Answer:
[tex]\boxed {\boxed {\sf 0.56 \ L \ CO_2}}[/tex]
Explanation:
We can convert particles to moles in 3 steps:
1. Convert Particles to MolesFirst, we must convert particles to moles. 1 mole of any substance contains the same number of particles: 6.022*10²³ or Avogadro's Number. For this problem, we have particles of carbon dioxide or CO₂. We can make a ratio.
[tex]\frac{6.022 *10^{23} \ particles \ CO_2}{1 \ mol \ CO_2}[/tex]
Since we are converting 1.5*10²² particles to moles, we multiply the ratio by that value.
[tex]1.5 *10^{22} \ particles\ CO_2*\frac{6.022 *10^{23} \ particles \ CO_2}{1 \ mol \ CO_2}[/tex]
Flip the ratio. It remains equivalent, but the units of particles of carbon dioxide can cancel.
[tex]1.5 *10^{22} \ particles\ CO_2*\frac{1 \ mol \ CO_2}{6.022 *10^{23} \ particles \ CO_2}[/tex]
[tex]1.5 *10^{22}*\frac{1 \ mol \ CO_2}{6.022 *10^{23} }[/tex]
[tex]\frac{1.5 *10^{22} }{6.022 *10^{23} }\ mol \ CO_2[/tex]
[tex]0.0249086682165 \ mol \ CO_2[/tex]
2. Convert Moles to LitersThere are 22.4 liters in 1 mole of any gas. Let's set up another ratio.[tex]\frac{22.4 \ L \ CO_2}{1 \ mol \ CO_2}[/tex]
Multiply by the number of moles we calculated.
[tex]0.0249086682165\ mol \ CO_2*\frac{22.4 \ L \ CO_2}{1 \ mol \ CO_2}[/tex]
The units of moles of carbon dioxide cancel.
[tex]0.0249086682165*\frac{22.4 \ L \ CO_2}{1}[/tex]
[tex]0.0249086682165*{22.4 \ L \ CO_2[/tex]
[tex]0.55795416805\ L \ CO_2[/tex]
3. RoundThe original measurement of particles (1.5*10²²) has 2 significant figures (1 and 5). Our answer must have the same number. For the number we calculated, that is the hundredth place.
The 7 in the thousandth place (0.55795416805) tells us to round the 5 in the hundredth place up to a 6.
[tex]0.56 \ L \ CO_2[/tex]
1.5*10²² particles of carbon dioxide is equal to 0.56 liters of carbon dioxide.
How many kilojoules (kJ) in 373 joules (J)?
Answer: There are 0.373 kJ in 373 joules.
Explanation:
According to the standard conversion units 1 kJ is equal to 1000 J. This means that 1 J is equal to 0.001 kJ.
Hence, 373 joules is converted into kilojoules as follows.
[tex]1 J = 0.001 kJ\\373 J = 373 J \times \frac{0.001 J}{1 kJ}\\= 0.373 kJ[/tex]
Thus, we can conclude that there are 0.373 kJ in 373 joules.
Which of the following is most easily oxidized?
A. Ni2+
B. Fe3+
C. H+
D. Fe2+
Answer:
B: Fe3+
Explanation:
Usually in oxidation reactions, the oxidation number of a monatomic ion is the same as the charge on the ion, for example: oxidation number for Na^(+) is +1 , while in S^(2-), oxidation number is -2.
Now, from the activity series of metals in aqueous solution which I attached, we will see that iron (Fe) is easily oxidized than Nickel (Ni2+) and hydrogen (H+).
So we are left with Fe^(2+) and Fe^(3+).
Now, an increase in oxidation number means the more likely to be oxidized.
Thus, Fe^(3+) is the most easily oxidized.
How many liters of Argon gas are present in a 10.5 mole sample?
Answer:
235.2 L ( if the sample is under S.T.P condition )
Explanation:
For any gas at S.T.P (0°c, 1 atm), 1 mole=22.4 L
Thus, for 10.5 mole of Ar, there are 10.5*22.4=235.2 L
what is hard water??
Answer:
Hard water is any water that does not lather easily with soap. pipe water is an example of hard water.
I hope this helps . good luck.
Titan, the largest moon of Saturn, has an atmosphere that is about 94% nitrogen (N2) and 6% methane (CH4). The molecular mass of nitrogen is 4.651e-26kg and the molecular mass of methane is 2.663e-26kg. The acceleration due to gravity at the surface is about 1.35 m/s^2. For this problem, assume that Titan's atmosphere is in thermal equilibrium at 100 K. What fraction of the atmosphere is methane at altitude 2 km
Answer:
9.493 e-01
Explanation:
Given that Titan's temperature at thermal equilibrium = 100 K
Determine the fraction of the atmosphere that is methane
at an altitude of 2 km
applying Ideal gas law
P = Po e^ -Z/k ---- ( 1 )
In this question Z = M₀ g z ( replace -Z in equation 1 with M₀gz )
P = Po e^- M₀gz / RT ------ ( 2 )
where : Mo = 16 * 10^ -3 kg/mol , g = 1.35 m/s^2 , z = 2 * 10^3 m , R = 8.3 J/mol.k , T = 100 k
insert values Back to equation 2
P = Po e^-0.052
P = 0.9493 Po
hence the fraction of the atmosphere that is methane
= P / Po = 9.493 * 10^-1
= 9.493 e-01
A chemist must dilute of aqueous potassium iodide solution until the concentration falls to . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to significant digits.
Answer:
The answer is "[tex]0.157\ L[/tex]"
Explanation:
Please find the complete question in the attached file.
[tex]M_1=13.5\ M\\\\V_1=58.0\ ml\\\\M_2=5.00\ M\\\\[/tex]
Using formula:
[tex]M_1V_1=M_2V_2\\\\V_2 = \frac{(M_1V_1)}{M_2}\\\\[/tex]
[tex]= \frac{(13.5 \times 58.0)}{5.0}\\\\= 156.6 \ ml\\\\[/tex]
[tex]= \frac{156.6}{1000}\ L\\\\ =0.157\ L\\\\[/tex]
Is anyone good at chemistry if so Is it possible could someone help me please
NO LINKS I REPEAT NO LINKS
344.0 / 68.8 = 5 (no.of half life that have elapsed)
Mass remains = (1/2)^n × (original mass)
= (1/2)^5 × 200
= (0.5) ^5 × 200
= 0.03125 × 200
= 6.25 grams
An Arrhenius base increases the concentration of hydrogen ions when dissolved in solution. (3 points)
Answer:
Explanation:
False
Answer:
false
Explanation:
took the test
How many liters of C3H6O are present in a sample weighing 25.6 grams?
Answer:
V = 0.0327 L.
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to calculate the liters of C3H6O by the definition of density. We can tell the density of this substance as that of acetone (0.784 g/mL) and therefore calculate the liters as shown below:
[tex]V=25.6g*\frac{1mL}{0.784g}*\frac{1L}{1000mL}\\\\V=0.0327L[/tex]
Regards!
What is the
empirical formula for a compound that is 36.1% Ca and 63.9% Cl?
Answer:
CaCl
2
Explanation:
As with all these problems, we assume a
100
⋅
g
of compound, and divide through by the ATOMIC masses of each component element:
Moles of calcium
=
36.1
⋅
g
40.08
⋅
g
⋅
mol
−
1
=
0.901
⋅
mol
.
Moles of chlorine
=
63.9
⋅
g
35.45
⋅
g
⋅
mol
−
1
=
1.802 mol
.
We divide each molar quantity through by the smallest molar quantity (that of calcium) to give an empirical formula of
CaCl 2
.
For ionic materials, we do not speak of the molecular formula, and the empirical formula is the formula we quote for reference.
Define Aesthenosphere
A chemist wants to extract copper metal from copper chloride solution. The chemist places 0.25 grams of aluminum foil in a solution of 0.40 grams of copper (II) chloride. A single replacement reaction takes place. What are the likely observations when the reaction stops? Unbalanced equation: CuCl2 + Al → AlCl3 + Cu
Answer: About 0.20 grams of copper (II) is formed, and some aluminum is left in the reaction mixture
Answer:Answer B: About 0.20 grams of copper (II) is formed, and some aluminum is left in the reaction mixture
Explanation:
What is the mass of 6.02 x 1023 atoms of carbon-12?
A)
me
6 grams
B)
6.02 grams
6.02 x 1023
grams
D)
12 grams
Answer: its D 12 grams
Explanation: you just have to find the molar mass of carbon in the periodic table
What is renewable energy?
A. Energy that will not be regenerated in our lifetime.
B. Energy that will never be used up.
C. Energy that take millions of years to form.
D. Energy that is inexpensive but produce harmful waste
products
Answer: The answer might be A or B.
Explanation:
mechanism of the reaction citric acid with sodium bicarbonate?
Explanation:
When citric acid and baking soda react with one another, they change chemi- cally and form sodium ions, citric acid ions, carbon dioxide gas, and water. ... It also makes up the bubbles in carbonated drinks and is a gas we naturally exhale. Carbon dioxide gas is safe in the quantities produced in the activities.
Maintaining constant pressure, the volume of a gas is increased from 12,0 L
to 32.0 L by heating it. If the original temperature was 23.0°C, what is the
new temperature? *
23. 45 K
61.33 K
789.33 K
567.87 K
Answer:
790 K
Explanation:
Step 1: Given data
Initial volume of the gas (V₁): 12.0 LInitial temperature of the gas (T₁): 23.0 °CFinal volume of the gas (V₂): 32.0 LStep 2: Convert 23.0 °C to Kelvin
We will use the following expression.
K = °C + 273.15 = 23.0 + 273.15 = 296.2 K
Step 3: Calculate the final temperature of the gas
Assuming constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.
T₁/V₁ = T₂/V₂
T₂ = T₁ × V₂/V₁
T₂ = 296.2 K × 32.0 L/12.0 L = 790 K
What chemical is used to represent compounds
Answer:
Compounds are represented by chemical formulas. Elements in a compound are represented by chemical symbols, and the ratio of different elements is represented by subscripts.
When fluorine (F) forms chemical compounds with metals, the fluorine atom gains electrons , looses electrons
how much mercury-203 remains after 200 days
Answer:
50%
Explanation:
How many grams of calcium chloride are required to make 20 grams of calcium hydroxide? CaCl2 + 2 NaOH → Ca(OH)2 + 2 NaCl
Answer:
30.0g CaCl2
Explanation:
20.0g Ca(OH)2=0.270mol
(0.270mol)(111.0g/mol)=30.0g CaCl2
How are photosynthesis and cellular respiration related?
A. Photosynthesis releases energy, while cellular respiration stores energy
B. Cellular respiration breaks down glucose, while photosynthesis produces glucose.
C. Cellular respiration is the process animals use to produce glucose, while photosynthesis is the process plants use to produce glucose.
D. Photosynthesis produces water molecules, while cellular respiration splits water molecules apart.
Answer:
B part is the correct answer
A nurse practitioner prepares 470. mL of an IV of normal saline solution to be delivered at a rate of 85 mL/h. What is the infusion time, in hours, to deliver 470. mL?
Answer: Infusion time is 5.5 h
Explanation: Time is 470 ml / 85 ml/h = 5.5 h
Se hace reaccionar 4,00 g de aluminio y 42,00 g de bromo, según la reacción: Al(s)+Br2(l)⟶AlBr3(s) Calcular las moles de AlBr3(s) producido. PA: Al=27; Br=80
Answer:
0.145 moles de AlBr3.
Explanation:
¡Hola!
En este caso, al considerar la reacción química dada:
Al(s)+Br2(l)⟶AlBr3(s)
Es claro que primero debemos balancearla como se muestra a continuación:
2Al(s)+3Br2(l)⟶2AlBr3(s)
Así, calculamos las moles del producto AlBr3 por medio de las masas de ambos reactivos, con el fin de decidir el resultado correcto:
[tex]n_{AlBr_3}^{por\ Al}=4.00gAl*\frac{1molAl}{27gAl} *\frac{2molAlBr_3}{2molAl}=0.145mol AlBr_3\\\\n_{AlBr_3}^{por\ Br_2}=42.00gr*\frac{1molr}{160g Br_2} *\frac{2molAlBr_3}{3molBr_2}=0.175mol AlBr_3[/tex]
Así, inferimos que el valor correcto es 0.145 moles de AlBr3, dado que viene del reactivo límite que es el aluminio.
¡Saludos!
Which process produces the energy that is used by solar panels?
O A. Nuclear fusion
O B. Combustion
O C. Chemical decay
D. Nuclear decay
Answer:
B
Explanation:
Answer:
A
Explanation: got it right
How much is 1 mole of something?
Answer: D.
Explanation:
6.02 * 10^-23
What is the [OH-] of a solution with a pH of 3.89?
Which one is it?
7.76 x 10^-11
1.29 x 10^-4
2.11 x 10^-6
4.51 x 10^-10
Answer:
the answer is 211106 is better than anything else about u and then let's go play with kids like that first time in the class ohh ok
Why is it necessary to keep the total number of drops in the test tubes
consistent?
Answer:
I don't know if this is right but..
Explanation:
It is important to keep the volume of the reactant constant because it ensures that the temperature change was the result of the reactants consumed
Why it is necessary to keep the to drops in the test tubes consistent is:
To be able to achieve your desire results, it is imperative that you follow the procedure and use the drops specified because any other drop may shift the equilibrium to the right and this will increase the rate of reaction leading to more collisions of that reactant in a specific time period and therefore alter (slow or increase) the chemical reaction.In a chemical reaction, the reactants, are undergoing chemical reaction which therefore brings about a products. The reaction rate shows how quickly or slowly the reaction takes place.Conclusively, Why it is necessary to keep the to drops in the test tubes consistent is:
To be able to achieve your desire results, it is imperative that you follow the procedure and use the drop specified because any other drop may shift the equilibrium to the right and this will increase the rate of reaction leading to more collisions of that reactant in a specific time period.Learn more from
https://brainly.com/question/14197404
The minimum combined kinetic energy reactant particles must possess in order for their collision to result in a reaction is called the
Answer: Activation energy
Explanation:
In a chemical reaction, the reactants contains particles which must collide in order for a reaction to occur. The rate of reaction depends on the frequency of effective collision between the reacting particles. Effective collision are those that result in reactions, which when they occur the colliding particles become activated with increased kinetic energy.
This energy must exceed a particular energy barrier for a particular reaction if the reaction must take place. This energy barrier that must be overcome before a reaction takes place is known as the ACTIVATION ENERGY.
To explain further, when two particles or molecules A and B come in contact with each other, for a reaction to take place, they must collide with a sufficient force to break the bond that exists between them. The minimum combined kinetic energy these reactant particles must possess in order for their collision to result in a reaction is called the activation energy.
Adding more baking soda and vinegar to the bag in the Air Bag Lab resulted in faster production of gaseous products True False
Answer:
True
Explanation:
The more of each substanse that you add to the bag will cause it to produce faster and more gas.
To increase the temperature of 100.0 g
of ice from -50.0? to -10.0?, how
much energy is required?
We are given:
Mass of ice = 100 grams
Initial temperature = -50°C
Final Temperature = -10°C
We know that the specific heat of ice is 2.09 joules / (gram * °c)
Heat Absorbed:
We know that:
ΔQ = mcΔT [where ΔQ is the heat absorbed]
ΔQ = (100 grams)(2.09)(-10 - (-50))
ΔQ = (100)(2.09)(40)
ΔQ = 8360 Joules