I need guidance on this question
Answer:
(C) NO2 has covalent bonds.
Which of the following is true for a gas under conditions of very high pressure? (5
points)
1) PV > nRT, because the real volume of the gas would be more than the ideal
volume.
2) PV = nRT, because intermolecular forces are considerable at very high
pressures.
3) PV = nRT, because all gases behave as ideal gases at very high pressures.
04) PV = nRT, because the volume of the gas would become negligible.
Answer:
1) PV > nRT, because the real volume of the gas would be more than the ideal
volume.
Explanation:
According to the ideal gas equation; PV = nRT. Let us recall that this equation only holds under ideal conditions.
Gases exhibit ideal behavior under high temperature and low pressure. At higher pressure, the real volume of the gas is larger than the ideal volume of the gas.
Thus, at high pressure, PV > nRT, because the real volume of the gas would be more than the ideal volume.
Answer:
1) PV > nRT, because the real volume of the gas would be more than the ideal volume.
Explanation:
just took the test :)
At 27.0°C, the volume of a gas is 630 L. At the same pressure, its volume is 92,0 mL at a temperature of
Answer:
–272.96 °C
Explanation:
From the question given above, the following data were obtained:
Initial temperature (T₁) = 27.0 °C
Initial volume (V₁) = 630 L.
Final volume (V₂) = 92.0 mL
Final temperature (T₂) =?
Next, we shall convert 27.0 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Initial temperature (T₁) = 27.0 °C
Initial temperature (T₁) = 27.0 °C + 273
Initial temperature (T₁) = 300 K
Next, we shall convert 92.0 mL to L. This can be obtained as follow:
1000 mL = 1 L
Therefore,
92 mL = 92 mL × 1 L / 1000 mL
92 mL = 0.092 L
Next, we shall determine the final temperature.
Initial temperature (T₁) = 300 K
Initial volume (V₁) = 630 L.
Final volume (V₂) = 0.092 L
Final temperature (T₂) =?
V₁ / T₁ = V₂ / T₂
630 / 300 = 0.092 / T₂
2.1 = 0.092 / T₂
Cross multiply
2.1 × T₂ = 0.092
Divide both side by 2.1
T₂ = 0.092 / 2.1
T₂ = 0.04 K
Finally, we shall convert 0.04 K to celsius temperature. This can be obtained as follow:
T(°C) = T(K) – 273
Final temperature (T₂) = 0.04 K
Final temperature (T₂) = 0.04 – 273
Final temperature (T₂) = –272.96 °C
4. The device shown is a
that's used to measure the heat transferred by a reaction under constant volume.
A. bomb calorimeter
B. reaction vessel
C. thermometer
D. coffee-cup calorimeter
Answer:
The device shown is a calorimeter that used to measure the heat transfer by a reaction under constant volume.
Explanation:
what do adamantium,vibranium and unobtainum have in common
Answer:
they're all fake
Explanation:
How much heat must be absorbed by 375 grams of water to raise its temperature by 25 degrees Celsius? Specific heat for water= 4.184 J/g/C or K
Answer:
[tex]3.9*10^4 J[/tex]
Explanation:
See image for explanation!Answer:
[tex]\boxed {\boxed {\sf 39, 225 \ Joules}}}[/tex]
Explanation:
Since we are given the mass, temperature, and specific heat, we should use the following formula to calculate heat energy.
[tex]q=mc \Delta T[/tex]
We have 375 grams of water, the specific heat of water is 4.184 J/g ° C, and the temperature is raised 25 degrees Celsisus. Therefore:
m= 375 g c= 4.184 J/g °C ΔT= 25°CSubstitute the values into the formula.
[tex]q= (375 \ g)(4.184 \ J/g \textdegree C)(25 \textdegree C)[/tex]
Multiply the first two values together. The units of grams will cancel.
[tex]q=1569 \ J/ \textdegree C(25 \textdegree C)[/tex]
Multiply again. This time, the degrees Celsius cancel, so we are left with only the units of Joules.
[tex]q= 39225 \ J[/tex]
39,255 Joules of heat must be absorbed by the water.
Ice melts after adding heat. The free energy is ————— !
A. Exothermic
B. Not temperature dependent
C. Temperature dependent
D. Depended on how it is heated
E. React with active metals to form h2 gas
F. Endothermic
HCN
H:C:N:
3.
Is this Lewis Structure correct?
Answer:
No, your missing some bonds
Which of the following substances can be dissolved in pure water to give a basic solution?
Hydrogen chloride
Sodium bromide
Sodium hydroxide
Sodium chloride
I think it's sodium hydroxide
Explanation:
sodium hydroxide is a base
How many moles are in 3.72 x 10^27 atoms of iron?
Answer: There are [tex]0.617 \times 10^{4}[/tex] moles present in [tex]3.72 \times 10^{27}[/tex] atoms of iron.
Explanation:
According to the mole concept, there are [tex]6.022 \times 10^{23}[/tex] atoms present in one mole of a substance.
Hence, moles present in [tex]3.72 \times 10^{27}[/tex] atoms are calculated as follows.
[tex]Moles = \frac{3.72 \times 10^{27}}{6.022 \times 10^{23}}\\= 0.617 \times 10^{4} mol[/tex]
Thus, we can conclude that there are [tex]0.617 \times 10^{4}[/tex] moles present in [tex]3.72 \times 10^{27}[/tex] atoms of iron.
How do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the product?
Answer: It depends equilibrium constant K
Explanation: You need to to have reaction formula.
If K >> 1 then concentrations of products are much bigger than
concentrations of reactants. If K < < 1, concentration of products is small.
What is the limiting reactant in the following equation? How much Fe2O3 will be produced if 2.1 g of Fe reacts with 2.1 g of O2?
4 Fe + 3O2 —> 2Fe2O3
Answer:
Fe is limiting reactant and 3.00g of Fe2O3 will be produced
Explanation:
To solve this question we must convert the mass of each reactant to moles and, using the reaction we can find limiting reactant. With moles of limiting reactant we can find moles of Fe2O3 and its mass as follows:
Moles Fe -Molar mass: 55.845g/mol-
2.1g * (1mol / 55.845g) = 0.0376 moles
Moles O2 -Molar mass: 32g/mol-
2.1g * (1mol / 32g) = 0.0656 moles
For a complete reaction of 0.0656 moles of O2 are needed:
0.0656moles O2 * (4mol Fe / 3 mol O2) = 0.0875 moles Fe
As there are just 0.0376 moles,
Fe is limiting reactant
The mass of Fe2O3 is:
Moles:
0.0376 moles Fe* (2mol Fe2O3 / 4mol Fe) = 0.0188 moles Fe2O3
Mass:
0.0188 moles Fe2O3 * (159.69g / mol) =
3.00g of Fe2O3 will be produced
mrs tuckers class is doing an experiment they fill up a cup with ice water they measure the temperature of both the water and the classroom after one hour . what will mrs tucker observe about the temperature of ice water after one hour
A. The temperature will increase
B. The temperature Will remain the same
C. The temperature will decrease greatly
D. The temperature Will decrease slightly
Answer:
Ofc D. bc if the temp decreases, that means it is getting colder u dummy! But if it increases, it is getting warmer.
Explanation:
I got it right on USATestprep for using common sense, mark me the brainliest.
What compound(s) does pure water contain?
If the pH of a solution is 6.96, then the solution is a
Answer:
acid
Explanation:
solution with pH less than 7 is acid
those with more that 7 is base
those equal to 7 is neutral
If 3.13 mol of an ideal gas has a pressure of 2.33 atm and a volume of 72.31 L, what is the temperature of the sample in degrees Celsius?
Answer:
382.49 C degree Celsius
Explanation:
Hello,
This problem deals with understanding the ideal gas law which hopes to predict how ideal gases might behave in any given condition. I listed the formula below and we are basically just going to solve for temperature by rearranging the equation as seen on the picture (there's also other rearranged ones in case you need to solve for those).
Universal gas constant R has a value of 0.0821 L * atm/(mole * K) when working with these given units so it will be part of this equation. R value changes based on what units you have.
T = PV/nR
= (2.33) (72.31) / (3.13)(0.0821)
= 655.64 K
Question is asking temperature in celsius so we employ the formula attached below:
C = K - 273.15
= 655.64-273.15
= 382.49 degree Celsius
382.49 degree Celsius is the answer!
Calculate the molarity of the two solutions.
The first solution contains 0.200 mol of NaOH in 2.00 L of solution.
The second is 15.5G of NaCl in 671mL of solution
Answer:
a) 0.100 M
b) 0.395 M
Explanation:
a) Calculate the molarity of a solution that contains 0.200 moles of NaOH (solute) in 2.00 L of solution
We will use the following expression for molarity.
[NaOH] = moles of solute / liters of solution
[NaOH] = 0.200 mol/2.00 L = 0.100 M
b) Calculate the molarity for a solution that contains 15.5 g of NaCl (solute, 58.44 g/mol) in 671 mL of solution
We will use the following expression for molarity.
[NaCl] = mass of solute / molar mass of solute × liters of solution
[NaCl] = 15.5 g / 58.44 g/mol × 0.671 L = 0.395 M
Study the reaction.
CH4 + 2O2 → CO2 + 2H2O
If 7.4 moles of carbon dioxide (CO2) form at the end of the reaction, how many moles of methane (CH4) and oxygen gas (O2) entered the reaction?
? moles of methane and
? moles of oxygen gas
7.4 moles of methane (CH₄)
14.8 moles of oxygen gas (O₂)
What is the total number of moles of O2(g) that must react completely with 5.00 moles of C4H10(g)?
Answer:
32.5 moles of O2(g) are necessaries for a complete reaction
Explanation:
Based on the reaction of combustion of C4H10(g):
C4H10(g) + 13/2 O2(g) → 4CO2(g) + 5H2O(g)
1 mole of C4H10 needs 13/2 moles O2 for a complete reaction.
That means, the moles of O2 required for a reaction of 5.00 moles of C4H10 are:
5.00 moles C4H10 * (13/2mol O2 / 1mol C4H10) =
32.5 moles of O2(g) are necessaries for a complete reaction
Determine the hydroxide ion concentration in
a solution that is 0.00034 M Ca(OH)2.
Answer in units of M.
Answer:
[tex]0.00068M[/tex]
Explanation:
Hello there!
In this case, according to the ionization of calcium hydroxide, a strong base:
[tex]Ca(OH)_2\rightarrow Ca^{2+}+2OH^-[/tex]
Thus, since there is a 1:2 mole ratio of calcium hydroxide to hydroxide ions, we apply the following proportional factor to obtain:
[tex]0.00034\frac{molCa(OH)_2}{L}*\frac{2molOH^-}{1molCa(OH)_2} \\\\=0.00068\frac{OH^-}{L}\\\\=0.00068M[/tex]
Regards!
in writing a chemical equation that produces hydrogen gas, the correct representation of hydrogen gas is
a.H
b.2H
c.H2
d.OH
Answer:
h2
Explanation:
The cation that has the same number of electrons (isoelectronic) as Ne is
None of the listed options
O Na
Mg 2-
All of the listed options
O AI 3-
PLEASE HELP!! ORGANIC CHEMISTRY
A sample of a diatonic gas is loaded into an evacuated bottle at STP. The 0.25 L bottle contains 1.76 grams of the unidentified gas. Calculate the molar mass of the gas. What is the identity of the diatomic gas?
Answer:
(a) 157.7 g
(b) 7.04 g/dm³
Explanation:
(a) From the question,
According to Avogadro's Law,
1 mole of every gas at STP occupies a volume of 22.4 dm³
But mass of 1 mole of the diatomic gas = molar mass of the gas.
This Implies that,
The molar mass of the gas at STP occupies a volume of 22.4 dm³
From the question,
If,
0.25 L bottle contain 1.76 g of the gas,
Therefore,
Molar mass of the gas = (1.76×22.4)/0.25
Molar mass of the gas = 157.7 g.
(b) Density of the gas = mass/volume
D = m/v
Given: m = 1.76 g, v = 0.25 L = 0.25 dm³
Therefore,
D = 1.76/0,25
D = 7.04 g/dm³
8
What happens to solid waste in the circulatory system?
A it's expelled through the lungs
B
It pumps into the coronary circulation
C
It's dropped off in the kidneys
D
It's deposited in the aorta
Answer:c it’s dropped off in the kidneys
Explanation:
I took the quiz
The solid wastes are from the circulatory system is expelled to the kidney where, the nitrogenous wastes like urea and uric acid is excreted as urine from the body.
What is circulatory system ?A circulatory system is an organ system, where the blood is purified and oxygenation of blood takes place. Through circulatory system, the blood reaches throughout the body pumped from the heart through veins.
The organs included in circulatory system are lungs, heart, aorta, veins, blood vessels etc. There are various kinds of blood vessels each having specific functions.
There is a network of blood vessels including arteries and large veins, capillaries that join the venules and other veins. All the nutrients and ions are circulated throughout the body through blood and solid wastes are then expelled to kidney.
Kidney function as a sieve to clean the good fluid from waste products. Uric acid and urea along with water excreated as urine then. Thus, option C is correct.
To find more about circulatory system, refer the link below:
https://brainly.com/question/10103458
#SPJ6
_HCN+_CUSO4=_CUSO4+_CU(CN)2
Consider the aldol-dehydration reaction. Draw the two possible products of the reaction between benzaldehyde and methylethylketone. (Do not draw the products of the double-condensation.)
Solution :
An [tex]$\text{aldol condensation}$[/tex] reaction is a type of [tex]\text{condensation reaction}[/tex] in organic chemistry where the enol or an enolate ion reacts with the carbonyl compound and forms a [tex]$\beta$[/tex]-hydroxyaldehyde or a [tex]$\beta$[/tex]-hydroxyketone, and then followed by a dehydration to give conjugated enone.
Benzaldehyde reacts with methylketone and forms two products:
[H+] [OH-] =
NEED HELP ASAP!!!
A 251 ml sample of 0.45M HCl is added to 455 mL of distilled water. What is the molarity of the
final solution?
We are given:
251 mL sample of 0.45M HCl added to 455 mL distilled water
Whack a mole! (finding the number of moles):
We know that in order to find molarity, we use the formula:
Molarity = number of moles / Volume (in L)
so, number of moles is:
Number of moles = Molarity * Volume(in L)
now let's plug the values for the HCl solution to find the number of moles
Number of moles = 0.45M * 0.251 L
Number of moles = 0.113 moles
Time to concentrate (finding the final concentration):
Total final volume = 251 mL + 455 mL = 706 mL = 0.706 L
Number of moles of HCl = 0.113 moles
Molarity = Number of moles / Volume (in L)
Molarity = 0.113 / 0.706
Molarity = 0.16 M
___________________________________________________________
BONUS METHOD TIME!!!
We know the relation:
M1 * V1 = M2 * V2
where M1 and M2 are the initial and final molarities and V1 and V2 are initial and final volumes respectively
notice that I didn't mention that the volume has to be in Liters, that's because of the units being concerned with both sides of the equation, say I have the volume in mL and want to convert both these volumes to L, I would divide both sides by 1000, which would NOT change the overall value
Now, plugging values in this equation
(0.45) * (251) = (251 + 455)* (M2)
112.95 = (706)(M2)
M2 = 112.97/706 [dividing both sides by 706]
M2 = 0.16 Molar
A bottle labeled 0.01 M HCl is found in the laboratory. Assuming that the HCl is completely ionized calculate the [H+], [OH-] and the pH of the solution.
Answer:
[H⁺] = 0.01 M[OH⁻] = 1x10⁻¹² MpH = 2Explanation:
The assumption that the HCl is completely ionized means that the original concentration of the acid is equal to [H⁺].
[H⁺] = 0.01 MWith [H⁺], we can calculate [OH⁻], by using the following formula:
[H⁺] * [OH⁻] = 10⁻¹⁴0.01 M * [OH⁻] = 10⁻¹⁴[OH⁻] = 1x10⁻¹² MFinally we calculate the pH of the solution:
pH = -log[H⁺]pH = 2Do u believe that you are beautiful/handsome?
Yes or No?