9:8

–> C9H16

verify

molar mass C9H16 =124

3.1g = 0.025 mol

oxidise C9H16 + 13O2 —> 9CO2 + 8H2O

0.025 mol + 13*0.025 mol (0.35mol) —> 9*0.025 + 8*0.025 —> 0.0.225 + 0.2

147.05 g/mol

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

CuClO₃

Step 2: Find MM

Molar Mass of Cu - 63.55 g/mol

Molar Mass of Cl - 35.45 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of CuClO₃ - 63.55 + 35.45 + 3(16.00) = 147.05 g/mol

3.33 mol H₂O

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

60.0 g H₂O (Water)

Step 2: Identify Conversions

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol

Step 3: Convert

Step 4: Convert

Follow sig fig rules and round. We are given 3 sig figs.

3.32963 mol H₂O ≈ 3.33 mol H₂O

Answer:

SUBSTANCE

Explanation:

hope that help you thanx

Answer:

two components of the same thing

Explanation:

Answer:

[tex]C^{2+}[/tex]

Explanation:

When a proton is removed, it changes the whole element. However, when electrons are removed, it becomes an ion. Since we are removing two electrons, we are subtracting a negative number, giving us positive two as our net ionic charge. Therefore, the answer is [tex]C^{2+}[/tex]

Answer:

whats zinc?

Explanation:

Answer:

[tex]V_{HCl}=48.0 mL[/tex]

Explanation:

Hello!

In this case, since the reaction between calcium hydroxide and hydrochloric acid shows a 2:1 mole ratio between them:

[tex]2HCl+Ca(OH)_2\rightarrow CaCl_2+2H_2O[/tex]

We need to use the following mole ratio:

[tex]2n_{Ca(OH)_2}=n_{HCl}[/tex]

That can be written in volumes and concentrations:

[tex]2M_{Ca(OH)_2}V_{Ca(OH)_2}=M_{HCl}V_{HCl}[/tex]

Thus, we solve for the volume of HCl as it is the unknown:

[tex]V_{HCl}=\frac{2M_{Ca(OH)_2}V_{Ca(OH)_2}}{M_{HCl}}[/tex]

Therefore, we plug in to obtain:

[tex]V_{HCl}=\frac{2*0.120M*25.0mL}{0.150M} \\\\V_{HCl}=48.0 mL[/tex]

Best regards!

Answer:

0.0195 g

Explanation:

Ag^+(aq) + e -------> Ag(s)

Since 1 electron was transferred, that means 96500C of electricity was required

108 g is deposited 96500 C

xg is deposited 220 × 10^-3 × 79.0

x = 108 × 220 × 10^-3 × 79.0/96500

x= 19.5 × 10^-3 g

x= 0.0195 g

The air barrier system

Answer:

NARUTOOOO

Explanation:

Answer:

Strength of the bond

Masses of the bonded atoms.

Explanation:

The lack of such groups means that they are not endogenous in the concentrate. 1. A bond's spreading frequency relies on the frequency of the bond and the concentrations of the atoms that are bonded.

The percentage of water in the compound CaSO₄.6H₂O = 44.26%

Given

Compound CaSO₄. 6H₂O

Required

The percentage of water

Solution

MW CaSO₄. 6H₂O :

= 40 + 32 + 4.16 + 12.1 + 6.16

= 244

MW 6H2O :

= 12.1 + 6.16

= 108

%water = (108 : 244) x 100%

%water = 44.26

The percentage of water in the compound CaSO₄.6H₂O is 44.26%

Since MW CaSO₄. 6H₂O :

= 40 + 32 + 4.16 + 12.1 + 6.16

= 244

Now

MW 6H2O :

= 12.1 + 6.16

= 108

So, percentage of water = (108 : 244) x 100%

= 44.26

learn more about water here: https://brainly.com/question/5534000

Answer:

Number of moles of Al₂O₃ = 0.45 mol

Explanation:

Given data:

Number of moles of Fe produced = 1.35 mol

Number of moles of Al₂O₃ = ?

Solution:

2Al + 3FeO   →    3Fe + Al₂O₃

now we will compare the moles of iron and  Al₂O₃

              Fe         :           Al₂O₃

               3          :             1

              1.35      :            1/3×1.35 = 0.45 mol

The molecular formula =C₆H₁₂O₆

Given

6.00 g of a certain compound X

The molecular molar mass of 180. g/mol

CO₂=8.8 g

H₂O=3.6 g

Required

The molecular formula

Solution

mass C in CO₂ :

= 1.12/44 x 8.8

= 2.4 g

mass H in H₂O :

= 2.1/18 x 3.6

= 0.4 g

Mass O in compound :

= 6-(2.4+0.4)

= 3.2 g

Mol ratio C : H : O

= 2.4/12 : 0.4/1 : 3.2/16

= 0.2 : 0.4 : 0.2

= 1 : 2 : 1

The empirical formula : CH₂O

(CH₂O)n=180 g/mol

(12+2+16)n=180

(30)n=180

n=6

(CH₂O)₆=C₆H₁₂O₆

Answer:

28 oc

Explanation:

Answer:

The solution will be dilute

Explanation:

The concentration of a solution is defined as the ratio between an amount of solute (Glucose, in this case) and an amount of solvent (Water in this case).

As the student is adding some water (Solvent), the amount of solute per amount of solvent will decrease. That is, if the concentration decreases,

the solution will be dilute

0.125 mol Ca

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

5.00 g Ca

Step 2: Identify Conversions

Molar mass of Ca - 40.08 g/mol

Step 3: Convert

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

0.12475 mol Ca ≈ 0.125 mol Ca

Answer:

Mass = 63.19 g

Explanation:

Given data:

Number of moles = 0.89 mol

Mass of Cl₂ = ?

Solution:

Formula:

Number of moles = mass/molar mass

Molar mass of Cl₂ = 71 g/mol

by putting values,

0.89 mol = mass/ 71 g/mol

Mass = 0.89 mol × 71 g/mol

Mass = 63.19 g

Answer:

See explanation

Explanation:

The nitrate ion is a polyatomic ion. It means that the nitrate ion contains more than one atom. These atoms are one nitrogen atom and three oxygen atoms.

However, we can not fully describe the bonding in the nitrate ion using one structure. I have shown three resonance structures that describe the bonding in the nitrate ion in the image attached to this answer.

Answer: d. Arrangement of grains

Explanation:

Edge:)))

Answer:

m = 7.39 g.

Explanation:

Hello!

In this case, since the molar mass of iron (III) phosphate is 150.82 g/mol based on its molecular formula (FePO₄), we can compute the mass in grams of 0.0490 moles of this compound by setting up the following dimensional analysis:

[tex]m=0.0490mol*\frac{150.82g}{1mol} \\\\m=7.39 g[/tex]

Best regards!

Answer:

Density of the oil is lesser than that of the water

Explanation:

The density of water is given as 1.0g/cm³.

  Salad oil is found to float on water, this implies that the density of this salad oil is lesser than that of the water.

Density is the mass per unit volume of a substance.

Answer:

Explanation:

The average atomic mass (sometimes called atomic weight) of an element is the weighted average mass of the atoms in a naturally occurring sample of the element. Average masses are generally expressed in unified atomic mass units (u), where 1 u is equal to exactly one-twelfth the mass of a neutral atom of carbon-12.

Answer:

C₃H₄O₄

Explanation:

In order to get the empirical formula of a compound, we have to follow a series of steps.

Step 1: Divide the percent by mass of each element by its atomic mass.

C: 34.6/12.01 = 2.88

H: 3.9/1.01 = 3.86

O: 61.5/16.00 = 3.84

Step 2: Divide all the numbers by the smallest one, i.e., 2.88

C: 2.88/2.88 = 1

H: 3.86/2.88 ≈ 1.34

O: 3.84/2.88 ≈ 1.33

Step 3: Multiply all the numbers by a number that makes all of them integer

C: 1 × 3 = 3

H: 1.34 × 3 = 4

O: 1.33 × 3 = 4

The empirical formula is C₃H₄O₄.

Answer:

The correct answer would be - the easiest way is to wash with some polar solvent or salt solution or soap and water

Explanation:

Butyric acid is a carboxylic acid that has a putrid odor like rancid butter. If an individual touch this chemical will have the same odor on his hand and to get rid of it one should wash his hand with a polar solvent such as methanol, or salt solutions such as like NaHCO3, or soap and water that will form sodium butyrate that has no smell and easily dissolve and remove.

Thus, the easiest way is to wash with some polar solvent or salt solution or soap and water

126 g Fe

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

2.25 mol Fe

Step 2: Identify Conversions

Molar Mass of Fe - 55.85 g/mol

Step 3: Convert

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

125.663 g Fe ≈ 126 g Fe