Why is a pencil used to mark the chromatogram instead of pen?

The extraction of iron from its ore involves reduction with carbon monoxide at high temperatures, yielding iron metal and carbon dioxide. The equilibrium partial pressures of CO(g) and CO2(g) can be determined by employing the kp equation with initial and equilibrium pressures.

The question is asking for the partial pressures of CO(g) and CO2(g) during the extraction of iron from its ore. Our reaction of interest is FeO(s) + CO(g) → Fe(s) + CO2(g), where kp = 0.403 at 1000°C. The reaction involves reducing FeO(s), iron(II) oxide, to Fe(s), i.e., iron metal, with carbon monoxide, or CO(g), in a high-temperature furnace. In the process, CO(g) is converted to CO2(g), or carbon dioxide gas. Given an initial pressure of CO(g) as 1.58 atm and that FeO(s) is in excess, at equilibrium, the partial pressure of CO(g) will be decreased as it is used up, while that of CO2(g) will be increased as it is produced.

From the kp equation [P of products / P of reactants], we have kp = PCO2 / PCO. We need to find the decrease in partial pressure of CO (x) such that the increase in partial pressure of CO2 equals x. This gives us PCO = (Initial P of CO) - x and PCO2 = x. Substituting these expressions into the kp equation, we get 0.403 = (x) / (1.58 - x). Solving this equation will yield the equilibrium pressures of CO(g) and CO2(g).

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The equilibrium partial pressures are approximately 0.454 atm for CO₂(g) and 1.126 atm for CO(g).

Firstly, we need to set up the equilibrium expression using the given Kp:

Kp = P(CO₂) / P(CO)
0.403 = P(CO₂) / (1.58 - x)
Assuming x is the change in pressure for both CO₂ and CO:

Kp = P(CO₂)/(1.58 − P(CO2)) = 0.403
Let P(CO₂) = y. Hence, 0.403 = y / (1.58 − y)
Solve for y (P(CO₂)):
0.403 (1.58 − y) = y
0.63734 = 1.403y
y = 0.63734 / 1.403 ≈ 0.454 atm

Thus, the equilibrium partial pressure of CO₂(g) is 0.454 atm, and for CO(g) it is 1.58 - 0.454 = 1.126 atm.

When 0.30 moles of water react with excess sodium, 0.15 moles of hydrogen gas are produced, judged by the 2:1 molar ratio between water and hydrogen in the reaction.

The reaction between water (H2O) and sodium (Na) produces sodium hydroxide (NaOH) and hydrogen gas (H2). The balanced chemical equation for this reaction is: 2Na + 2H2O -> 2NaOH + H2.

In this reaction, it's clear that the molar ratio between water and hydrogen gas is 2:1. That means, for every two moles of water consumed in the reaction, one mole of hydrogen gas is produced. If only 0.30 moles of water is reacted, then 0.30 / 2 = 0.15 moles of hydrogen gas would be produced.

So, in the reaction of 0.30 moles of water and excess sodium, 0.15 moles of hydrogen gas would be produced.

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The number of moles of NH₃ that are necessary to produce 0.824 mol N₂ is 0.6592 mol.

The mole is a SI unit of measurement that is used to calculate the quantity of any substance. Mass is defined as the product of the compound's molar mass and the moles of the substance.

Many compounds have a molar mass that may be estimated by dividing the compound's mass by the number of moles. A physical body's mass is the amount of matter it contains. Ammonia is a gas and nitrogen is also a gas.

4 mol NH₃ → 5 mol N₂

x mol NH₃ → 0.824 mol N₂

x = 0.824 x 4/5 = 0.6592 mol

Therefore, the number of moles of NH₃ that are necessary to produce 0.824 mol N₂ is 0.6592 mol.

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Heating the can increases the kinetic energy of the gas molecules.

Increasing the kinetic energy of the gas molecules increases the pressure of the gas on the can.

Crushing the can reduces its volume.

As volume decreases, the pressure inside the can increases because the gas molecules collide with the can’s walls more often.

If the pressure gets too high, the can may explode.

are the answers for edg

Heating can cause an increase in the kinetic energy of molecules. As the air is compressed the volume decreases and the pressure will be high.

Boyle’s law can be described as the pressure acted by a given mass of gas at a constant temperature of the gas being inversely proportional to the volume of the gas.

The pressure and volume are inversely proportional as long as the temperature is kept constant.

P ∝ 1/V

P₁.V₁ = P₂.V₂                                                    ...........(1)

The heating of the aerosol can cause an increase in the kinetic energy of gas molecules. When the air is compressed, its volume decreases, and the pressure will be high. As the temperature increased, the volume of the gas is also directly proportional to the temperature.

Therefore, the heating will increase the temperature and the volume of the compressed air. Therefore, it can explode in the presence of heat.

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B. A substance that donates electron to form a covalent bond

Answer: it is a weighted average of the masses of an element’s isotopes

Explanation:

Answer:

B

Explanation:

i just had the quiz for plato, the guy above is correct too, so brainliest to him

Answer:

a Cumbustion reaction, i just did it

Explanation:

Answer:

In metallic bonds the electrons of the valence shell can move freely within the metal, thus explaining its electric conductivity.

The mass percent of nitrogen in lead (II) nitrate (Pb(NO3)2) is calculated by dividing the total mass of nitrogen by the molecular mass of lead (II) nitrate and multiplying by 100%, which is approximately 8.46%.

To determine the mass percent of nitrogen in lead (II) nitrate (Pb(NO3)2), you need to find the total mass of nitrogen in the compound and divide it by the molecular mass of lead (II) nitrate. The molar mass of lead (II) nitrate is the sum of the mass of one lead atom, two nitrogen atoms, and six oxygen atoms. Thus, the molar mass of Pb(NO3)2 is 207.2 (mass of Pb) + 2(14.007) (mass of N) + 6(15.999) (mass of O) = 331.209 g/mol. The total mass of nitrogen is 2 × 14.007 g/mol = 28.014 g/mol.

To find the mass percent, we use the formula:

Mass percent of N = (Total mass of N / Molar mass of Pb(NO3)2) × 100%

Mass percent of N = (28.014 g/mol / 331.209 g/mol) × 100% ≈ 8.46%

The mass percent ( m ÷ m ) of a solution prepared by dissolving 55.84 g of NaCl in 152.7 g of H₂O is 26.78 %

Mass is a physical body's total amount of matter. Inertia, or the body's resistance to acceleration when a net force is applied, is also measured by this term.

The intensity of an object's gravitational pull to other bodies is also influenced by its mass. The kilogram is the primary mass unit in the SI.

The amount of matter that makes up every item or body is the greatest way to understand mass. Everything that we can see has mass. Examples of objects with mass include a table, a chair, your bed, a football, a glass, and even air.

m ( NaCl)   = 55.84 g  and m ( H2O ) = 157.2 g.

m (  solution) = m ( NaCl ) +  m ( H₂O )

w ( NaCl ) = 100 m ( NaCl ) ÷ m (  solution ) = 100 m   ( NaCl )  / ( m ( NaCl ) + m ( H₂O )

w ( NaCl ) = 100 × 55.84/  ( 55.84+152.7 ) = 26.78%

Thus, the mass percent ( m ÷ m ) of a solution prepared by dissolving 55.84 g of NaCl in 152.7 g of H₂O is 26.78 %

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Answer:

MnF₂*10H₂O.

Explanation:

Yes, salicylic acid is the limiting reactant. The theoretical yield is calculated using the moles of the limiting reactant and converting it to grams of the product. The percent yield is then determined by comparing the actual yield to the theoretical yield.

Yes, you are correct that salicylic acid is the limiting reactant in this reaction. The first step in this scenario is to calculate the theoretical yield, which is the quantity of product that would be produced assuming that the reaction proceeds perfectly and all of the limiting reactant is consumed. This is done by calculating the moles of the limiting reactant (salicylic acid), then using stoichiometry to convert this to moles of the product (acetylsalicylic acid), and finally converting this to grams. The next step is to calculate the actual yield, which is the amount of product that was actually produced in the reaction, and then use these values to calculate the percent yield using the formula:

Percent Yield = (Actual Yield / Theoretical Yield) x 100%

In this case, the actual yield is given as 1.39 g of acetylsalicylic acid. So, you would calculate the percent yield by dividing this value by the theoretical yield (which you calculated in the previous step) and then multiply by 100%.

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Answer:

Reactants or Products?

The answer is reactants.

Reactants Definition- A reactant is the chemical substances present at the start of a chemical reaction.

A products definition is the substance produced in a chemical reaction.

The answer is reactants because they start at the beginning of a chemical reaction, and have to interact with other substances to make a product. product is not able to interact with new substances, nor make new substances. Therefore, in a chemical reaction, if you want the substances to interact, and form new substances, it has to be a reactant.

A way to remember this is think of it as if  you are a reactant and you are interacting to form new substances.

The limiting reactant in the reaction is NaOH, 0.925 moles of Na2CO3 can be produced, and there would be 0.075 moles of CO2 remaining after the reaction is complete.

The given balanced reaction is: 2NaOH(aq) + CO2(aq) → Na2CO3(aq) + H2O(1). Firstly, let's identify the limiting reactant. For every mole of CO2, two moles of NaOH are required. Therefore, 1.85 moles of NaOH would react completely with 0.925 moles of CO2. But since we have 1.00 mol of CO2, our limiting reactant is NaOH.

Since the reaction produces 1 mole of Na2CO3 for every 2 moles of NaOH, we can expect to produce 0.925 moles of Na2CO3 based on the amount of our limiting reactant.

Finally, to determine the remaining amount of the excess reactant after the completion of the reaction, we subtract the amount of CO2 that reacted (0.925 moles) from the initial amount (1.00 mol), which gives us 0.075 moles of CO2 remaining.

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Answer: The correct answer is Option b.

Explanation:

The given reactions are the examples of single displacement reactions.

Single displacement reactions are defined as the reactions in which more reactive metal replaces the less reactive metal from its chemical reaction. The reactivity of metals is given by the series known as reactivity series.

The metals which lie above in the series can replace the metals which lie low in the reactivity series.

[tex]A+BX\rightarrow AX+B[/tex]

For the given options:

Option a: [tex]Ag+Cu^{2+}\rightarrow Ag^++Cu[/tex]

Silver lies low in the series than copper and hence is less reactive. Therefore, it will not replace copper. Thus, this is a non-spontaneous reaction.

Option b: [tex]Al+H^+\rightarrow Al^{3+}+H_2[/tex]

Aluminium lies above in the series than hydrogen and hence is more reactive. Therefore, it will easily replace hydrogen. Thus, this is a spontaneous reaction.

Option c: [tex]H_2+Al^{3+}\rightarrow H^++Al[/tex]

Hydrogen lies low in the series than aluminium and hence is less reactive. Therefore, it will not replace aluminium. Thus, this is a non-spontaneous reaction.

Option d: [tex]Na+K^+\rightarrow Na^++K[/tex]

Sodium lies low in the series than potassium and hence is less reactive. Therefore, it will not replace potassium. Thus, this is a non-spontaneous reaction.

Hence, the correct answer is Option b.

To determine the empirical formula of the compound given, we need to determine the ratio of the elements present in the compound. To do that we use the given amount of sample of the compound and the masses of each of the element included. Then, we calculate for the number of moles of each element. We do as follows:
                       mass                                       moles
Potassium       5.81                                       0.1486
Chlorine          5.27                                       0.1487
Oxygen           18.21 - 5.81 - 5.27 = 7.13     0.4456

Dividing the number of moles of each element with the smallest value of number of moles, we will have the ratio of the elements:

K = 1  Cl = 1 O = 3

Therefore, the empirical formula would be KClO3.

The empirical formula of the compound is KClO3.

To calculate the empirical formula, we need to determine the ratio of the different elements present in the compound. In this case, we have 5.81 g of potassium (K), 5.27 g of chlorine (Cl), and an unknown amount of oxygen (O).

To find the amount of oxygen, we subtract the combined mass of potassium and chlorine from the total mass of the compound: 18.21 g - (5.81 g + 5.27 g) = 7.13 g.

Now we can find the moles of each element by dividing their masses by their molar masses (K = 39.10 g/mol, Cl = 35.45 g/mol, O = 16.00 g/mol). The moles of each element are approximately K: 0.148, Cl: 0.149, O: 0.445.

Dividing these mole values by the smallest one (0.148), we find that the ratio of elements is approximately K: 1, Cl: 1, O: 3. Therefore, the empirical formula of the compound is KClO3.

After heating a CoCl₂ hydrate to remove water, the formula is determined using the mass of water lost and the molar masses of CoCl₂ and H₂O. The calculations show that every mole of CoCl₂ is associated with 6 moles of H₂O, giving the hydrate a formula of CoCl₂•6H₂O, known as cobalt(II) chloride hexahydrate.

To determine the formula of the hydrate of cobalt(II) chloride (CoCl₂ hydrate), you first need to calculate the mass of water lost during heating. The initial mass of the hydrate was 1.62 g and the mass after heating was 0.88 g. The mass of the water is therefore the difference between these two masses.

Mass of water lost = Initial mass \'96 Final mass = 1.62 g \'96 0.88 g = 0.74 g

Next, calculate the number of moles of CoCl₂ and H₂O. The molar mass of anhydrous CoCl₂ is 129.84 g/mol.

Moles of CoCl₂ = Mass of anhydrous CoCl₂ / Molar mass of CoCl₂ = 0.88 g / 129.84 g/mol = 0.006776 moles of CoCl₂

The molar mass of H₂O is approximately 18.015 g/mol.

Moles of H2O = Mass of water / Molar mass of H₂O = 0.74 g / 18.015 g/mol = 0.04107 moles of H₂O

To find the ratio of CoCl₂ to H₂O in the hydrate, divide the moles of water by the moles of CoCl₂.

Ratio = Moles of H₂O / Moles of CoCl₂ = 0.04107 / 0.006776 = 6.06, which rounds to 6.

The formula of the hydrate is CoCl₂•6H₂O. The full name of the hydrate is cobalt(II) chloride hexahydrate.