How can you tell if a sample contains baking soda and cornstarch or baking powder?

The given compound is made up of 71.65% chlorine, 24.27% carbon, and 4.07% hydrogen. It's molar mass is 98.96g/mol. To determine the molecular formula of the given compound, follow the steps given below: Step 1: Determine the empirical formula. The empirical formula can be determined from the percent composition of the compound. Assume that we have a 100-gram sample, then the number of grams of each element can be calculated:71.65 g Cl × (1 mol Cl/35.45 g Cl) = 2.02 mol Cl24.27 g C × (1 mol C/12.01 g C) = 2.02 mol C4.07 g H × (1 mol H/1.008 g H) = 4.04 mol H. Next, divide each number of moles by the smallest number of moles: Cl: 2.02 / 2.02 = 1C: 2.02 / 2.02 = 1H: 4.04 / 2.02 = 2The empirical formula of the compound is CH2Cl.Step 2: Calculate the empirical formula mass.

The empirical formula mass of CH2Cl is:1 × 12.01 (molar mass of C) + 2 × 1.008 (molar mass of H) + 1 × 35.45 (molar mass of Cl) = 49.48 g/mol. Step 3: Determine the scaling factor Divide the molar mass of the compound (98.96 g/mol) by the empirical formula mass (49.48 g/mol) to determine the scaling factor:98.96 g/mol ÷ 49.48 g/mol = 1.998The scaling factor is approximately 2, so multiply the subscripts in the empirical formula by 2 to get the molecular formula: Molecular formula = C2H4Cl2Thus, the molecular formula of the given compound is C2H4Cl2.

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Answer:

a

Explanation:

Answer:

48546.7kg or 48546745g

Explanation:

so from this u can work out the amount of moles in phosphorous by doing mass / mr you have to convert the mass in kg to g so you times it by 1000. then divide it by 31 which is the mr of phosphorous. then u can use the molar ratio which is 2:1 . Then use the equation mass= moles*mr

so 97000*1000/31=312903moles

2:1

so 312903/2=156451 moles of ca3(PO4)2

so mass= moles*mr

156451*310.3=48494g

hope this helps u to understand(*°▽°*)

Answer:

6

Explanation:

Answer: 6

Explanation:

I just took this thang

Answers:

n = mass/Mr

mass = n × Mr

Hence , mass = 7.8 × 95

= 741 grams

Answer: D: sun

Explanation:

Answer:

iron, magnesium, and calcium but low in potassium and sodium.

Edible mushrooms: Consuming edible mushrooms is safe and provides health advantages like fiber, vitamins, and minerals.

Non-Edible mushrooms: Mushrooms that cannot be eaten could be harmful or have unappealing flavors and textures that could be harmful if consumed.

Answer:

Oxides of Nitrogen (NOx)

NOx is a collective term used to refer to two species of oxides of nitrogen: nitric oxide (NO) and nitrogen dioxide (NO2).

Annual mean concentrations of NO2 in urban areas are generally in the range 10-45 ppb (20-90 µgm-3). Levels vary significantly throughout the day, with peaks generally occurring twice daily as a consequence of "rush hour" traffic. Maximum daily and one hourly means can be as high as 200 ppb (400 µgm-3) and 600 ppb (1200 µgm-3) respectively.

Globally, quantities of nitrogen oxides produced naturally (by bacterial and volcanic action and lightning) far outweigh anthropogenic (man-made) emissions. Anthropogenic emissions are mainly due to fossil fuel combustion from both stationary sources, i.e. power generation (21%), and mobile sources, i.e. transport (44%). Other atmospheric contributions come from non-combustion processes, for example nitric acid manufacture, welding processes and the use of explosives.

Sulphur Dioxide (SO2)

SO2 is a colourless gas. It reacts on the surface of a variety of airborne solid particles, is soluble in water and can be oxidised within airborne water droplets.

Annual mean concentrations in most major UK cities are now well below 35 ppb (100 µgm-3) with typical mean values in the range of 5-20 ppb (15-50 µgm-3). Hourly peak values can be 400-750 ppb (1000-2000 µgm-3) on infrequent occasions. Natural background levels are about 2 ppb (5 µgm-3).

The most important sources of SO2 are fossil fuel combustion, smelting, manufacture of sulphuric acid, conversion of wood pulp to paper, incineration of refuse and production of elemental sulphur. Coal burning is the single largest man-made source of SO2 accounting for about 50% of annual global emissions, with oil burning accounting for a further 25-30%.

Carbon Monoxide (CO)

Carbon Monoxide is a colourless, odourless, tasteless gas that is slightly lighter than air.

Natural background levels of CO fall in the range of 10-200 ppb. Levels in urban areas are highly variable, depending upon weather conditions and traffic density. 8-hour mean values are generally less than 10 ppm (12 mgm-3) but have been known to be as high as 500 ppm (600 mgm-3).

CO is an intermediate product through which all carbon species must pass when combusted in oxygen (O2). In the presence of an adequate supply of O2 most CO produced during combustion is immediately oxidised to carbon dioxide (CO2). However, this is not the case in spark ignition engines, especially under idling and deceleration conditions. Thus, the major source of atmospheric CO is the spark ignition combustion engine. Smaller contributions come from processes involving the combustion of organic matter, for example in power stations and waste incineration.

Ozone (O3)

O3 is the tri-atomic form of molecular oxygen. It is a strong oxidising agent, and hence highly reactive.

Background levels of O3 in Europe are usually less than 15 ppb but can be as 100 ppb during summer time photochemical smog episodes. In the UK ozone occurs in higher concentrations during summer than winter, in the south rather than the north and in rural rather than urban areas.

Most O3 in the troposphere (lower atmosphere) is formed indirectly by the action of sunlight on nitrogen dioxide - there are no direct emissions of O3 to the atmosphere. About 10 - 15% of tropospheric O3 is transported from the stratosphere where it is formed by the action of ultraviolet (UV) radiation on O2. In addition to O3, photochemical reactions involving sunlight produce a number of oxidants including peroxyacetyl nitrate (PAN), nitric acid and hydrogen peroxide, as well as secondary aldehydes, formic acid, fine particulates and an array of short lived radicals. As a result of the various reactions that take place, O3 tends to build up downwind of urban centres where most of NOx is emitted from vehicles.

Explanation:

From the structure of SF4 shown, the molecular geometry of the molecule is trigonal bipyramidal.

The term molecular geometry has to do with the arrangement of the electron pairs in a molecule.

The arrangement of electron pair in a molecule is based on the valence shell electron pair repulsion theory.  From the structure of SF4 shown, the molecular geometry of the molecule is trigonal bipyramidal.

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Answer:

3.57 m

Explanation:

Expressed in the correct number of significant digits, The product of the number 1000 and the measurement 0.00357 m will give us;

1000 × 0.00357 = 3.57 m

The correct number of significant figures is three significant figures as seen in 3.57 m

Answer:

this equation is not proper see that where is the reactant.

Explanation:

give give a proper question and I will

if fecl2 + c2 gives a fecl3 where does the carbon compound go

Answer:

2FeCl2 + Cl2 → 2FeCl3

Explanation:

Answer:

\(56 \times { \frac{01514344}{?} }^{2} 5566648443hffii51 \\ \div 232333\)

Answer:

write a letter to the presiding member of your district assessment telling him or her about two of the achievement of your community over the last five years and the plans for the future

Approximately 0.038 grams of hydrogen.

To find the mass of hydrogen produced in the reaction, we can use the ideal gas law equation:

PV = nRT

where:

P = total pressure of the gas (converted to atm) = 1.056 atm

V = volume of the gas (converted to liters) = 465 mL = 0.465 L

n = number of moles of the gas (hydrogen)

R = ideal gas constant = 0.0821 L·atm/(mol·K)

T = temperature of the gas (converted to Kelvin) = 42°C + 273.15 = 315.15 K

First, we need to calculate the partial pressure of hydrogen gas. The total pressure is the sum of the partial pressure of hydrogen and the vapor pressure of water:

The partial pressure of hydrogen = Total pressure - Vapor pressure of water

Converting the vapor pressure of water from torr to atm:

Vapor pressure of water = 32 torr / 760 torr/atm = 0.042 atm

Partial pressure of hydrogen = 1.056 atm - 0.042 atm = 1.014 atm

Now, we can rearrange the ideal gas law equation to solve for moles (n):

n = PV / RT

Putting the values:

n = (1.014 atm * 0.465 L) / (0.0821 L·atm/(mol·K) * 315.15 K)

Calculating the value:

n ≈ 0.0188 moles

The molar mass of hydrogen is approximately 2.016 g/mol. To find the mass of hydrogen produced, we can multiply the number of moles by the molar mass:

Mass = n * molar mass

Mass = 0.0188 moles * 2.016 g/mol

Calculating the value:

Mass ≈ 0.038 g

Therefore, approximately 0.038 grams of hydrogen were produced in the reaction.

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To determine Eo for the given reaction, we can use the equation:  Eo(cell) = Eo(cathode) - Eo(anode)

The reduction potential for the cathode is the reduction potential of Ti²⁺, which is -1.63 V.

The reduction potential for the anode is the reduction potential of Fe³⁺, which is 0.77 V.

Plugging the values into the equation, we have:

Eo(cell) = (-1.63 V) - (0.77 V)

Eo(cell) = -2.40 V

Therefore, the standard cell potential (Eo) for the given reaction is -2.40 V.

This negative value indicates that the reaction is not spontaneous under standard conditions. The electrons flow from the anode (Fe³⁺) to the cathode (Ti²⁺), resulting in a negative cell potential. The reaction would require an external energy source to proceed.

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Answer:

Most solar cells are made from silicon—the same semiconductor material that is at the heart of computers. The cells are expensive to produce because it takes a great deal of energy to purify the silicon.

Answer:

Explanation:

The density of a substance can be found by using the formula

\(density = \frac{mass}{volume} \\\)

From the question

mass of sphere = 4000 g

Volume of a sphere is given by

\(V = \frac{4}{3} \pi {r}^{3} \\ \)

where r is the radius

\(r = \frac{diameter}{2} \\ \)

From the question

diameter = 150 cm

\(r = \frac{150}{2} = 75 \: \: \: cm\)

The volume of the sphere is

\(V = \frac{4}{3} \times {75}^{3} \pi \\ = \frac{4}{3} \times 421875\pi \\ = 562500\pi \\ = 1767145.86...\)

We have the answer as

volume = 1767145.86 cm³

So we have

\(density = \frac{4000}{1767145.86} \\ = 0.002263536...\)

We have the final answer as

Hope this helps you

Answer:

Base Alkali

1)All bases are not alkali 1)All alkali are bases

2)It neutralizes acids 2) It releases OH- ions, accepts a proton

3)Example: Zinc hydroxide, copper oxide 3)Example: potassium hydroxide, sodium hydroxide

To solve such this we must know the concept of chemical reaction. Therefore, the rate of reaction increases as the concentration of HCl increases.

Chemical reaction is a process in which two or more than two molecules collide in right orientation and energy to form a new chemical compound. The mass of the overall reaction should be conserved. There are so many types of chemical reaction reaction like combination reaction, double displacement reaction.

The rate of reaction depends on the number of collisions among the reactants and their orientation. As the number of concentration of reactants  increases, the number of collisions increases and the rate of reaction also increases.

Therefore, the rate of reaction increases as the concentration of HCl increases.

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Answer:

The answer is

Explanation:

To find the number of atoms in an element given it's number of moles we use the formula

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question

n = 7.2 mol

The number of atoms in iron ( Fe) is

N = 7.2 × 6.02 × 10²³

We have the final answer as

Hope this helps you

The FALSE statement among the given options is (b) A saturated aqueous solution of AgCl is predicted to exhibit an approximately neutral pH at 25°C.

When AgCl dissolves in water, it reacts with water molecules to form H+ and OH- ions, which leads to an acidic solution. Therefore, a saturated aqueous solution of AgCl is predicted to exhibit an acidic pH, not a neutral pH.Option (a) is true because AgCl is more soluble in pure water than in 0.10 M HCl due to the common-ion effect. Option (c) is false because Ag2CO3 is more soluble in 0.10 M HCl than in pure water. Option (d) is true because the formation of the complex ion Ag(CN)2− increases the solubility of AgCl in the presence of excess CN-.

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Barium sulfate has a solubility of approximately 2.80x10^-3 g/L or 2.80 mg/L (2.80 ppm) at 30.0 degrees Celsius, requiring approximately 357 liters of water to dissolve 1.00 g of the compound.

The solubility of barium sulfate in water can be calculated using the given molar solubility at 30.0 degrees Celsius. The molar solubility is 1.20x10^-5 M.

a. To calculate the solubility in grams per liter (g/L), we need to convert the molar solubility to grams of barium sulfate. The molar mass of BaSO4 is 233.4 g/mol.

Molar solubility = 1.20x10^-5 M

Molar mass of BaSO4 = 233.4 g/mol

Solubility (g/L) = Molar solubility (M) x Molar mass (g/mol)

                 = (1.20x10^-5 M) x (233.4 g/mol)

                 = 2.80x10^-3 g/L

Therefore, the solubility of barium sulfate in water at 30.0 degrees Celsius is 2.80x10^-3 g/L.

b. To determine the volume of water required to dissolve 1.00 g of barium sulfate, we can use the solubility value calculated in part (a).

Solubility (g/L) = 2.80x10^-3 g/L

Mass of barium sulfate = 1.00 g

Volume (L) = Mass (g) / Solubility (g/L)

            = 1.00 g / 2.80x10^-3 g/L

            = 357 L

Therefore, approximately 357 liters of water are required to dissolve 1.00 g of barium sulfate.

c. The solubility of barium sulfate can also be expressed in parts per million (ppm). To calculate this, we need to convert the solubility in grams per liter to milligrams per liter (mg/L) and then multiply by 10^3.

Solubility (g/L) = 2.80x10^-3 g/L

Solubility (mg/L) = Solubility (g/L) x 10^3

                  = 2.80x10^-3 g/L x 10^3

                  = 2.80 mg/L

Therefore, the solubility of barium sulfate in water is 2.80 mg/L, or 2.80 ppm.

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To determine the number of moles of water contained in 96.0 g, we need to use the molar mass of water. The molar mass of a substance is the mass of one mole of that substance, and it is calculated by adding up the atomic masses of all the atoms in the chemical formula.

The chemical formula for water is H2O, indicating that each molecule of water contains two hydrogen atoms and one oxygen atom. The atomic masses of hydrogen and oxygen are approximately 1 g/mol and 16 g/mol, respectively.

To calculate the molar mass of water, we multiply the atomic mass of hydrogen by 2 (since there are two hydrogen atoms in water) and add it to the atomic mass of oxygen:

Molar mass of water = (2 x 1 g/mol) + (1 x 16 g/mol) = 18 g/mol

Now, we can use the molar mass to determine the number of moles in 96.0 g of water. We divide the given mass by the molar mass:

Number of moles = Mass / Molar mass = 96.0 g / 18 g/mol ≈ 5.33 mol

Therefore, there are approximately 5.33 moles of water in 96.0 g of water.

It is important to note that the molar mass of water can be rounded to three decimal places since the given mass has only three significant figures (96.0 g).

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The word equation that represents the violent reaction between sodium and water is as follows: sodium + water → sodium hydroxide + hydrogen.

A chemical reaction is the process, typically involving the breaking or making of interatomic bonds, in which one or more substances are changed into others.

According to this question, sodium (Na) and water (H2O) are involved in a chemical reaction to produce sodium hydroxide (NaOH) and hydrogen gas (H2).

Therefore, the word equation that represents the violent reaction between sodium and water is as follows: sodium + water → sodium hydroxide + hydrogen

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Answer: D. If the reaction occurs in the gas phase

Explanation:

Answer:

D is correct via A P e x

Explanation:

High levels of photochemical smog are primarily caused by nitrogen dioxide (NO2), sulfur dioxide (SO2), and volatile organic compounds (VOCs).

Photochemical smog is a type of air pollution that forms when sunlight reacts with certain pollutants in the atmosphere. Nitrogen dioxide (NO2), which is emitted from vehicles and industrial processes, is a key contributor to the formation of photochemical smog. Sulfur dioxide (SO2), primarily released from burning fossil fuels, also plays a role in smog formation.

Additionally, volatile organic compounds (VOCs), which come from sources like vehicle emissions and industrial solvents, contribute to the chemical reactions that lead to smog formation. These three pollutants, along with sunlight and other atmospheric conditions, interact to produce the characteristic hazy and polluted air associated with photochemical smog.

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The dispersion and mixing of particles would be made easier through the application of ultrasonic waves.

Ultrasonic waves can facilitate the dispersion and mixing of particles in an experimental procedure. When ultrasonic waves are applied, they generate high-frequency sound waves that create alternating compression and rarefaction waves in a liquid medium.

These waves produce tiny bubbles due to the phenomenon of cavitation. During cavitation, the bubbles rapidly expand and collapse, creating localized areas of high pressure and temperature.

This process exerts mechanical forces on the surrounding particles, leading to their effective dispersion and mixing. The energy from ultrasonic waves helps to break down agglomerates, disperse fine particles, and enhance the overall homogeneity of the mixture.

The application of ultrasonic waves can be particularly beneficial in procedures such as sample preparation, emulsification, dispersion of nanoparticles, and dissolution of substances. It improves the efficiency and effectiveness of processes that require uniform distribution and thorough mixing of components.

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