How many mL of 0.774 M HBr are needed to dissolve 6.73 g of CaCO3?
2HBr(aq) + CaCO3(s) -> CaBr2(aq) + H2O(1) + CO2(g)
____mL

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".

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:

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.

We 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,

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,

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,

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.

Learn more about heating curves here: https://brainly.com/question/10481356

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

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.

1.53 mol CO₂

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Stoichiometry

Step 1: Define

9.24 × 10²³ molecules CO₂

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.

1.53437 mol CO₂ ≈ 1.53 mol CO₂

Explanation:

How many neutrons are there in the nucleus of arsenic?42 neutrons

The nucleus consists of 33 protons (red) and 42 neutrons (blue).

0.836 mol Al

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Stoichiometry

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

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.

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.

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.

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

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:

Thus 26.67 moles of HCl would react completely with 8.89 moles of Al(OH)₃.

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

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

Answer Tu mama por si acaso

Explanation:

jkand

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

Answer:

Cu2 + 4 NH3 = Cu (NH3) 42+

so - - >

[Cu (NH3) 6] ^ 2+

Explanation:

Answer:

they are a lot tougher and are expecting only greatness, sort of like theater critiques.

Explanation:

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:

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

Answer:

16.09 kg

Explanation:

To solve this problem first we convert those 5.0 gallons of ethanol into liters:

Now we calculate the mass of that volume of ethanol, using its density:

We convert 18.9 L ⇒ 18.9 * 1000 = 18900 mL

Finally we convert the masses of the bottle and shipping container and packaging and add them to the mass of ethanol:

So the shipping weight would be 16088.04 g, or 16.09 kg

Answer: 1and 4

Explanation: iron is an element not an alloy. An ionic lattice is not bonded covalently.

Answer:

It is D !!

Explanation:

Just did test

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)

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.

Answer:

Calcium Hydroxide is an ionic compound

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  %

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.

The 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 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 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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