How many grams are in a sample of 7.9 moles of zinc?

Answer:

c

Explanation:

Answer:

P₂ = 1.05 atm

Explanation:

Given data:

Initial temperature = 24.0 °C (24+273 = 297 K)

Initial pressure = 0.900 atm

Final pressure = ?

Final temperature = 75 °C (75 + 273 =348 K)

Volume = constant

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

0.900 atm / 297 K = P₂/348 K

P₂ = 0.900 atm × 348 K / 297 K

P₂ = 313.2 atm. K /297 K

P₂ = 1.05 atm

Answer:

H+(aq) + OH-(aq) -> H2O(l)

Explanation:

This is neutralization

The volume of water added to dissolve potassium hydrogen phthalate (KHP) does not matter because the mass of KHP used is known and it will dissolve completely in any volume of water.

In volumetric analysis, the primary objective is to find the exact concentration of an analyte in a given solution. Analyte refers to the substance whose concentration is to be determined.In order to measure the analyte concentration, the known volume of the titrant of known concentration is added to the analyte until the endpoint is reached.Endpoint refers to the point in a titration where the reaction between the analyte and titrant is complete. The endpoint can be detected by observing a physical change in the system.In the case of KHP, it dissolves completely in any volume of water.

Therefore, the mass of KHP used can be accurately measured and dissolved in any volume of water. As a result, the volume of water added to dissolve the KHP does not affect the accuracy of the experiment.In summary, the volume of water added to dissolve KHP does not matter because the mass of KHP used is known and it will dissolve completely in any volume of water.

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Answer:

1.09 mL

Explanation:

Density is a measure of a substance's mass over its volume.

d = m/v

We can rearrange the equation to solve for volume, using algebra.

v = d/m

Therefore v = 6.35/5.80 = 1.09 mL

Chemistry =>Introduction to Chemistry => Scientific Method

A scientific method corresponds to a methodology to obtain new knowledge.

We must start from an idea, an assumption of how a compound or a process behaves, this is our hypothesis.

Following this, we must identify what can affect our process, what are the variables, and what will be the response variable, for this we carry out an experiment.

Once the experiments have been carried out, we must analyze the results, draw conclusions as to why the behavior occurs, and if our hypothesis is true or not.

It is useless for us to obtain new knowledge if we do not share it, We have to share the results, in this way other people can start from that knowledge to create another,

Therefore, the answer will be:

1. Make a hypothesis

2. Conduct an experiment

3. Analyze the experiment data

4. Communicate the results

The technical machinist should build a cubical steel tank with a smallest possible inside length of 0.65 meters in order to hold 280 liters of water.

To calculate the smallest possible inside length of the cubical steel tank, we need to determine the dimensions of the tank based on its volume and the fact that it is a cube.

Given that the tank needs to hold 280 liters of water, we can convert this volume to cubic meters by dividing by 1000. So, the volume of the tank is 280/1000 = 0.28 cubic meters.

Since the tank is a cube, all sides have the same length. Let's call this length "x". Therefore, the volume of the tank can be expressed as x * x * x = x^3.

Now we can set up the equation x^3 = 0.28 and solve for x. Taking the cube root of both sides, we find x = ∛0.28.

Using a calculator, we can find the cube root of 0.28 to be approximately 0.648. This gives us the length of one side of the cube.

Rounding this value to the nearest 0.01 meter, the smallest possible inside length of the tank is 0.65 meters.

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Answer:

Conditions to Avoid: Natural gas is extremely flammable and explosive; avoid heat, sparks, open flames, and all possible sources of ignition. Heat will increase pressure in containers used to store natural gas.Jun 1, 2015

Answer:

Natural Gas can be explosive or flammable depending on it's concentration in air.  

Natural gas has a flammability range of approximately 5 to 15 percent.

Any percentage greater than that is explosive for natural gas.

Hope this helps.

Answer:

.668 mole

Explanation:

1.67 * .4 = .668 mole

Answer:

0.497 moles/L

Explanation:

The reaction that takes place is:

First we calculate the moles of lactic acid in 0,821 g, using its molar mass:

One mole of lactic acid reacts with one mole of sodium hydroxide (it is a monoprotic acid), so in 18,34 mL of NaOH solution there are  9,122x10⁻³moles of NaOH:

Answer:

observation

Explanation: you observe something then create a question and a hypotesis

The first step in the Scientific Method is to make objective observations.

Hope this helps!

first you draw a table as I've drawn.

Since moles = mass÷RAM

divide the element with the lowest ram to it self and the other element to find ratio..

Then to the unknown number[n] Multiply it to the formula C H2 and equate it to 84..

n will be 6 hence C6 H12

Answer:

They help stablize the strucure of an atom.

Explanation:

Take into consider isotopes where there are more or less than the ideal amount of neurtrons. These isotopes are radioactive and unstable to the point hey are used as atomic bombs. So with the proper amount of nuetrons it helps the atom maintain structure and not degrade

Answer: they have an important role to keep the atom stable

Explanation:

since protons are positively charged, there is an incredibly strong repulsive force between all the protons in a nucleus

Thermochemistry is the study of the relationships between chemistry and energy. It involves understanding how energy, particularly in the form of heat, is transferred during chemical reactions and physical processes.

This field focuses on the measurement and calculation of heat and energy changes that occur during chemical reactions, as well as the relationship between temperature and chemical reactions. Understanding the principles of thermochemistry can provide valuable insights into the behavior of chemical reactions and help predict the outcomes of chemical processes. In the context of relationships, thermochemistry can also play a role in understanding the energy dynamics between individuals and the chemistry that underlies attraction and bonding.

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Picric acid and phenol, Salicylic acid and phenol & Benzylamine and aniline can be separated using liquid-liquid extraction but Triethylamine and diethylamine & 3-nitrobenzoic acid and 2-nitrobenzoic acid cannot be separated using liquid-liquid extraction.

1. Picric acid and phenol can be separated using liquid-liquid extraction. Picric acid is a stronger acid (pKa ~0.4) than phenol (pKa ~10). Adding aqueous NaOH will deprotonate picric acid and make it soluble in the aqueous layer, while phenol remains in the organic layer. Then, the two compounds can be separated.
2. Salicylic acid and phenol can also be separated using liquid-liquid extraction. Salicylic acid (pKa ~3) is more acidic than phenol (pKa ~10). Adding aqueous NaHCO3 will deprotonate salicylic acid, making it soluble in the aqueous layer, while phenol remains in the organic layer. The compounds can then be separated.
3. Triethylamine and diethylamine cannot be easily separated via liquid-liquid extraction, as both are bases (pKb values are similar). Aqueous HCl, NaOH, or NaHCO3 will not be effective in separating these compounds. Alternative separation methods, like distillation, may be needed.
4. 3-nitrobenzoic acid and 2-nitrobenzoic acid cannot be separated using liquid-liquid extraction, as they have similar acidity (pKa values are close) and will react similarly with HCl, NaOH, or NaHCO3. Alternative separation methods, like chromatography, should be considered.
5. Benzylamine and aniline can be separated using liquid-liquid extraction. Benzylamine is a weaker base (pKb ~4.2) than aniline (pKb ~9.4). Adding aqueous HCl will protonate aniline, making it soluble in the aqueous layer, while benzylamine remains in the organic layer. The two compounds can then be separated.

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Answer:

jkrifhcuhixjck

gvudd

Explanation:

dugucdsorfooggigj

a CUCO3(s) + ( I don't have the symbol on my phone ) delta CUo(s) + CO2(g)

b NH4NO3➡️ HNo3 + H2O

c. Ba(OH)2+CO2 ➡️ BaCO3+H20

d Na +H20 ➡️NaOH +h2

Explanation:

I think this should be it , I think that 8s the symbol for hydrogen gas if its not correct I'm sorry

Sodium is not a metal because it does not have the characteristic properties of a metal. In general, metals are known for their metallic luster, high thermal and electrical conductivity, and their ability to lose electrons to form positive ions.

Sodium, on the other hand, has a low melting point and boiling point, and is a very reactive element. It is a silvery-white metal that is highly reactive with water, causing it to catch fire and explode. This is because sodium is highly electropositive, meaning it easily loses electrons, and forms a positive ion (Na+). When sodium comes into contact with water, it reacts with the water molecules and forms sodium hydroxide (NaOH) and hydrogen gas (H2), which causes the explosion.

Additionally, Sodium has a relatively low density and is a relatively poor conductor of heat and electricity, compared to most metals.

In summary, Sodium is not classified as a metal because it does not possess the characteristic properties of a metal such as high thermal and electrical conductivity, metallic luster, and ability to lose electrons to form positive ions. Instead, it is a highly reactive and electropositive element that forms positive ions and reacts readily with water.

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The percent error introduced into the mass of CO2 if we did not correct for the buoyant force due to the displaced air, we need to compare the actual mass of CO2 with the measured mass of CO2.

The buoyant force is the upward force exerted on an object immersed in a fluid, in this case, air. When we measure the mass of CO2, we usually do it in air, and the buoyant force affects the measurement. To correct for the buoyant force, we need to subtract the buoyant force from the measured mass. The buoyant force is equal to the weight of the displaced air.

To calculate the percent error, we can use the following formula:

Percent Error = ((Actual Mass - Measured Mass) / Actual Mass) x 100 Since we want to know the percent error introduced if we did not correct for the buoyant force, we can use the formula:

Percent Error = ((Actual Mass - Measured Mass without correcting for buoyant force) / Actual Mass) x 100

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Answer: increasing volume

Explanation: adding a catalyst would increase reaction time and increasing  INCREASING concentration definently makes reaction time alot faster increasing pressure actually makes it more concentrated, so no it is not

Answer:

1. 0.422 atmospheres

2. 633281.25 Pascals

3. (a) Move up

(b) 868 mmHg

4. 868 mmHg

5. 775 mmHg

6. Partial pressure of He is 0.64 atm.

Partial pressure of oxygen is 1.29 atm.

Partial pressure of N is 2.57 atm.

7. 445.72 torr.

Explanation:

1. To convert 321  torr to atmospheres

1  atmosphere = 760 torr

∴ 1 torr = 1/760 atmospheres

Hence, 321 torr = 321 × 1/760 = 321/760 atmospheres = 0.422 atmospheres

2. To convert 6.25 atmospheres to Pascals, we have;

1 atmosphere = 101325 Pascals

∴ 6.25 atmospheres = 6.25 × 101325 Pascals = 633281.25 Pascals

3. (a) Here we have, given that the value of the pressure on the bottle = 830 mmHg, when the valve is opened, the mercury in the open-end arm will move up because the pressure of the gas inside the flask is more than the pressure on the other side of the open-end arm

(b) After the mercury stops moving the difference between the two columns will be the difference between the two pressures, that is 830 mmHg - 745 mmHg = 85 mmHg

4. From the diagram, it is seen that the differenc beteen the two columns is 123 mm, therefore, the pressure in the flask is 123 mmHg more than the external pressure, hence the pressure of the as in the flask = 745 mmHg + 123 mmHg = 868 mmHg

5. Here we have that the height of the mercury in the open-end is less than the height of the mercury on the arm closer to the flask, therefore, the pressure of the gas in the flask = 825 mmHg - 50 mmHg = 775 mmHg

6. Number of moles of He = 1 mole

Number of moles of oxygen, O = 2 mole

Number of moles of nitrogen, N = 4 mole

From Dalton's law of partial pressure we have that, the total pressure of a given mass of gas is equal to the partial pressure of the individual gases

\(That \ is \ \chi _i = \frac{n_i}{n_{total}} \ and \ P_i = \chi_i \cdot P_{total}\)

Hence;

Total number of moles = 1 + 2 + 4 = 7 moles

Mole fraction of He = 1/7

Partial pressure of He = 1/7×4.5 = 0.64 atm.

Mole fraction of oxygen, O = 2/7

Partial pressure of oxygen= 2/7×4.5 = 1.29 atm.

Mole fraction of N = 4/7

Partial pressure of N = 4/7×4.5 = 2.57 atm.

7. From Boyle's law

P₁×V₁ = P₂×V₂

Hence;

P₂ = P₁×V₁/V₂

Where:

P₁ = Initial pressure = 2.57 atm

V₁ = Initial volume =1.57 liters

V₂ = New volume = 6.88 liters

P₂ = New pressure = 2.57×1.57/6.88  = 0.59 atm.

To convert 0.59 atm. to torr, we multiply by 760 thus;

0.59 atm. = 0.59 × 760 torr = 445.72 torr.

Significant figures are important in scientific measurements because they indicate the precision and accuracy of the measurement, and ensure that calculations and conclusions based on those measurements are valid and reliable.

Significant figures are important in scientific measurements because they indicate the precision or accuracy of a measurement. The number of significant figures in a measurement represents the number of digits that are known with certainty plus one estimated digit.

It is important to use the correct number of significant figures when reporting measurements to ensure that the data is reliable and consistent. Using too few or too many significant figures can lead to incorrect calculations or conclusions. Therefore, scientists must be careful to use the appropriate number of significant figures when measuring and reporting data.

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--The complete question is, What is the importance of significant figures in scientific measurements?--

\(2 HCl + Mg(OH)_2\) → \(2 H_2O + MgCl_2\)

\(3 Ca(ClO)_2\) → \(2 CaCl_2\) + \(Ca(ClO_3)_2\)

\(2 KBr + Ca(NO_3)_2\) →\(2 KNO_3 + CaBr_2\)

\(2Al +6HCl\) → \(2AlCl_3 +3H_2\)

\(2C_2H_6+7O_2\) → \(4CO_2+6H_2O.\)

A balanced chemical reaction is an equation that has equal numbers of each type of atom on both sides of the arrow.

Balanced chemical equation:

\(2 HCl + Mg(OH)_2\) → \(2 H_2O + MgCl_2\)

\(3 Ca(ClO)_2\) → \(2 CaCl_2\) + \(Ca(ClO_3)_2\)

\(2 KBr + Ca(NO_3)_2\) →\(2 KNO_3 + CaBr_2\)

\(2Al +6HCl\) → \(2AlCl_3 +3H_2\)

\(2C_2H_6+7O_2\) → \(4CO_2+6H_2O.\)

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i) A is to B: hypoosmotic (Solution A has a lower osmolarity compared to Solution B). ii) B is to A: hyperosmotic (Solution B has a higher osmolarity compared to Solution A)

iii) A is to C: isosmotic (Solution A and Solution C have the same osmolarity)

iv) C is to A: isosmotic (Solution C and Solution A have the same osmolarity)

When you drink water, the osmolarity of body fluids will decrease. This is because water is a hypotonic solution compared to body fluids.

Hypotonic refers to a solution that has a lower solute concentration compared to another solution or a reference solution. In a hypotonic solution, there is a higher concentration of water molecules relative to solute particles.

By drinking water, you are diluting the solute concentration in the body, leading to a decrease in osmolarity. Therefore, the values related to osmolarity, such as the concentration of solutes in the body fluids, would decrease.

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0.50 mol SiO₂

Math

Pre-Algebra

Order of Operations: BPEMDAS

Chemistry

Atomic Structure

Step 1: Define

30 g SiO₂ (sand)

Step 2: Identify Conversions

Molar Mass of Si - 28.09 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of SiO₂ - 28.09 + 2(16.00) = 60.09 g/mol

Step 3: Convert

Step 4: Check

Follow sig figs and round. We are given 2 sig figs.

0.499251 mol SiO₂ ≈ 0.50 mol SiO₂

Answer:

\(\boxed {\boxed {\sf About \ 0.5 \ moles \ of \ SiO_2}}\)

Explanation:

To convert from grams to moles, we must use the molar mass.

1. Molar Mass

Use the Periodic Table to find the masses of the individual elements (silicon and oxygen) in sand.

Examine the formula for sand: SiO₂. There is a subscript of 2 after oxygen, so there must be 2 oxygen atoms. Multiply oxygen's mass by 2 and add silicon's mass to find the molar mass of sand.

2. Calculate Moles

Use the molar mass as ratio.

\(\frac{60.083 \ g \ SiO_2}{1 \ mol \ SiO_2}\)

Multiply by the given number of grams (30)

\(30 \ g \ SiO_2 * \frac{60.083 \ g \ SiO_2}{1 \ mol \ SiO_2}\)

Flip the fraction so the grams of sand will cancel.

\(30 \ g \ SiO_2 *\frac{1 \ mol \ SiO_2}{60.083 \ g \ SiO_2}\)

\(30 *\frac{1 \ mol \ SiO_2}{60.083 }\)

\(\frac{30 \ mol \ SiO_2}{60.083 }\)

\(0.499309289 \ mol \ SiO_2\)

3. Round

The original measurement of grams has 1 signfiicant figure. We must round our answer to 1 sig fig.

For the answer we found, that is the tenth place. The 9 in the hundredth tells us to round the 4 to a 5.

\(\approx 0.5 \ mol \ SiO_2\)

There are about 0.5 moles of SiO₂ in 30 grams.

Chemistry quizzes What is the mass  of a single carbon atom if a mole of carbon atoms weighs 12 grams. The fact that 1 mole of carbon atoms weighs 12 grams is a given.

There are 6. 022 10 23 atoms in total, or Avogadro's number, in a mole of carbon atoms. As a result, 1 carbon atom weighs 2 10 - 23 g (in grams). The weight of one mole of carbon atoms is 12 g. 12 g to 12 amu. Because we defined the mole to make it so, the atomic mass and molar mass are in agreement. A material can have a variable mass per mole while yet having the same number of particles. Are there any examples you might use to support the claim? In current usage, the term "mole" merely denotes a group of countable items, more specifically the Avogadro number of the entities in question.

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To carry out the experiment, follow the procedure described in task 1, part d. Perform three trials for each drop height and record the data in a table.

Remember to estimate heights to the nearest centimeter, and you may choose to reduce the simulation rate and watch the bounces in slow motion to improve data collection. Once you have recorded the data for all trials, average the bounce height measurements to get a final reading. Finally, round the average bounce heights to the nearest whole number. This will give you accurate data that can be used to analyze and draw conclusions. To carry out the experiment, first, set up the drop heights according to Task 1, Part D. Perform three trials for each height, ensuring you accurately estimate them to the nearest centimeter. You can slow down the simulation rate to observe bounces more easily and improve data collection. Record your findings in a table. After completing all trials, calculate the average bounce height for each drop height and round your results to the nearest whole number. This process will provide you with precise and reliable data for further analysis.

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Answer:

Explanation:

Ca++

CO3--

CaCO3