Answer:
Mass = 19.85 g
Explanation:
Given data:
Volume of chlorine gas = 80.4 L
Temperature = standard = 273.15 K
Pressure = standard = 1 atm
Mass of chlorine = ?
Molar mass of chlorine gas = 70.9 g/mol
Solution:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
By putting values,
1 atm × 80.4 L = n× 0.0821 atm.L/mol.K × 273.15 K
80.4 atm.L = n× 22.43 atm.L/mol
n = 22.43 atm.L/mol / 80.4 atm.L
n = 0.28 mol
Mass of Cl₂:
Mass = number of moles × molar mass
Mass = 0.28 mol × 70.9 g/mol
Mass = 19.85 g
a ______ is a single kind of matter that has a specific composition.
Answer:
SUBSTANCE
Explanation:
hope that help you thanx
A sample of 25.0 mL of 0.120 M Ca(OH)2(aq) is titrated with 0.150 M HCl(aq). What volume of HCl(aq) is needed to completely neutralize the Ca(OH)2(aq)
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!
Salad oil floats on water. Water has a density of 1.0 g/cm3. What can you say about the density of the salad oil?
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.
When the density of a substance is greater than another, it will sink. If the density of the salad oil is greater than that of water, then it will sink and not float. Since the oil floats on water, the density of the oil is lesser than that of the water.Density is the mass per unit volume of a substance.
HELP ME SLOVE RN IT IS FOR CHEM
Answer:
NARUTOOOO
Explanation:
1. Which of the following elements has the smallest ionization energy
a. arsenic
b. nitrogen
c. bismuth
d. chlorine.
Answer:
chlorine
Explanation:
hope this helps
Complete combustion of 3.10 g of a hydrocarbon produced 9.90 g of CO2 and 3.55 g of H2O. What is the empirical formula for the hydrocarbon
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
When does a chemical bond form between two atoms? Select one :
O a. When attractive forces are greater than repulsive forces.
O b. When potential energy is lowest for the pair.
O c. When potential energy is greatest for the pair .
O d. When repulsive forces are greater than attractive forces.
3.25 x 10^24 molecules of dinitrogen pentoxide would be how many moles?
5.40 mol N₂O₅
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Using Dimensional AnalysisAvogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.Explanation:Step 1: Define
3.25 × 10²⁴ molecules N₂O₅
Step 2: Identify Conversions
Avogadro's Number
Step 3: Convert
Set up: [tex]\displaystyle 3.25 \cdot 10^{24} \ molecules \ N_2O_5(\frac{1 \ mol \ N_2O_5}{6.022 \cdot 10^{23} \ molecules \ N_2O_5})[/tex]Multiply: [tex]5.39688 \ mol \ N_2O_5[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
5.39688 mol N₂O₅ ≈ 5.40 mol N₂O₅
What are the amount of moles in 12.15 grams of Magnesium?
The frequency of the stretching vibration of a bond in IR spectroscopy depends on what two quantities?
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.
What is the molar mass of CuCIO3
147.05 g/mol
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableExplanation: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
Two electron(s) are removed from an carbon atom. Enter the chemical symbol of the element.
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]
HURRY HELP 10 POINTS ILL GOVE BRAINLIEST I HAVE TO PASS PICTURE PROVIDED
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.
CONVERSIONS
Complete the following conversions
3. Given the following reaction, how many moles of Al2O3 will be produced if 1.35 moles of Fe are produced?
(8 points)
2 AI 3 Feo
3 Fe + Al2O3
+
it’s number 3 pls help
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
Suppose a current of 220.mA is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 79.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.
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
Write out an example of a single replacement reaction involving silver and zinc.
Answer:
whats zinc?
Explanation:
butyric acid has a putrid odor like rancid butter. If you got some of this material on your hands, how could you remove the odor
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
If a steel container holds 3.50 moles of hydrogen gas and 3.50 moles of helium gas, and the total pressure is 4.00 atm., what is the partial pressure of each of the gases
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
A student adds 34.2 mL of water to 72.3 mL of a 7.50 M glucose solution. (i) Will this solution be concentrated or dilute
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
Gaseous butane CH3CH22CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of carbon dioxide formed from the reaction of 3.49g of butane and 17.1g of oxygen gas
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
To what temperature must an ideal gas at 27 o C be cooled to reduce its volume by 1/3
Answer:
28 oc
Explanation:
What is meant by the term average mass
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.
mass
6.00 g of a certain compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 180. g/mol, is burned
completely in excess oxygen, and the mass of the products carefully measured:
product
carbon dioxide 8.80 g
3.60 g
Use this information to find the molecular formula of X.
water
alo
O
х
?
The molecular formula =C₆H₁₂O₆
Further explanationGiven
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
Draw the Lewis structures for three resonance forms of the nitrate ion, NO−3 . Include electron lone pairs, and any formal charges.
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.
How many moles are in 60.0 grams of water?
3.33 mol H₂O
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableUsing Dimensional AnalysisExplanation: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
Set up: [tex]\displaystyle 60.0 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O})[/tex]Multiply: [tex]\displaystyle 3.32963 \ mol \ H_2O[/tex]Step 4: Convert
Follow sig fig rules and round. We are given 3 sig figs.
3.32963 mol H₂O ≈ 3.33 mol H₂O
What would the mass be, in grams, of 0.89 moles of Cl2?
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
Which characteristic is used to classify metamorphic rocks as foliated or non-foliated?
Answer: d. Arrangement of grains
Explanation:
Edge:)))
A homogeneous mixture is?
Answer:
two components of the same thing
Explanation:
What is the mass, in grams, of 0.0490 mol of iron(III) phosphate
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!
can you make energy with ionized particles? yes or no and how