Answers
Answer:
173.9 mL of HBr
Explanation:
We'll begin by calculating the number of mole in 6.73 g of CaCO₃. This can be obtained as follow:
Mass of CaCO₃ = 6.73 g
Molar mass of CaCO₃ = 40 + 12 + (16×3)
= 40 + 12 + 48
= 100 g/mol
Mole of CaCO₃ =?
Mole = mass / Molar mass
Mole of CaCO₃ = 6.73 / 100
Mole of CaCO₃ = 0.0673 mole
Next, we shall determine the number of mole of HBr that will react with 6.73 g (i.e 0.0673 mole) of CaCO₃. This can be obtained as follow:
2HBr + CaCO₃ —> CaBr₂ + H₂O + CO₂
From the balanced equation above,
2 moles of HBr reacted with 1 mole of CaCO₃.
Therefore, Xmol of HBr will react with 0.0673 mole of CaCO₃ i.e
Xmol of HBr = 2 × 0.0673
Xmol of HBr = 0.1346 mole
Thus, 0.1346 mole of HBr reacted.
Next, we shall determine the volume of HBr needed for the reaction. This can be obtained as follow:
Mole of HBr = 0.1346 mole
Molarity of HBr = 0.774 M
Volume =?
Molarity = mole / Volume
0.774 = 0.1346 / volume
Cross multiply
0.774 × volume = 0.1346
Divide both side by 0.774
Volume = 0.1346 / 0.774
Volume = 0.1739 L
Finally, we shall convert 0.1739 L to mL. This can be obtained as follow:
1 L = 1000 mL
Therefore,
0.1739 L = 0.1739 L × 1000 mL / 1 L
0.1739 L = 173.9 mL
Thus, 173.9 mL of HBr is needed for the reaction.
Related Questions
What amount of heat (in kJ) is required to convert 14.0 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g･°C; specific heat capacity of gas = 0.792 J/g･°C; ∆Hvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4°C)
Answers
Answer:
1.24 kJ is required to convert 14 g of liquid from 43.5°C to 128.2°C
Explanation:
This is a typical calorimetry problem:
We have to assume, no heat is lost to sourrounding.
First of all, we need to go from 43.5°C to 97.4°C, the boiling point.
Q = Ce . m . ΔT
We replace data, 1.18° J/g . 14 g . (97.4°C - 43.5°C)
Heat for the first stage is: 890.4 Joules
Now we have to change the state, and we need the ΔH. As we do not have latent heat, we can proceed like this:
1 mol release 30.1 kJ at vaporization.
We convert the mass to moles → 14 g. 1mol/ 67.44g = 0.207 mol
0.207 mol will release (0.207 . 30.1 kJ) = 6.25 kJ
Now, we are at gaseous phase.
Q = Ce . m . ΔT → 0.792 J/g°C . 14g . (128.2°C - 97.4°C)
Q = 341.5 Joules
To determine the amount of heat, we sum all the obtained values:
890.4 Joules + 6250 Joules + 341.5 Joules = 1238.2 J
We convert to kJ → 1238.2 J . 1kJ / 1000J = 1.24 kJ
The heat required to convert 14.0 g of an unknown liquid at 43.5 °C to gas at 128.2 °C is 7.48 kJ.
We want to calculate the heat required to convert 14.0 g of an unknown liquid at 43.5 °C to gas at 128.2 °C.
We can divide this process in 3 steps.
Heating of the liquid from 43.5 °C to 97.4 °C (normal boiling point).Vaporization of the liquid at 97.4 °C.Heating of the gas from 97.4 °C to 128.2 °C.1. Heating of the liquid from 43.5 °C to 97.4 °CWe will calculate the heat for this step (Q₁) using the following expression.
Q₁ = c(l) × m × ΔT
Q₁ = (1.18 J/g･°C) × 14.0 g × (97.4 °C - 43.5 °C) = 890 J = 0.890 kJ
where,
c(l) is the specific heat capacity of the liquid.m is the mass of the substance.ΔT is the change in the temperature.2. Vaporization of the liquid at 97.4 °C.We will calculate the heat for this step (Q₂) using the following expression.
Q₂ = (m/M) × ΔHvap
Q₂ = [14.0 g/(67.44 g/mol)] × 30.1 kJ/mol = 6.25 kJ
where,
m is the mass of the substance.M is the molar mass of the substance.ΔHvap is the enthalpy of vaporization of the substance.3. Heating of the gas from 97.4 °C to 128.2 °C.We will calculate the heat for this step (Q₃) using the following expression.
Q₃ = c(g) × m × ΔT
Q₃ = (0.792 J/g･°C) × 14.0 g × (128.2 °C - 97.4 °C) = 342 J = 0.342 kJ
where,
c(g) is the specific heat capacity of the gas.m is the mass of the substance.ΔT is the change in the temperature.4. Total amount of heat required (Q)Q = Q₁ + Q₂ + Q₃ = 0.890 kJ + 6.25 kJ + 0.342 kJ = 7.48 kJ
The heat required to convert 14.0 g of an unknown liquid at 43.5 °C to gas at 128.2 °C is 7.48 kJ.
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Convert 9.24 x 1023 molecules CO2 to moles
Answers
1.53 mol CO₂
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.Stoichiometry
Using Dimensional AnalysisExplanation:Step 1: Define
9.24 × 10²³ molecules CO₂
Step 2: Identify Conversions
Avogadro's Number
Step 3: Convert
Set up: [tex]\displaystyle 9.24 \cdot 10^{23} \ molecules \ CO_2(\frac{1 \ mol \ CO_2}{6.022 \cdot 10^{23} \ molecules \ CO_2})[/tex]Multiply/Divide: [tex]\displaystyle 1.53437 \ mol \ CO_2[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
1.53437 mol CO₂ ≈ 1.53 mol CO₂
how many moles of aluminum are needed to produce 0.418 mol of Al2(SO4)3? 2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
Answers
0.836 mol Al
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Stoichiometry
Using Dimensional AnalysisReactions RxNExplanation:Step 1: Define
[RxN - Balanced] 2Al (s) + 3H₂SO₄ (aq) → Al₂(SO₄)₃ (aq) + 3H₂ (g)
[Given] 0.418 mol Al₂(SO₄)₃
[Solve] x mol Al
Step 2: Identify Conversions
[RxN] 2 mol Al (s) → 1 mol Al₂(SO₄)₃ (aq)
Step 3: Stoich
[DA] Set up: [tex]\displaystyle 0.418 \ mol \ Al_2(SO_4)_3(\frac{2 \ mol \ Al}{1 \ mol \ Al_2(SO_4)_3})[/tex][DA] Multiply/Divide [Cancel out units]: [tex]\displaystyle 0.836 \ mol \ Al[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
Since our final answer already has 3 sig figs, there is no need to round.
Iron is a metal. The structure of iron is described as a lattice of positive ions in a sea of
electrons. Which of the following statements about iron are correct?
1 iron conducts electricity because the electrons are free to move
2 iron has a high melting point due to the strong covalent bonds
3 iron is an alloy
4 iron is malleable because the layers of atoms can slide over one another
A. 1 only
B. 1 and 3
C. 1 and 4
D. 2, 3 and 4
Answers
Answer: 1and 4
Explanation: iron is an element not an alloy. An ionic lattice is not bonded covalently.
A chemistry student needs 50.0ml of tetrahydrofuran for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of tetrahydrofuran is . Calculate the mass of tetrahydrofuran the student should weigh out. Be sure your answer has the correct number of significant digits.
Answers
Answer:
44.45 g of tetrahydrofuran.
Explanation:
From the question given above, the following data were obtained:
Volume of tetrahydrofuran = 50 mL
Density of tetrahydrofuran = 0.889 g/mL
Mass of tetrahydrofuran =?
Density of a substance is simply defined as the mass of the substance per unit volume of the substance. Mathematically, density is expressed as shown below:
Density = mass / volume
With the above formula, we shall determine the mass of tetrahydrofuran needed. This can be obtained as follow:
Volume of tetrahydrofuran = 50 mL
Density of tetrahydrofuran = 0.889 g/mL
Mass of tetrahydrofuran =?
Density = mass / volume
0.889 = mass / 50
Cross multiply
Mass = 0.889 × 50
Mass of tetrahydrofuran = 44.45 g
Therefore, the student should weigh out 44.45 g of tetrahydrofuran.
The lattice energy of a salt is 350 kJ/mol and the solvation energies of its ions add up to 320 kJ/mol for the preparation of a 0.50 M solution. In the preparation of this solution would the solution get colder or warmer
Answers
Answer:
It would get colder
Explanation:
The lattice energy is the energy involved in the disruption of interactions between the ions of the salt. In this case, we have: ΔHlat = 350 kJ/mol > 0, so it is an endothermic process (the energy is absorbed).
The solvation energy is the energy involved in forming interactions between water molecules and the ions of the salt. In this case, we have: ΔHsolv = 320 kJ/mol > 0, so it is an endothermic process (the energy is absorbed).
The dissolution process involve both processes: the disruption of ion-ion interactions of the salt and the solvation process. Thus, the enthalphy change (ΔHsol) in the preparation of the solution is calculated as the addition of the lattice energy and solvation energy:
ΔHsol= ΔHlat + ΔHsolv = 350 kJ/mol + 320 kJ/mol = 370 kJ/mol
370 kJ/mol > 0 ⇒ endothermic process
Since the preparation of the solution is an endothermic process, it will absorb energy from the surroundings, so the solution would get colder.
5. Which model shows the progression of the movement of particles from fastest to slowest as thermal energy is removed?
Answers
Answer:
A nivel microscópico y en el marco de la Teoría cinética, es el total de la energía cinética media presente como el resultado de los movimientos aleatorios de átomos y moléculas o agitación térmica, que desaparecen en el acto.
Explanation:
esoes
Final volume of Argon gas:
6. Volume-Volume Problem: If water vapor is added to Magnesium Nitride, ammonia gas is produced
when the mixture is heated, according to the following reaction:
Mg3N2 (s) +
H2O (g)—->
Mgo (s) +
NH3 (g)
If 10.2 mL of water reacts with magnesium nitride, what volume (in Liters) of Ammonia gas will form at
STP?
Answers
Answer:
6.78 × 10⁻³ L
Explanation:
Step 1: Write the balanced equation
Mg₃N₂(s) + 3 H₂O(g) ⇒ 3 MgO(s) + 2 NH₃(g)
Step 2: Calculate the moles corresponding to 10.2 mL (0.0102 L) of H₂O(g)
At STP, 1 mole of H₂O(g) has a volume of 22.4 L.
0.0102 L × 1 mol/22.4 L = 4.55 × 10⁻⁴ mol
Step 3: Calculate the moles of NH₃(g) formed from 4.55 × 10⁻⁴ moles of H₂O(g)
The molar ratio of H₂O to NH₃ is 3:2. The moles of NH₃ produced are 2/3 × 4.55 × 10⁻⁴ mol = 3.03 × 10⁻⁴ mol.
Step 4: Calculate the volume corresponding to 3.03 × 10⁻⁴ moles of NH₃
At STP, 1 mole of NH₃(g) has a volume of 22.4 L.
3.03 × 10⁻⁴ mol × 22.4 L/mol = 6.78 × 10⁻³ L
What is true about the inertia of two cars, Car A of mass 1,500 kilograms and Car B of mass 2,000 kilograms?
OA.
Car A and Car Bhave the same inertia.
B.
Car A has more inertia than Car B.
Oc.
Car Bhas more inertia than Car A.
ОО
D.
Both the cars have negligible inertia.
I’m
Answers
Answer:
Car B has more inertia than Car A
Explanation:
Given that,
Mass of car A = 1500 kg
Mass of car B = 2000 kg
Inertia is directly proportional to the mass of an object. Inertia is the measure of the mass of an object.
In this case, the mass of car B is more than that of car A, it means the inertia of car B is more than that of car A.
Hence, the correct option is (c) "Car B has more inertia than Car A".
How many particles are in 67.9 grams of water (H2O)?
Answers
Answer:
3.769022740695677
Explanation:
Answer:We get 1.81×1024 water molecules... Explanation: We assess the molar quantity of water in the usual way... Number of moles=massmolar mass.
brainliest plz
A student measures a boiling water bath with two different thermometers. The digital thermometer records the temperature as 100.2°C and has an uncertainty of 0.1°C. The analog thermometer records the temperature as 99.0°C and has an uncertainty of 0.5°C. What is the percent uncertainty of each thermometer? And what is the percent error given that water boils at 100.0°C?
Answers
Answer:
Explanation:
Measurement made = 100.2 °C
uncertainty = 0.1°C
percent uncertainty = .1 x 100 / 100.2
= .099 %
2 nd thermometer :
Measurement made = 99.0 °C
uncertainty = 0.5°C
percent uncertainty = .5 x 100 / 99
= .505 %
Percent error :
1 st thermometer
Error = 100.2 - 100 = .2 °C
measurement = 100.2
percent error = .2 x 100 / 100.2
= .1996 %
2 nd thermometer
Error = 100.00 - 99 = 1.00 °C
measurement = 99
percent error = 1 x 100 / 99
= 1.01 %
The percent error of digital thermometer is 0.1996 %. The percent error of analog thermometer is 1.01 %.
Percent uncertainty is the measure of degree of error region with the uncertainty in the measurement.
The percentage error is the difference in the measurement of the values with actual value.
Computation for percent uncertainty and percent errorThe percent uncertainty (%U) is calculated by:
[tex]\% U=\rm \dfrac{Uncertainty}{Measurement}\;\times\;100[/tex]
The percent error (%E) is calculated by:
[tex]\%E=\rm \dfrac{error\;value-actual\;value}{error\;value}\;\times\;100[/tex]
The percent uncertainty and error for digital thermometer is given as:The Recorded temperature = 100.2 degree Celsius
The actual temperature = 100 degrees Celsius
The uncertainty in the readings is 0.1 degree Celsius
The percent uncertainty is given by:
[tex]\%U=\dfrac{0.1}{100.2}\;\times\;100\\\\ \%U=0.099\;\%[/tex]
The percent uncertainty of digital thermometer is 0.099 %.
The percent error is given by:
[tex]\% E=\dfrac{100.2-100}{100.2}\;\times\;100 \\\\\% E=\dfrac{0.2}{100.2}\;\times\;100\\\\ \% E=0.1996\;\%[/tex]
The percent error of digital thermometer is 0.1996 %.
The percent uncertainty and error for analog thermometer is given as:The Recorded temperature = 99 degree Celsius
The actual temperature = 100 degrees Celsius
The uncertainty in the readings is 0.5 degree Celsius
The percent uncertainty is given by:
[tex]\%U=\dfrac{0.5}{99}\;\times\;100\\\\ \%U=0.505\;\%[/tex]
The percent uncertainty of analog thermometer is 0.505%.
The percent error is given by:
[tex]\% E=\dfrac{100-99}{99}\;\times\;100 \\\\\% E=\dfrac{1}{99}\;\times\;100\\\\ \% E=1.01\;\%[/tex]
The percent error of analog thermometer is 1.01 %.
Learn more about percent error, here:
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i am having trouble solving it pls help
Answers
Answer:
1. 0.097 s
2. 0.420 M
Explanation:
To solve both questions we'll use the formula:
[A]ₓ = [A]₀ - kt
Where [A]ₓ is the concentration of A at a given time; and [A]₀ is the initial concentration.
1) We input the data given by the problem:
0.167 M = 0.700 M - 5.48 M/s * t
And solve for t:
t = 0.097 s
2) We input the new data:
[A]ₓ = 0.500 M - 0.361 M/s * 0.220 s
and solve for [A]ₓ:
[A]ₓ = 0.420 M
What is the definition of lava?
Answers
Answer:
Lava, magma (molten rock) emerging as a liquid onto Earth's surface. The term lava is also used for the solidified rock formed by the cooling of a molten lava flow.
Explanation:
Determine the chemical equation for the reaction between Fe3+ and Cu2+ with NH3
Answers
Answer:
Cu2 + 4 NH3 = Cu (NH3) 42+
so - - >
[Cu (NH3) 6] ^ 2+
Explanation:
Ethanol, the alcohol in alcoholic beverages, has a density of 0.7893 g/mL. What is the shipping weight of a 5.0-gallon container of pure ethanol if the bottle weighs 1.82 lb and the shipping container and packaging weigh 0.76 lb
Answers
Answer:
16.09 kg
Explanation:
To solve this problem first we convert those 5.0 gallons of ethanol into liters:
5.0 gallons * [tex]\frac{3.78L}{1gallon}[/tex] = 18.9 LNow we calculate the mass of that volume of ethanol, using its density:
We convert 18.9 L ⇒ 18.9 * 1000 = 18900 mL
Mass = Density * VolumeMass = 0.7893 g/mL * 18900 mL = 14917.77 gFinally we convert the masses of the bottle and shipping container and packaging and add them to the mass of ethanol:
1.82 lb * 453.592 = 825.54 g0.76 lb * 453.592 = 344.73 gTotal Mass = 14917.77 g + 825.54 g + 344.73 g = 16088.04 gSo the shipping weight would be 16088.04 g, or 16.09 kg
A formula unit made with Na and unknown nonmetal "Z" has the formula, NaZ. Which element does "Z" represent?
Answers
Which of the following is considered a complex (Macro)molecule?
Glucose
DNA
Carbon dioxide
Answers
Answer:
it is Glucose hope it helps
Answer:
Glucose and DNA
Explanation:
Complex macromolecules are the combination of more than two molecules which are large and complex. The major types of complex macromolecules consists of 4 types which are carbohydrates, lipids, proteins, and nucleic acids.
Glucose is one of the carbohydrates, while DNA is another form of nuclei acid.
In an experiment, a student places a small piece of pure Mg(s) into a beaker containing 250.mL of 6.44MHCl(aq) . A reaction occurs, as represented by the equation above.
The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr
(ii) The number of moles of H2(g) produced in the reaction
Answers
Answer:
0.81 moles H2
Explanation:
The equation of the reaction is;
Mg(s) + 2HCl(aq) ------>MgCl2(aq) + H2(g)
Number of moles of HCl reacted = concentration * volume
Number of moles of HCl reacted = 6.44 * 250/1000
Number of moles of HCl reacted = 1.61 moles of HCl
If 2 moles of HCl produces 1 mole of H2
1.61 moles of HCl produces 1.61 * 1/2 = 0.81 moles H2
is calcium hydroxide an ionic compound, covalent compound, or acid?
Answers
Answer:
Calcium Hydroxide is an ionic compound
Some antacid tables contain aluminum hydroxide. The aluminum hydroxide reacts with stomach acid according to the equation: Al(OH)3 + 3HCl →AlCl3 + 3H2O. Determine the moles of stomach acid (HCl) required if a tablet contains 8.89 moles of Al(OH)3.
Answers
Answer:
26.67 mol HCl
Explanation:
Al(OH)₃ + 3HCl → AlCl₃ + 3H₂O
In order to solve this problem, we need to convert Al(OH)₃ moles to HCl moles.
To do so we use the stoichiometric ratios of the balanced reaction:
8.89 mol Al(OH)₃ * [tex]\frac{3molHCl}{1molAl(OH)_{3}}[/tex] = 26.67 mol HClThus 26.67 moles of HCl would react completely with 8.89 moles of Al(OH)₃.
Please match the correct type of reaction to its name.
Answers
2. Decomposition reaction
3. Double replacement reaction
4. Combustion reaction
5. Single replacement reaction
The figure shows different possible transitions of electrons as they move from higher energy states to lower energy states. Which transition will produce the spectrum line with the lowest wavelength in this element’s atomic spectrum?
A. A
B. B
C. C
D. D
Answers
Answer:
It is D !!
Explanation:
Just did test
Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide). (a) Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water. (b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.
Answers
Answer:
See explanation
Explanation:
The balanced reaction equation of the reaction between SiO2 and HF is shown below;
SiO2(s) + 4HF(aq) = SiF4(g) + 2H2O(l)
b)
2NaF(aq) + CaCl2(aq) --------> 2NaCl(aq) + CaF2(s)
The complete ionic equation is;
2 Na^+(aq) + 2F^-(aq) + Ca^+(aq) + 2 Cl^-(aq)------> 2 Na^+(aq) + 2 Cl^-(aq) + CaF2(s)
The net ionic equation;
Ca^+(aq) + 2F^-(aq) -------> CaF2(s)
Western art criticism unique in that
Answers
Answer:
they are a lot tougher and are expecting only greatness, sort of like theater critiques.
Explanation:
Why was d-day and the battle of France so important to American and the allies
Answers
Answer:
The Importance of D-Day
The D-Day invasion is significant in history for the role it played in World War II. It marked the turn of the tide for the control maintained by Nazi Germany; less than a year after the invasion, the Allies formally accepted Nazi Germany's surrender.
How many grams of a nonelectrolyte (78.2 g/mol) must be dissolved in 1 kg of solvent to obtain a freezing point of solution of 1.57ºC? The freezing point of the pure solvent is 4.72ºC and the freezing point depression constant of the solvent is 3.89 ºC/m
Answers
Answer Tu mama por si acaso
Explanation:
jkand
How do you balance this equation?
Answers
Answer:
HC₂H₃O₂ + NaHCO₃ —> NaC₂H₃O₂ + CO₂ + H₂O
The coefficients are: 1, 1, 1, 1, 1
Explanation:
_HC₂H₃O₂ + _NaHCO₃ —> _NaC₂H₃O₂ + _CO₂ + _H₂O
To balance an equation, we simply do a head count of the individual elements and ensure they are balanced on both side.
For the above equation, we shall balance it as :
HC₂H₃O₂ + NaHCO₃ —> NaC₂H₃O₂ + CO₂ + H₂O
Reactant:
H = 5
C = 3
O = 5
Na = 1
Product:
H = 5
C = 3
O = 5
Na = 1
From the above, we can see that each element is the same on both side of the equation. Thus the equation is already balanced
HC₂H₃O₂ + NaHCO₃ —> NaC₂H₃O₂ + CO₂ + H₂O
The coefficients are: 1, 1, 1, 1, 1
What is the term for the chemical reaction that makes soap?
Answers
Answer: soaps are a sodium or potassium salts of long chain fatty acids.when triglycerides in fat/oil react with aqueous NaOH or KOH,they are converted into soap and glycerol.This is called alkaline hydrolysis of esters.Since this reaction leads to formation of soap, it is called the saponification process.
Explanation:
what does GCAT help us remember?
Answers
f) How many neutrons are there in the nucleus of arsenic?
1. Neodymium
2. Selenium
3. Strontium
Answers
Explanation:
How many neutrons are there in the nucleus of arsenic?42 neutrons
The nucleus consists of 33 protons (red) and 42 neutrons (blue).
An element has isotopes, which means the same number of protons but different numbers of neutrons.