Which two types of organisms are found in the domain Eukarya?
A Protists
B. Archaea
O C. Animals
D. Bacteria

Answer:

SUBSTANCE

Explanation:

hope that help you thanx

Answer:

10.56 g

Explanation:

C4H10(g) + 13/2O2 (g) -------> 4CO2(g) + 5H2O(l)

Number of moles of butane = 3.49g/ 58 g/mol = 0.06 moles

1 mole butane yields 4 moles of CO2

0.06 moles of butane = 0.06 × 4/1 = 0.24 moles of CO2

Number of moles of oxygen = 17.1g/32g/mol = 0.53 moles of oxygen

6.5 moles of oxygen yields 4 moles of CO2

0.53 moles of oxygen yields 0.53 × 4/6.5 =0.33 moles of CO2

Butane is the limiting reactant

Theoretical yield of CO2 = 0.24 moles × 44g/mol = 10.56 g

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

H₂SO₄ is composed of the most atoms

Given

Compounds of A. H2SO4 B. Li2N C. Mg(OH)2 D. NaF

Required

The most atoms

Solution

Compounds are composed of atoms of the same or different types

The number of atoms can be indicated from the subscript of each of the constituent atoms of the compound

A. H₂SO₄ : 2 atoms H, 1 atom S, 4 atoms O = 7 atoms

B. Li₂N : 2 atoms L, 1 atoms N = 3 atoms

C. Mg(OH)₂ : 1 atom Mg, 2 atoms O, 2 atoms H = 5 atoms

D. NaF : 1 atom Na, 1 atom F = 2 atoms

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:

chlorine

Explanation:

hope this helps

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.

The locations with subatomic particles with the least mass are locations 1 and 4.

An atom is usually divided into two main regions:

The three sub-particles previously mentioned (neutrons, protons, and electrons) differ not only in their location but also in their mass. Indeed, electrons have a lower mass if compared to neutrons and protons.

Based on this, the outer region (locations 1 and 4) has sub particles with the least mass.

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Answer:

1 and 4

Explanation:

took the test

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Answer:

A) HCI( hydrochloric acid)

Explanation:

HCI is a strong acid because it has more number of hydrogen ions whereas acetic acid contains less number of hydrogen ions so its a weak acid

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:

28 oc

Explanation:

Answer:

try looking the equations or find a calulator for those type of eqautions

Explanation:

Answer:

I' really don't know I'm sorry

Answer:

its a diffrent color :)

Explanation:

Answer:

The molar concentration of normal saline is 0.15 mol/L.

Explanation:

The mass of NaCl in 0.85% of normal saline is:

[tex] 0.85 \% = \frac{0.85 g}{100 ml} [/tex]

[tex] m_{NaCl} = 0.85 g [/tex]

The molar concentration can be found using the following equation:

[tex] C = \frac{n}{V} [/tex]        

So we need to find the number of moles of NaCl in 1 liter of solution.

[tex]m_{NaCl} = \frac{0.85 g}{100 mL}*\frac{1000 mL}{1 L}*1 L = 8.5 g[/tex]

[tex]n = \frac{m_{NaCl}}{M}[/tex]

Where:

M: is the molar mass of NaCl = 58.44 g/mol

[tex] n = \frac{8.5 g}{58.44 g/mol} = 0.15 moles [/tex]

Hence, the molar concentration is:

[tex]C = \frac{0.15 moles}{1 L} = 0.15 mol/L[/tex]        

Therefore, the molar concentration of normal saline is 0.15 mole per liter.

I hope it helps you!      

Answer: d. Arrangement of grains

Explanation:

Edge:)))

Answer:

1. Partial pressure of H₂ = 2 atm

2. Partial pressure of He = 2 atm

Explanation:

The following data were obtained from the question:

Mole of H₂ = 3.50 moles

Mole of He = 3.50 moles

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ =?

Partial pressure of He =?

Next, we shall determine the mole fraction of each gas this can be obtained as follow:

Mole of H₂ = 3.50 moles

Mole of He = 3.50 moles

Total mole = Mole of H₂ + Mole of He

Total mole = 3.50 + 3.50

Total mole = 7 moles

Mole fraction of H₂ = mole of H₂ / Total mole

Mole fraction of H₂ = 3.5/7

Mole fraction of H₂ = 0.5

Mole fraction of He = mole of He / Total mole

Mole fraction of He = 3.5/7

Mole fraction of He = 0.5

1. Determination of the partial pressure of H₂.

Mole fraction of H₂ = 0.5

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ =?

Partial pressure of H₂ = Mole fraction of H₂ × Pₜ

Partial pressure of H₂ = 0.5 × 4

Partial pressure of H₂ = 2 atm

2. Determination of the partial pressure of He.

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ = 2 atm

Partial pressure of He =?

Total pressure (Pₜ) = Partial pressure of H₂ + Partial pressure of He

4 = 2 + Partial pressure of He

Collect like terms

Partial pressure of He = 4 – 2

Partial pressure of He = 2 atm

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

5.40 mol N₂O₅

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

3.25 × 10²⁴ molecules N₂O₅

Step 2: Identify Conversions

Avogadro's Number

Step 3: Convert

Step 4: Check

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

5.39688 mol N₂O₅ ≈ 5.40 mol N₂O₅

Answer:

whats zinc?

Explanation:

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

Answer:

0.10M of Ba²⁺ is the concentration of the metal in excess

Explanation:

Based on the chemical reaction:

K₂CO₃(aq) + Ba(NO₃)₂(aq) → BaCO₃(s) + 2KNO₃(aq)

1 mole of potassium carbonate reacts per mole of barium nitrate

To solve this question we need to find the moles of each salt to find then the moles of Barium in excess:

Moles K₂CO₃:

0.025L * (0.25mol / L) = 0.00625moles K₂CO₃ = moles CO₃²⁻

Moles Ba(NO₃)₂:

0.030L * (0.40mol/L) = 0.012 moles of Ba(NO₃)₂ = 0.012 moles of Ba²⁺

That means moles of Ba²⁺ that don't react are:

0.012 mol - 0.00625mol = 0.00575 moles Ba²⁺

In 25 + 30mL = 55mL:

0.00575 moles Ba²⁺ / 0.055L =

The concentration of the excess metal ion after the precipitation reaction is complete is 0.1045 M

From the question,

We are to determine the concentration of the excess metal ion after the precipitation reaction is complete

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

K₂CO₃ + Ba(NO₃)₂ → BaCO₃ + 2KNO₃

This means

1  mole of K₂CO₃ is required to react completely with 1 mole of Ba(NO₃)₂

Now, we will determine the number of moles of each reactant present.

Volume = 25.0 mL = 0.025 L

Concentration = 0.25 M

Using the formula

Number of moles = Concentration × Volume

∴ Number of moles of K₂CO₃ present = 0.25 × 0.025

Number of moles of K₂CO₃ present = 0.00625 mole

Volume = 30.0 mL = 0.03 L

Concentration = 0.40 M

∴ Number of moles of Ba(NO₃)₂ present = 0.40 × 0.03

Number of moles of Ba(NO₃)₂ present = 0.012 mole

Since

1 mole of K₂CO₃ is required to react completely with 1 mole of Ba(NO₃)₂

Then,

The 0.00625 mole of K₂CO₃ will react with 0.00625 mole of Ba(NO₃)₂

∴ Only 0.00625 mole of the Ba(NO₃)₂ will react

This means Ba(NO₃)₂ is the excess reactant.

Now, we will determine the number of moles of Ba(NO₃)₂ remaining

Number of moles of Ba(NO₃)₂ remaining = 0.012 mole - 0.00625 mole

Number of moles of Ba(NO₃)₂ remaining = 0.00575 mole

Now, for the concentration

Using the formula

[tex]Concentration = \frac{Number\ of\ moles}{Volume}[/tex]

Volume = Total volume of the solution = 0.025L + 0.03L

Volume = 0.055 L

∴ Concentration of the excess metal ion = [tex]\frac{0.00575}{0.055}[/tex]

Concentration of the excess metal ion = 0.1045 M

Hence, the concentration of the excess metal ion after the precipitation reaction is complete is 0.1045 M

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Answer:

This idea helps students explain why more rain forms over West Ferris than East Ferris. ... Therefore, when students explain that water vapor condenses higher in the atmosphere, they are actually explaining that water vapor condenses high in the troposphere, which is relatively low in the atmosphere.

Explanation:

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: 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