Answer: CO2(g)+H2O(I) > H2CO3(Aq)
Explanation:
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A mixture of krypton and nitrogen gases, at a total pressure of 711 mm Hg, contains 11.7 grams of krypton and 4.10 grams of nitrogen. What is the partial pressure of each gas in the mixture
Answer:
A. Partial pressure of krypton, Kr is 346.97 mmHg
B. Partial pressure of nitrogen, N2 is 364.03 mmHg.
Explanation:
Step 1:
Data obtained from the question. This include the following:
Total pressure (Pt) = 711 mmHg
Mass of Kr = 11.7 g
Mass of N2 = 4.10 g
Partial pressure of Kr =..?
Partial pressure of N2 =...?
Step 2:
Determination of the number of mole of krypton, Kr and nitrogen, N2. This is illustrated below:
Molar mass of Kr = 84g/mol
Mass of Kr = 11.7g
Mole of Kr =?
Mole = mass /Molar mass
Mole of Kr = 11.7/84 = 0.139 mole
Molar mass of N2 = 2x14 = 28g/mol
Mass of N2 = 4.10g
Mole of N2 =?
Mole = mass /Molar mass
Mole of N2 = 4.1/28 = 0.146 mole
Step 3:
Determination of the mole fraction for each gas. This is illustrated below:
Mole of Kr = 0.139 mole
Mole of N2 = 0.146 mole
Total mole = 0.139 + 0.146 = 0.285 mole
Mole fraction of Kr = mol of Kr/total mol
Mole fraction of Kr = 0.139/0.285
Mole fraction of Kr = 0.488
Mole fraction of N2 = mol of N2/total mol
Mole fraction of N2 = 0.146/0.285
Mole fraction of N2 = 0.512
A. Determination of the partial pressure of krypton, Kr.
This is illustrated below:
Total pressure (Pt) = 711 mmHg
Mole fraction of Kr = 0.488
Partial pressure of Kr =..?
Partial pressure = mole fraction x total pressure
Partial pressure of Kr = 0.488 x 711
Partial pressure of Kr = 346.97 mmHg
B. Determination of the partial pressure of nitrogen, N2
This is illustrated below:
Total pressure (Pt) = 711 mmHg
Mole fraction of N2 = 0.512
Partial pressure of N2 =?
Partial pressure = mole fraction x total pressure
Partial pressure of N2 = 0.512 x 711
Partial pressure of N2 = 364.03 mmHg
Average Molarity for HCl is .391
Average Molarity for NaOH is .0962
Volume for HCl is:
Trial 1 Your Answer: 14mL
Trial 2 Your Answer: 14mL
Trial 3 Your Answer: 14mL
Volume for NaOH is:
Trial 1: 34.26mL
Trial 2: 33.48mL
Trial 3: 33.84mL
Entry # mass tablet(g) mass antacid(g) Vol HCl(mL) Vol NaOH(mL)
#1: 1.515 0.9010 14.00 34.26
#2: 1.452 0.8370 14.00 33.48
#3: 1.443 0.8280 14.00 33.84
I need help finding the mmoles HCl/mg please.
Answer:
#1: 0.00144 mmolHCl/mg Sample
#2: 0.00155 mmolHCl/mg Sample
#3: 0.00153 mmolHCl/mg Sample
Explanation:
A antiacid (weak base) will react with the HCl thus:
Antiacid + HCl → Water + Salt.
In the titration of antiacid, the strong acid (HCl) is added in excess, and you're titrating with NaOH moles of HCl that doesn't react.
Moles that react are the difference between mmoles of HCl - mmoles NaOH added (mmoles are Molarity×mL added). Thus:
Trial 1: 0.391M×14.00mL - 0.0962M×34.26mL = 2.178 mmoles HCl
Trial 2: 0.391M×14.00mL - 0.0962M×33.48mL = 2.253 mmoles HCl
Trial 3: 0.391M×14.00mL - 0.0962M×33.84mL = 2.219 mmoles HCl
The mass of tablet in mg in the 3 experiments is 1515mg, 1452mg and 1443mg.
Thus, mmoles HCl /mg OF SAMPLE for each trial is:
#1: 2.178mmol / 1515mg
#2: 2.253mmol / 1452mg
#3: 2.219mmol / 1443mg
#1: 0.00144 mmolHCl/mg Sample#2: 0.00155 mmolHCl/mg Sample#3: 0.00153 mmolHCl/mg SampleAccording to valence bond theory, which orbitals overlap in the formation of the bond in HCl?
a) 1s on H and 3p on Cl
b) 1s on H and 4s on Cl
c) 1s on H and 2p on Cl
d) 2s on H and 3p on Cl
e) 2s on H and 2p on Cl
solution solution solution
Answer:
Oxygen present in food items makes then rancid due to the presence of oils and fats. If the food is flushed with nitrogen, it prevents it from being oxidised (the nitrogen acts as an antioxidant).
Hope it helps ! :)
Determine the [OH⁻] concentration in a 0.344 M Ca(OH)₂ solution.
Answer:
[tex]0.688M[/tex]
Explanation:
Hello,
In this case, it is widely acknowledged that strong bases usually correspond to those formed with metals in groups IA and IIA which have relatively high activity and reactivity, therefore, when they are dissolved in water the following dissociation reaction occurs (for calcium hydroxide):
[tex]Ca(OH)_2\rightarrow Ca^{2+}+2OH^-[/tex]
In such a way, for the same volume, we can compute the concentration of hydroxyl ions by simple stoichiometry (1:2 molar ratio):
[tex]0.344\frac{molCa(OH)_2}{L}*\frac{2molOH^-}{1molCa(OH)_2} \\\\0.688\frac{mol OH^-}{L}[/tex]
Or simply:
[tex]0.688M[/tex]
Regards.
Using the volumes of EDTA solution you just entered and the corresponding dry unknown sample masses entered earlier, calculate the percent mass of calcium carbonate in the unknown sample mixture.
Enter the calculated percent mass of calcium carbonate in the dry unknown sample for each of the 3 acceptable trials.
Be sure to enter your mass percentages to the correct number of significant digits and in the corresponding order that you entered your masses of your dry unknown samples and volumes of your EDTA previously. The dry unknown sample mass you entered for entry #1 below should correspond to the percent mass of calcium carbonate you enter for entry #1 here.
Trial #: Mass (Grams):
#1: 0.015
#2: 0.015
#3: 0.015
Volume (mL)
#1: 16.4
#2: 15.00
#3: 18.70
Molarity of EDTA Solution: 0.0675
Answer:
#1
Explanation:
molarity of EDTA solution 0.0675
no1
By what mechanism does cyclohexanol react when treated in sulfuric acid and what compound results?A) E 1; methoxycyclohexane B) E2: methoxycyclohexane C) SN 1; methoxycycloheXafle D) E2; cyclohexene E) E 1: cyclohexene
Answer:
E 1: cyclohexene
Explanation:
This reaction is an example of the dehydration of cyclic alcohols. The reaction proceeds in the following steps;
1) The first step of the process is the protonation of the cyclohexanol by the acid. This now yields H2O^+ attached to the cyclohexane ring.
2) the water molecule, which a good leaving group now leaves yielding a carbocation. This now leaves a cyclohexane carbocation which is highly reactive.
3) A water molecule now abstracts a proton from the carbon adjacent to the carbocation leading to the formation of cyclohexene and the regeneration of the acid catalyst. This is an E1 mechanism because it proceeds via a carbocation intermediate and not a concerted transition state, hence the answer.
How many water molecules are in a block of ice containing 0.500 mol of water (H2O)?
Answer:
3.01 × 10²³ molecules
Explanation:
Step 1: Given data
Moles of water (n): 0.500 mol
Step 2: Calculate the molecules of water present in 0.500 moles of water
In order to perform this calculation, we will use the Avogadro's number: in 1 mole of water there are 6.02 × 10²³ molecules of water.
0.500 mol × (6.02 × 10²³ molecules/1 mol) = 3.01 × 10²³ molecules
For a given sample of C3H8(g), the enthalpy change during the reaction is -784kJ. How many grams of CO2 are produced? Group of answer choices g
Answer:
[tex]m_{CO_2}=46.6gCO_2[/tex]
Explanation:
Hello,
In this case, considering the combustion of propane:
[tex]C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)\ \ \ \Delta _CH=-2220.0 kJ/mol[/tex]
We can compute the burnt moles of propane as shown below:
[tex]n=\frac{-784kJ}{-2220.0 kJ/mol} =0.353molC_3H_8[/tex]
Then, by noticing propane and carbon dioxide are in a 1:3 molar ratio, we can compute the grams carbon dioxide by using the shown below stoichiometric procedure:
[tex]m_{CO_2}=0.353molC_3H_8*\frac{3molCO_2}{1molC_3H_8} *\frac{44gCO_2}{1molCO_2} \\\\m_{CO_2}=46.6gCO_2[/tex]
Best regards.
Grams of cl in 38g of cf3cl
Answer:
114 grams
Explanation:
3chlorines per compound*38grams=114
If the NaOH is added to 35.0 mL of 0.167 M Cu(NO3)2 and the precipitate isolated by filtration, what is the theoretical yield of the reaction?
Answer:
The correct answer is - 0.570 grams
Explanation:
The balanced chemical reaction is given by
Cu(NO3)2(aq) + 2NaOH(aq) --------> Cu(OH)2(s) + 2NaNO3(aq)
1.0 mole 2.0 mole 1.0 mole 2.0 mole
number of mol of Cu(OH)2,
n = Molarity * Volume
= [tex]35.0*0.167 = 5.845[/tex] millimoles
As clear in the equation, 1 mole of Cu(NO3)2 gives 1 mole of Cu(OH)2 , So, 5.845 millimoles of Cu(NO3)2 will produce 5.845 millimoles of Cu(OH)2
Mass of Cu(OH)2 = number of mol * molar mass
= [tex]97.5*5.845*10^-3[/tex]
= 0.570 grams
Thus, the correct answer is - 0.570 grams
Write a balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product.
Answer:
2 CH₃OH + 3 O₂ ⇒ 2 CO₂ + 4 H₂O
Explanation:
Methanol is CH₃OH. Oxygen is O₂. A combustion produces CO₂ and H₂O. Create an equation using this information and balance.
CH₃OH + O₂ ⇒ CO₂ + H₂O
2 CH₃OH + 3 O₂ ⇒ 2 CO₂ + 4 H₂O
The balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product is
CH₃OH(l) + O₂(g) → CO₂(g) + H₂O(g)
From the question,
We are to write a balanced equation for the combustion of liquid methanol in air.
The combustion of liquid methanol in air is the reaction between methanol (CH₃OH) and oxygen (O₂). The reaction yields carbon(IV) oxide and water.
Now, for the balanced equation for the combustion of liquid methanol in air
The balanced chemical equation is
CH₃OH(l) + O₂(g) → CO₂(g) + H₂O(g)
Hence, the balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product is CH₃OH(l) + O₂(g) → CO₂(g) + H₂O(g)
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Which products are formed when aluminum is added to a silver chlorine solution?
Answer:
Alcl3 and Cl2
Explanation:
the product above will be formed
Answer:
silver (Ag) and aluminum chloride (AlCl₃)
Explanation:
The reaction between aluminum and silver chloride is a single replacement reaction. A single replacement reaction is when one element switches places with another.
Al + 3AgCl ➔︎ 3Ag + AlCl₃
In the reaction, the cations (positively charged ions) switch places. Aluminum (Al) switches places with Silver (Ag). So, the products of the reaction are silver and aluminum chloride.
Hope this helps.
What is a heterogeneous mixture?
Answer:
The type of mixture whose components are seen through our naked eyes is known as heterogeneous mixture. it is a mixture of small constituent parts of substances.
for eg, mixture of sand and sugar.
hope it helps..
The substance used by homeowners and municipal workers to melt ice on sidewalks and roadways is usually calcium chloride rather than sodium chloride. Discuss two possible rea-sons for this preference.
Answer:
1. It dissolves much more ice faster than sodium chloride
2. Calcium chloride is more effective in melting ice at lower temperatures.
Explanation:
Salts are used to melt ice on roadways and sidewalks because they help to lower the freezing point of water.
Sodium chloride and calcium chloride are both salts used for this purpose but calcium chloride is usually preferred for the following two reasons:
1. It dissolves much more ice faster than sodium chloride: Calcium chloride dissolves much more ice faster than sodium chloride because when it dissociates, it produces three ions instead of the two produced when sodium chloride. Therefore, the heat of hydration of its ions is greater than that of sodium chloride.
2. Calcium chloride is more effective in melting ice at lower temperatures. It lowers the freezing point of water more than sodium chloride. Calcium chloride is able to lower the freezing point of water to about -52°C while sodium chloride only lowers it to about -6°C.
The Ka1 value for oxalic acid is 5.9 x10-2 , and the Ka2 value is 4.6 x 10-5 . What are the values of Kb1 and Kb2 of the oxalate ion
Answer:
2.17x10⁻¹⁰ = Kb1
1.69x10⁻¹³ = Kb2
Explanation:
Oxalic acid, C₂O₄H₂, has two intercambiable protons, its equilibriums are:
C₂O₄H₂ ⇄ C₂O₄H⁻ + H⁺ Ka1 = 5.9x10⁻²
C₂O₄H⁻ ⇄ C₂O₄²⁻ + H⁺ Ka2 = 4.6x10⁻⁵
Oxalate ion, C₂O₄²⁻, has as equilibriums:
C₂O₄²⁻ + H₂O ⇄ C₂O₄H⁻ + OH⁻ Kb1
C₂O₄H⁻ + H₂O ⇄ C₂O₄H₂ + OH⁻ Kb2
Also, you can know: KaₓKb = Kw
Where Kw is 1x10⁻¹⁴
Thus:
Kw = Kb2ₓKa1
1x10⁻¹⁴ =Kb2ₓ4.6x10⁻⁵
2.17x10⁻¹⁰ = Kb1And:
Kw = Kb1ₓKa2
1x10⁻¹⁴ =Kb1ₓ5.9x10⁻²
1.69x10⁻¹³ = Kb1
That is because the inverse reaction of, for example, Ka1:
C₂O₄H⁻ + H⁺ ⇄ C₂O₄H₂ K = 1 / Ka1
+ H₂O ⇄ H⁺ + OH⁻ K = Kw = 1x10⁻¹⁴
=
C₂O₄H⁻ + H₂O ⇄ C₂O₄H₂ + OH⁻ Kb2 = Kw × 1/Ka1
Which of the possible compounds has a mass of 163 grams when
6.13 x 1024 molecules of the compound is put on a scale?
Answer:
CH4
Explanation:
In solving this problem, we must remember that one mole of a compound contains Avogadro's number of elementary entities. These elementary entities include atoms, molecules, ions etc. Recall that one mole of a substance is the amount of substance that contains the same number of elementary entities as 12g of carbon-12. The Avogadro's number is 6.02 × 10^23.
Hence we can now say;
If 163 g of the compound contains 6.13 ×10^24 molecules
x g will contain 6.02 × 10^23 molecules
x= 163 × 6.02 × 10^23 / 6.13 × 10^24
x= 981.26 × 10^23/ 6.13 ×10^24
x= 160.1 × 10^-1 g
x= 16.01 g
x= 16 g(approximately)
16 g is the molecular mass of methane hence x must be methane (CH4)
A 2.0 g sample of hydrocarbon was burned in the calorimeter. The temperature rose from 29°c to 32°c and heat and combustion is 11. Kj/g. Thr heat capacity of the calorimeter is
Answer:
THE HEAT CAPACITY OF THE CALORIMETER IS 3666.67 J/C
Explanation:
Mass = 2 g
Temperature difference = 32 C - 29 C = 3 C
Heat of combustion = 11 kJ/g
Heat capacity of the calorimeter = unknown
It is important to note that the heat of combustion of the reaction is the heat absorbed by the calorimeter in raising the mixture by 3 C
So therefore,
Heat = heat capacity * temperature difference
Heat capacity = Heat / temperature difference
Heat capacoty = 11 000 J / 3 C
Heat capacity = 3666.67 J/ C
Which aqueous solution will have the highest boiling point temperature? A. 0.100 molal NiBr2(aq) B. 0.250 molal CH3OH(aq) C. 0.100 molal MgSO4(aq) D. 0.150 molal Na2SO4(aq) E. 0.150 molal NH4NO3(aq)
Answer: 0.150 m [tex]Na_2SO_4(aq)[/tex] will have highest boiling point.
Explanation:
Formula used for Elevation in boiling point :
[tex]\Delta T_b=i\times k_b\times m[/tex]
where
[tex]\Delta T_b=T_b-T^o_b[/tex]= elevation in boiling point
[tex[k_b[/tex] = boiling point constant
m = molality
i = Van't Hoff factor
A) 0.100 m [tex]NiBr_2[/tex]
i = 3 as [tex]NiBr_2\rightarrrow Ni^{2+}+2Br^-[/tex]
concentration will be [tex]3\times 0.100=0.300[/tex]
B) 0.250 m [tex]CH_3OH[/tex]
i = 1 as [tex]CH_3OH[/tex] is a non electrolyte
concentration will be [tex]1\times 0.250=0.250[/tex]
C) 0.100 molal [tex]MgSO_4(aq)[/tex]
i = 2 as [tex]MgSO_4\rightarrrow Mg^{2+}+SO_4^{2-}[/tex]
concentration will be [tex]2\times 0.100=0.200[/tex]
D. 0.150 molal [tex]Na_2SO_4(aq)[/tex]
i = 3 as [tex]Na_2SO_4\rightarrrow 2Na^{+}+SO_4^{2-}[/tex]
concentration will be [tex]3\times 0.150=0.450[/tex]
E. 0.150 molal [tex]NH_4NO_3(aq)[/tex]
i = 2 as [tex]NH_4NO_3\rightarrrow NH_4^{+}+NO_3^{-}[/tex]
concentration will be [tex]2\times 0.150=0.300[/tex]
The solution having the highest concentration of ions will have the highest boiling point and thus 0.150 m [tex]Na_2SO_4(aq)[/tex] will have highest boiling point.
The aqueous solution that would have the highest temperature at boiling point would be:
D). 0.150 molal Na2SO4(aq)
What is a boiling point?The boiling point is described as the temperature at which the solution starts boiling or the vapor pressure becomes equivalent to the provided external/outer pressure.
To determine the elevation in boiling point, we will use:
Δ[tex]T_{b}[/tex] [tex]= i[/tex] × [tex]k_{b}[/tex] × [tex]m[/tex]
with
[tex]T_{b}[/tex] [tex]= T_{b} - T^{0}_{b}[/tex]
[tex]k_b[/tex] [tex]=[/tex] constant of boiling point
Using this formula,
0.150 molal Na2SO4(aq)
Given,
[tex]i = 3[/tex]
[tex]Na2So4[/tex] will have
[tex]2Na^{+}[/tex] [tex]+[/tex] [tex]SO^{2-}_{4}[/tex]
So,
Concentration [tex]= 3[/tex] × [tex]0.15[/tex][tex]0[/tex]
[tex]= 0.45[/tex][tex]0[/tex]
∵ 0.150 molal [tex]Na2SO4[/tex]Na2SO4(aq) has the maximum concentration.
Thus, option D is the correct answer.
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For the reaction 2 A - Products, the concentration of A is monitored over time. A graph of [A] versus time was found to be linear, with a negative slope. Select the true statement regarding this reaction.
A) The reaction is first order with respect to A.
B) The reaction is second order with respect to A.
C) The rate constant has a negative value.
D) In 2 The reaction has a half-life equal to k.
E) None of these statements is true.
Answer:
none of these statements is true
according to the question E) None of these statements is true.
What is a concentration in chemistry?The concentration of a chemical substance expresses the amount of a substance present in a mixture. There are many different ways to express concentration. Chemists use the term solute to describe the substance of interest and the term solvent to describe the material in which the solute is dissolved
What is concentration in chemistry units?
Quantitative units of concentration include molarity, molality, mass percentage, parts per thousand, parts per million, and parts per billion.
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Gallium chloride is formed by the reaction of 2.25 L of a 1.50 M solution of HCl according to the following equation: 2Ga 6HCl --> 2GaCl3 3H2 Determine the mass of gallium chloride, in grams, produced. Group of answer choices
Answer:
198.56g of GaCl3
Explanation:
We'll begin by calculating the number of mole HCl in 2.25 L of a 1.50 M solution of HCl. This is illustrated below:
Molarity of HCl = 1.50 M
Volume = 2.25 L
Mole of HCl =..?
Molarity = mole /Volume
1.5 = mole /2.25
Cross multiply
Mole = 1.5 x 2.25
Mole of HCl = 3.375 mole
Next, we shall determine the number of mole Gallium chloride, GaCl3 produced from the reaction. This is shown below:
2Ga + 6HCl —> 2GaCl3 + 3H2
From the balanced equation above,
6 moles of HCl reacted to produce 2 moles of GaCl3.
Therefore, 3.375 mole of HCl will react to produce = (3.375 x 2)/6 = 1.125 mole of GaCl3.
Therefore, 1.125 moles of GaCl3 were produced from the reaction.
Next, we shall convert 1.125 mole of GaCl3 to grams. This is illustrated below:
Molar mass of GaCl3 = 70 + (35.5x3) = 176.5g/mol
Mole of GaCl3 = 1.125 mole
Mass of GaCl3 =..?
Mole = mass /Molar mass
1.125 = mass of GaCl3 /176.5
Cross multiply
Mass of GaCl3 = 1.125 x 176.5
Mass of GaCl3 = 198.56g
Therefore, 198.56g of GaCl3 were produced from the reaction.
PLEASE ANSWER AS SOON AS POSSIBLE REALLY WOULD APPRECIATE IT
Answer:
The answer is option D.
Hope this helps you
Which of the following is an alkali metal?
A. Lithium (LI)
B. Boron (B)
c. Calcium (Ca)
D. Krypton (Kr)
Answer:
lithium is akali metal
Answer:
lithium is an alkali metal as it lies in group 1st in modern perodic table.
Calculate the work (kJ) done during a reaction in which the internal volume expands from 28 L to 51 L against an outside pressure of 4.9 atm.
Answer:
W= -11KJ
Explanation:
Given:
volume expands from 28 L to 51 L
pressure =4.9 atm.
We will need to Convert the pressure to Pascal SI
But 1 atm = 101,325 Pa.
Then,
Pressure= (4.9*101323)/1atm = 5*10^5 pa
Then we need to Convert the volumes to cubic meters
But we know that1 m³ = 1,000 L.
V1= 28L * 1m^3/1000L = 0.028m^3
V2=51L × 1m^3 /1000L =0.051m^3
The work done during the expansion of a gas can be calculated as
W= -P(V2-V1)
W= - 5*10^5(0.051m^3 - 0.028m^3)
W= -1.1× 10^4J
Then we can Convert the work to kiloJoule
But1 kJ = 1,000 J.
W= -1.1× 10^4J× 1kj/1000J
= -11KJ
A 32.3-gram sample of gas is found to have a volume of 1.9 liters at 301 K and 1.21 atm. What is the molar mass of this gas? Show all of the work used to solve this problem.
Answer:
351.1g/mol
Explanation:
you can find the answer using The ideal gas equation
n= PV/RT
n=(1.21*1.9/0.082*301)mol
n=0.092 mol
molar mass=Mass/mole
m=32.3g/0.092mol
m=351.1g/mol
What is the mass of 7.68 x 1024 molecules of phosphorus trichloride?
Answer:
THE MASS OF 7.68 *10^24 MOLECULES OF PHOSPHORUS TRICHLORIDE IS 1746.25 g.
Explanation:
Molar mass of PCl3 = ( 31 + 35.5 *3) = 137.5 g/mol
At 7.68 * 10^24 molecules, how many number of mole is present?
6.03 * 10^23 molecules = 1 mole
7.68*10^24 molecules = x mole
x mole = 7.68 *10^24 molecules/ 6.03 *10^23
x mole = 1.27 *10 moles
x mole = 12.7 moles
Using mole = mass / molar mass
mass = mole * molar mass
mass = 12.7 moles * 137.5 g/mol
mass = 1746.25 g
Hence, the mass of 7.68 *10^24 molecules is 1746.25 g
How many grams of CO are produced when 41.0 g of C reacts?
Answer:
95.7 g CO to the nearest tenth.
Explanation:
2C + O2 ---> 2CO
Using relative atomic masses:
24 g C produces 2*12 + 2*16 g CO.
So 41 g produces ( (2*12 + 2*16) * 41 ) / 24
= 95.7 g CO,
g A microwave oven heats by radiating food with microwave radiation, which is absorbed by the food and converted to heat. If the radiation wavelength is 12.5 cm, how many photons of this radiation would be required to heat a container with 0.250 L of water from a temperature of 20.0oC to a temperature of 99oC
Answer:
The total photons required = 5.19 × 10²⁸ photons
Explanation:
Given that:
the radiation wavelength λ= 12.5 cm = 0.125 m
Volume of the container = 0.250 L = 250 mL
The density of water = 1 g/mL
Density = mass /volume
Mass = Volume × Density
Thus; the mass of the water = 250 mL × 1 g/mL
the mass of the water = 250 g
the specific heat of water s = 4.18 J/g° C
the initial temperature [tex]T_1[/tex] = 20.0° C
the final temperature [tex]T_2[/tex] = 99° C
Change in temperature [tex]\Delta T[/tex] = (99-20)° C = 79 ° C
The heat q absorbed during the process = ms [tex]\Delta T[/tex]
The heat q absorbed during the process = 250 g × 4.18 J/g° C × 79° C
The heat q absorbed during the process = 82555 J
The energy of a photon can be represented by the equation :
= hc/λ
where;
h = planck's constant = [tex]6.626 \times 10^{-34} \ J.s[/tex]
c = velocity of light = [tex]3.0 \times 10^8 \ m/s[/tex]
= [tex]\dfrac{6.626 \times 10^{-34} \times 3.0 \times 10^8}{0.125}[/tex]
= [tex]1.59024 \times 10^{-24}[/tex] J
The total photons required = Total heat energy/ Energy of a photon
The total photons required = [tex]\dfrac{82555 J}{1.59024 \times 10^{-24}J}[/tex]
The total photons required = 5.19 × 10²⁸ photons
Why does a new period start on the periodic table, instead of the row continuing? A. A new period starts when a new energy shell starts. B. A new period starts when a new neutron cycle starts. C. None of these D. It is based on how many protons it has.
Answer:
B
Explanation:
All the elements in a period have valence electrons in the same shell. The number of valence electrons increases from left to right in the period. When the shell is full, a new row is started and the process repeats.
A new period starts when a new neutron cycle starts. Hence, option B is correct.
What is the period in the periodic table?A period in the periodic table is a row of chemical elements. All elements in a row have the same number of electron shells.
All the elements in a period have valence electrons in the same shell.
The number of valence electrons increases from left to right in the period.
When the shell is full, a new row is started and the process repeats.
Hence, option B is correct.
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Which one of the following would have the largest dispersion forces?
A) CH3CH2SH
B) CH3NH2
C) CH4
D) CH3CH3
Answer:
A) CH3CH2SH
Explanation:
Dispersion forces are weak attractions found between non-polar and polar molecules. The attractions here can be attributed to the fact that a non-polar molecule sometimes become polar because the constant motion of its electrons may lead to an uneven charge distribution at an instant. If this happens, the molecule has a temporary dipole. This dipole can induce the neighbouring molecules to be distorted and form dipoles as well. The attractions between these dipoles constitute the Dispersion Forces.
Therefore; the greater the molar mass of a compound or molecule, the higher the Dispersion Force. This implies that the compound or molecule with the highest molar mass have the largest dispersion forces.
Now; for option (A)
CH3CH2SH
The molar mass is :
= (12 + (1 × 3 ) +12 + (1 ×2) + 32+1)
= (12 + 3+ 12 + 2 + 32 + 1)
= 62 g/mol
For option (B)
CH3NH2
The molar mass is:
= (12 + (1 × 3 ) +14 + (1 × 2)
= (12 + 3 + 14 + 2)
= 31 g/mol
For option (C)
CH4
The molar mass is :
= 12 + (1 × 4)
= 12 + 4
= 16 g/mol
For option (D)
CH3CH3
The molar mass is :
= 12 + ( 1 × 3 ) + 12 + ( 1 × 3)
= 12 + 3 + 12 + 3
= 30 g/mol
Thus ; option (A) has the highest molar mass, as such the largest dispersion force is A) CH3CH2SH