Which statement correctly describes the actual yield and the theoretical yield of a reaction? (1 point)
The actual yield is calculated from the reactant amounts, but the theoretical yield must be measured for each instance of a reaction
The actual yield is calculated from the amount of the limiting reactant, and the theoretical yield is calculated from the amount of the excess
The actual yield depends on the reaction conditions, but the theoretical yield varies only with reactant amounts.
The actual yield represents the maximum yield possible, and the theoretical yield assumes perfect reaction conditions.

Answer:

Her speed is 1.1 m/s, and her velocity is 0 m/s.

Explanation:

Hello!

In this case, since the speed is the defined as the distance traveled over the elapsed time:

[tex]s=\frac{d}{t}[/tex]

And the velocity is defined as the change in displacement over the time interval:

[tex]v=\frac{\Delta d}{\Delta t}[/tex]

Thus, since the total distance traveled was 400 m and the total time 6 mins (360 s), we compute the speed as:

[tex]s=\frac{400m}{360s}=1.1m/s[/tex]

And the velocity is 0 m/s because the initial point is the very same final point as the track was circular. Therefore the answer is Her speed is 1.1 m/s, and her velocity is 0 m/s.

Best regards!

Explanation:

Both cohesion and molecular interchange contribute to liquid viscosity. The impact of increasing the temperature of a liquid is to reduce the cohesive forces while simultaneously increasing the rate of molecular interchange. The former effect causes a decrease in the shear stress while the latter causes it to increase.

temperature?

The viscosity of liquids decreases rapidly with an increase in temperature, and the viscosity of gases increases with an increase in temperature. Thus, upon heating, liquids flow more easily, whereas gases flow more sluggishly.

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Answer: The ratio of number of hydroxide ions to iodide ions is 2 : 1.

Explanation:

The chemical equation for the oxidation of iodide ion is oxidized to hypoiodite ion by permanganate follows:

[tex]2MnO_4^-+I^-+H_2O\rightarrow 2MnO_2(s)+IO_3^{-}+2OH^{-}[/tex]

According to mole concept:

1 mole of a substance contains [tex]6.022\times 10^{23}[/tex] number of particles

Moles of iodide ions = 1 mole

Number of iodide ions = [tex](1\times 6.022\times 10^{23}[/tex]

Moles of hydroxide ions = 2 mole

Number of hydroxide ions = [tex](2\times 6.022\times 10^{23}[/tex]

Taking the ratio of number of hydroxide ions and number of iodide ions are as follows:

[tex]\frac{\text{Number of hydroxide ions}}{\text{Number of iodide ions}}=\frac{(2\times 6.022\times 10^{23})}{(1\times 6.022\times 10^{23})}\\\\\frac{\text{Number of hydroxide ions}}{\text{Number of iodide ions}}=\frac{2}{1}[/tex]

Hence, the ratio of number of hydroxide ions to iodide ions is 2 : 1.

Answer:

air

Explanation:

Vocal folds vibrate when excited by aerodynamic phenomena; they are not plucked like a guitar string. Air pressure from the lungs controls the open phase. The passing air column creates a trailing “Bernoulli effect,” which controls the close phase.

Answer:

95.7 cal

Explanation:

The heat required can be calculated as follows:

heat = m x Cp x ΔT

Where:

m = mass of iron = 87 g

Cp = specific heat of iron = 0.110 cal/g.°C

ΔT = change in temperature = final T - initial T = 40°C - 30°C = 10°C

Thus, we introduce the data in the mathematical equation to calculate the heat in calories:

heat = 87 g x 0.110 cal/g.°C x 10°C = 95.7 cal

Answer:

iron (III) oxide =Fe2O3

iron(III) carbonate =Fe2(CO3)3

Answer:

[tex]Q=1.9x10^8J[/tex]

Explanation:

Hello!

In this case, since we first know the heat and mass of the first experiment, we are able to compute enthalpy of vaporization of gasoline as shown below:

[tex]Q=m\Delta _{vap} H\\\\\Delta _{vap} H=\frac{11kcal}{1.0g} =11\frac{kcal}{g}[/tex]

Next, we need to the compute the grams in 1.5 gallons of gasoline via its density with the proper units:

[tex]m_{gasoline}=1.5gal*\frac{3785.41mL}{1gal}*\frac{0.74g}{1mL} =4202g[/tex]

Therefore, the new joules are computed via:

[tex]Q=4202g*11\frac{kcal}{g}*\frac{1000cal}{1kcal}*\frac{4.184J}{1cal}\\\\Q=1.9x10^8J[/tex]

Best regards!

Answer:

48g

Explanation:

2Hg(l) + O₂(g) => 2HgO

44g      excess        ?

44g/200.59g·mol⁻¹ = 0.219 mole Hg(l) = 0.219 mole HgO(s) produced.*

*Since coefficients are equal for Hg and HgO then the moles of HgO produced is the same as moles Hg used.

Convert 0.219 mole HgO to grams => 0.219mol x 216.95g/mol = 47.512g HgO ≅ 48g (2 sig figs)

To calculate the atoms of an element in a given molecule, we need to multiply stoichiometry by the number that is written on the foot of that element. The correct option is option C.

Balanced equation is the one in which the total number of atoms of a species on reactant side is equal to the total number of atoms on product side. The mass of the overall reaction should be conserved. There are so many types of chemical reaction reaction like combination reaction, displacement reaction.

The other characteristic of balanced reaction is that physical state should be written with each compound or molecule on reactant and product side. Physical state should be written in brackets. s means solid, l means liquid, g means gas.

2Hg(l) + O₂(g) [tex]\rightarrow[/tex] 2HgO

44g      excess        ?

The mole ratio between Hg and HgO is 1:1.

44g÷200.59g/mol= 0.219 mole of Hg= 0.219 mole of HgO

mass of HgO=0.219mol x 216.95g/mol

                     = 47.512g

Therefore, the correct option is option C.

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Answer: The molar enthalpy change is 73.04 kJ/mol

Explanation:

[tex]HCl+NaOH\rightarrow NaCl+H_2O[/tex]

moles of HCl= [tex]molarity\times {\text {vol in L}}=0.415mol/L\times 0.1=0.0415mol[/tex]

As NaOH is in excess 0.0415 moles of HCl reacts with 0.0415 moles of NaOH.

volume of water = 100.0 ml + 50.0 ml = 150.0 ml

density of water = 1.0 g/ml

mass of water = [tex]volume \times density=150.0ml\times 1.0g/ml=150.0g[/tex]

[tex]q=m\times c\times \Delta T[/tex]

q = heat released

m = mass  = 150.0 g

c = specific heat = [tex]4.184J/g^0C[/tex]

[tex]\Delta T[/tex] = change in temperature = [tex]4.83^0C[/tex]

[tex]q=150.0\times 4.184\times 4.83[/tex]

[tex]q=3031.3J[/tex]

Thus 0.0415 mol of HCl produces heat = 3031.3 J

1 mol of HCL produces heat = [tex]\frac{3031.3}{0.0415}\times 1=73043.3J=73.04kJ[/tex]

Thus molar enthalpy change is 73.04 kJ/mol

_____________________________________________

M = m/v

= 100ml ÷ 2 spoons × 100%

= - 5,000 μg/ppb³

= 50% Diluted

M = m/v

= 200ml ÷ 5 spoons × 100%

= - 4,000 μg/ppb³

= 40% Diluted

M = m/v

= 300ml ÷ 6 spoons × 100%

= - 5,000 μg/ppb³

= 50% Diluted

M = m/v

= 600ml ÷ 8 spoons × 100%

= - 75,000 μg/ppb³

= 75% Diluted

_____________________________________________

Answer: 1.8 moles Fe and 2.7 moles [tex]CO_2[/tex] are produced.

Explanation:

The balanced chemical reaction is:

[tex]Fe_2O_3+3CO\rightarrow 2Fe+3CO_2[/tex]  

According to stoichiometry :

3 moles of [tex]CO[/tex] require 1 mole of [tex]Fe_2O_3[/tex]

Thus 2.7 moles of [tex]CO[/tex] will require=[tex]\frac{1}{3}\times 2.7=0.9moles[/tex]  of [tex]Fe_2O_3[/tex]

Thus [tex]CO[/tex] is the limiting reagent as it limits the formation of product and [tex]Fe_2O_3[/tex] is the excess reagent.

As 3 moles of [tex]CO[/tex] give = 2 moles of [tex]Fe[/tex]  and 3 moles of [tex]CO_2[/tex]

Thus 2.7 moles of [tex]CO[/tex] will give =[tex]\frac{2}{3}\times 2.7=1.8moles[/tex]  of [tex]Fe[/tex]  and [tex]\frac{3}{3}\times 2.7=2.7moles[/tex]  of [tex]CO_2[/tex]

Thus 1.8 moles Fe and 2.7 moles [tex]CO_2[/tex] are produced.

Answer:

a) 15.3 mol O₂

b) 10.2 mol CO₂; 13.6 mol H₂O

Explanation:

Step 1: Write the balanced equation

2 C₃H₇OH + 9 O₂ ⇒ 6 CO₂ + 8 H₂O

Step 2: Calculate the moles of O₂ that react with 3.40 moles of C₃H₇OH

The molar ratio of C₃H₇OH to O₂ is 2:9. The moles of O₂ required are 9/2 × 3.40 mol = 15.3 mol

Step 3: Calculate the moles of CO₂ produced from 3.40 moles of C₃H₇OH

The molar ratio of C₃H₇OH to CO₂ is 2:6. The moles of CO₂ produced are 6/2 × 3.40 mol = 10.2 mol

Step 4: Calculate the moles of H₂O produced from 3.40 moles of C₃H₇OH

The molar ratio of C₃H₇OH to H₂O is 2:8. The moles of H₂O produced are 8/2 × 3.40 mol = 13.6 mol

Answer:

Answers with detail are given below.

Explanation:

C₆H₁₂O₆   →   2C₂H₅OH  + 2CO₂

Anaerobic respiration in plants produced ethanol which if accumulate then cause the harmful effect in plants. It is also occur in some microorganisms such as yeast.

C₆H₁₂O₆    →   2C₃H₆O₃

Anaerobic respiration in animals pyruvate converted into lactic acid and it is not as harmful as ethanol in plant if accumulate. It is produced during exercise. It can produce the cramps which can be cured with massage.

C₆H₁₂ + O₂       →       CO₂ + H₂O

This reaction is the combustion reaction of cyclohexane. Cyclohexane burnt in the presence of oxygen and form water and carbon dioxide.

Answer:

Explanation:

I HOPE IT HELPS :)

Answer:

89.6 F

Explanation:

Brain-List?

Answer:

C

cell wall only in plants

chloroplast only in plants

enlarged vacuoles only in plants

cell membrane in both

hope this helps :)

Explanation:

Answer:

a. cell wall b. membrane

Answer:

0.350 g of iron

Explanation:

Step 1: Given data

Mass of iron (m): 350 mg

Step 2: Convert the mass of iron to milligrams

In order to convert the mass of iron from grams to milligrams we need a conversion factor. In this case, the conversion factor is 1 g = 1,000 mg.

350 mg Fe × 1 g Fe/1,000 mg Fe = 0.350 g Fe

350 milligrams of iron is equal to 0.350 grams of iron. We conserve the 3 significante figures of the original data.

Answer:

Amount (Mole) of carbon = 0.008303 mole

Mass (gramm)of Carbon = 0.0997 g.

Explanation:

From Avogadro's law, we know that 1 mole of carbon contains 6.022×10²³ atoms.

Then the mole of carbon that contains 5.0×10²¹ atoms can be computed as (5.0×10²¹ / 6.022×10²³)

=0.008303 mole

5.0×10²¹ atoms is contained in 0.008303 mole

Hence, Amount (Mole) of carbon = 0.008303 mole

the mass of carbon can be computed , we know that

Mole = mass /Molar mass

Where Molar mass of carbon = 12.01 g/mol

n=0.008303 mol

Making " mass" subject of the formula,

mass=Mole ,× Molar mass

=0.008303 x 12.01

= 0.0997 g.

Answer:

Ag+o ___>2Ag+3o

I think is answer

Answer:

4Ag  +  O₂   →    2Ag₂O

Explanation:

Given reaction expression:

               Ag  +  O₂   →    Ag₂O

The problem here is to balance the expression.

We are going to use a mathematical approach to solve this problem. Therefore, assign coefficients a,b and c to the species:

                     aAg  +  bO₂   →    cAg₂O

Conserving Ag;   a  = 2c

                    O;     2b  = c

Now let c = 1;

              a  = 2

              b  = [tex]\frac{1}{2}[/tex]  

Multiply a, b and c through by 2;

            a  = 4, b = 1 and c  = 2

                       4Ag  +  O₂   →    2Ag₂O

Answer:

It is always twice the value of the actual yield.

Explanation:

Answer:

Yes, water molecules becomes gas particles when the vapor pressure is lower than the external atmospheric temperature.

Explanation:

Vapor pressure is defined as the pressure of the vapor that lies above its surface. In other words, it is the pressure of the vapor which results from the evaporation of a liquid which is above a liquid in a closed or open container.

The liquid starts boiling or evaporation takes place when the vapor pressure of the liquid becomes equal to the external or atmospheric pressure. Now when the vapor pressure is less than the atmospheric pressure, the liquid boils at a higher temperature while when vapor pressure is more than the atmospheric temperature, the liquid starts boiling a lower temperature.

No water molecule is converted into gas when the atmospheric pressure is higher than vapour pressure.

No, water molecules will not become gas particles when the vapor pressure is lower than atmospheric pressure because of the higher pressure of surrounding environment on the water molecules. The water in liquid form is converted into gas form and evaporated when the vapour pressure is equal or higher than atmospheric pressure.

So if the vapour pressure is lower than the atmospheric pressure than the water molecules will not become gas particle so we can conclude that no water molecule is converted into gas when the atmospheric pressure is higher than vapour pressure.

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Answer:

CH₂

Explanation:

Given parameters:

Percentage composition:

          Carbon  = 40.1%

          Hydrogen  = 6.6%

Unknown:

Empirical formula of the compound  = ?

Solution:

The empirical formula of a substance is its simplest formula.

 Elements                             Carbon                             Hydrogen

Percentage

Composition                           40.1                                     6.6

Molecular mass                        12                                         1

Number of moles                  40.1/12                                  6.6/1

                                                3.342                                    6.6

Divide through by

the smallest                         3.342/3.342                           6.6/3.342

                                                      1                                        2

So the empirical formula of the compound is CH₂

Answer:

2000 millimoles of AlCl₃

Explanation:

From the question given above, the following data were obtained:

Volume of solution = 1.8 L

Molarity of solution = 1.1 mol /L

Millmole of AlCl₃ =?

Next, we shall determine the number of mole of AlCl₃ in the solution.

This can be obtained as follow:

Volume of solution = 1.8 L

Molarity of AlCl₃ solution = 1.1 mol /L

Number of mole of AlCl₃ =?

Molarity = mole /Volume

1.1 = Number of mole of AlCl₃ / 1.8

Cross multiply

Number of mole of AlCl₃ = 1.1 × 1.8

Number of mole of AlCl₃ = 1.98 moles

Finally, we shall convert 1.98 moles to millimoles. This can be obtained as follow:

1 mole = 1000 millimoles

Therefore,

1.98 mole = 1.98 mole × 1000 millimoles / 1 mole

1.98 mole = 1980 millimoles

1.98 mole ≈ 2000 millimoles

Thus, the chemist added 2000 millimoles of AlCl₃

Answer:

0.7 moles of Ag are produced

Explanation:

Given data:

Mass of silver carbonate = 97.4 g

Moles of silver produced = ?

Solution:

Chemical equation:

2Ag₂CO₃     →     4Ag + 3CO₂

Number of moles of Ag₂CO₃ :

Number of moles = mass/molar mass

Number of moles = 97.4 g/ 275.75 g/mol

Number of moles = 0.35 mol

Now we will compare the moles of Ag and Ag₂CO₃.

              Ag₂CO₃           :         Ag

                    2                :           4

                0.35              :             4/2×0.35 = 0.7

0.7 moles of Ag are produced.

Answer:

dissociation, in chemistry, separation of a substance into atoms or ions. ... For example, hydrogen molecules (H2) dissociate into atoms (H) at very high temperatures; at 5,000°K about 95% of the molecules in a sample of hydrogen are dissociated into atoms.

Explanation:

Answer: True

Explanation:

Answer:

60

Explanation:

The formula of the compound is given as:

              HC₂H₃O₂

To find the formula mass we sum up the atomic masses of the component elements;

  Atomic mass:

         H  = 1

         C  = 12

         O = 16

 HC₂H₃O₂  = 1 + 2(12) + 3(1) + 2(16)

                   = 1 + 24 + 3 + 32

                   = 60

Answer:

D. The model can be observed from the classroom more easily

Explanation:

From the concept of using wire coil to model and the concept of using spring coil to measure, we can come to the conclusion that the correct answer is Option D.