H2C=CH2 + H2 решение?
Answer:
[tex]CH _{3}CH _{3}[/tex]
Ethane
The Kc for the following is 5.0 at 100 degrees Celsius.
If an equilibrium mixture contains 0.53 M NO2 what is the molar concentration of N2O4?
Answer:
1.40M = [N2O4]
Explanation:
Based on the reaction:
2NO2(g) ⇄ N2O4(g)
Kc is defined as:
Kc = 5.0 = [N2O4] / [NO2]²
Where [] are the concentrations in equilibrium of each gas
As the equilibrium concentration of NO2 is 0.53M:
5.0 = [N2O4] / [0.53]²
5.0 = [N2O4] / [0.2809]
5.0*0.2809 = [N2O4]
1.40M = [N2O4]After the student closes the cooler, there NOT any inputs or outputs from this system because ________. a. no energy is being transferred into or out of the cooler b. there is no flow of energy across the system boundary c. there is no matter flowing into or out of the system d. all of the above
Answer:
d. All of the above
Explanation:
d. All of the above
what is the importance of energy in humans
Explanation:
Energy is essential to life and all living organisms. The sun, directly or indirectly, is the source of all the energy available on Earth. Our energy choices and decisions impact Earth's natural systems in ways we may not be aware of, so it is essential that we choose our energy sources carefully
Give the following for SO2 and BrF5:
(a) Number of domains on central atom (b) Domain geometry (c) Molecular geometry (d) Hybridization of central atom
Answer:
The given molecules are SO2 and BrF5.
Explanation:
Consider the molecule SO2:
The central atom is S.
The number of domains on S in this molecule is three.
Domain geometry is trigonal planar.
But there is a lone pair on the central atom.
So, according to VSEPR theory,
the molecular geometry becomes bent or V-shape.
Hybridization on the central atom is
[tex]sp^{2}[/tex].
Consider the molecule BrF5:
The central atom is Br.
The number of domains on the central atom is six.
Domain geometry is octahedral.
But the central atom has a lone pair of electrons.
So, the molecular geometry becomes square pyramidal.
The hybridization of the central atom is [tex]sp^{3} d^{2}[/tex].
The shapes of SO2 and BrF5 are shown below:
is Decanitrogen tetroxide Ionic or Molecular
Answer:
Decanitrogen is molecular
Explanation:
Answer:
Dec a nitrogen is Molecular
Explanation:
hey mate i hope it will help you...!
What’s the answer to the question
Answer: B
Explanation: im pretty sure my teacher mentioned something about N--h bonds are non polar
Answer:
C
Explanation:
50.0 g of Potassium chloride reacts with 50.0 g of oxygen to produce KCIO3. After writing
and balancing the reaction, determine the amount of potassium chlorate produced
128 g
32.0 g
082.2 g
None of these answers.
Explanation:
If 50.0 grams of Zinc are reacted with 50.0 grams of Hydrogen Chloride ... 50.09 Zn x 1 mol Zn , Imol ZnCl2 , 136.4g. ... If a decomposition reaction produces a 75.0% yield for the oxygen by mass (128.0 grams were.
What is the correct answer question
Answer:
B
Explanation:
In the reaction represented by the equation: N2 + 3H2 → 2NH3, what is the conversion factor of nitrogen to ammonia? Explain by using law of definite proportion
Answer:
10/3
Explanation:
Hope this helps
Answer:
The compound formula for the ammonia is
N
H
3
. It is a colorless gas. It is the result of the chemical reaction between nitrogen and hydrogen gas. The chemical reaction between the gases is shown below:
N
2
+
3
H
2
→
2
N
H
3
Determine how much sulfuric acid (in metric tons) is produced by the combustion of 1.2 metric ton of this coal. (A metric ton is 1000 kg.)
Helpppp
What is the volume of 2.99 moles of C3H8 at STP?
0.0680L
5.87 L
ОООО
1.52 L
67.0L
Answer:
67.0 L
Explanation:
Step 1: Given data
Moles of C₃H₈: 2.99 molPressure: 1 atm (standard pressure)Temperature: 273.15 K (standard temperature)Step 2: Calculate the volume occupied by 2.99 moles of C₃H₈ at STP
C₃H₈ is a gas. If we assume ideal behavior, 1 mole of C₃H₈ at STP occupies 22.4 L.
2.99 mol × 22.4 L/1 mol = 67.0 L
what is the enthalpy of the overall chemical reaction
Answer:
For a chemical reaction, the enthalpy of reaction (ΔHrxn) is the difference in enthalpy between products and reactants; the units of ΔHrxn are kilojoules per mole
NO2 (nitrogen dioxide) is a Greenhouse Gas that can be produced in car engines. The average diesel truck produces 80g of NO2 for every 1000 kilometers it drives. How many moles of NO2 are in 80g of NO2?
Answer:
[tex]1.74molNO_2[/tex]
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to perform mole-mass relationships by using the molar mass of the involved substance, in this case NO2, which is 46.0 g/mol; then we just set up a conversion factor like the one shown below:
[tex]80g*\frac{1mol}{46g}\\\\1.74molNO_2[/tex]
Regards!
Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm.
Answer: The frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm is [tex]5.49 \times 10^{14} s^{-1}[/tex].
Explanation:
Given: Wavelength = 546 nm [tex](1 nm = 10^{-9} m)[/tex] = [tex]546 \times 10^{-9} m[/tex]
The relation between frequency and wavelength is as follows.
[tex]\nu = \frac{c}{\lambda}[/tex]
where,
[tex]\nu[/tex] = frequency
c = speed of light = [tex]3.0 \times 10^{8} m/s[/tex]
[tex]\lambda[/tex] = wavelength
Substitute the values into above formula as follows.
[tex]\nu = \frac{c}{\lambda}\\= \frac{3.0 \times 10^{8} m/s}{546 \times 10^{-9} m}\\= 5.49 \times 10^{14} s^{-1}[/tex]
Thus, we can conclude that the frequency of the green light emitted by a hydrogen atom with a wavelength of 546 nm is [tex]5.49 \times 10^{14} s^{-1}[/tex].
A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is Determine the concentration of the permanganate solution in molarity. g
The question is incomplete, the complete question is:
A solution of permanganate is standardized by titration with oxalic acid. To react completely with 0.0018 mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:
[tex]\mathrm{MnO}_{4}^{-}(aq)+\mathrm{H}_{2}\mathrm{C}_{2}\mathrm{O}_{4}(aq)\stackrel{\mathrm{Acidic}}{\longrightarrow}\mathrm{Mn}^{2+}(aq)+\mathrm{CO}_{2}(\mathrm{g})[/tex]
Determine the concentration of the permanganate solution in molarity.
Answer: The molarity of permanganate solution is 0.026 M
Explanation:
The balanced chemical equation follows:
[tex]2MnO_4^-(aq)+6H^+(aq)+5H_2C_2O_4(aq)\rightarrow 2Mn^{2+}+8H_2O(l)+10CO_2(g)[/tex]
Given values:
Moles of oxalic acid = 0.0018 moles
By the stoichiometry of the reaction:
If 5 moles of oxalic acid reacts with 2 moles of permanganate solution
So, 0.0018 moles of oxalic acid will react with = [tex]\frac{2}{5}\times 0.0018mol=0.00072mol[/tex] of permanganate solution
Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:
[tex]\text{Molarity of solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (mL)}}[/tex] .....(1)
Given values:
Moles of permanganate solution = 0.00072 moles
Volume of solution = 28.18 mL
Putting values in equation 1, we get:
[tex]\text{Molarity of permanganate solution}=\frac{0.00072\times 1000}{28.18}\\\\\text{Molarity of permanganate solution}=0.026M[/tex]
Hence, the molarity of permanganate solution is 0.026 M
If the H3O is 4.950 x 10-12 what is the ph?
Answer:
pH = 11.3
Explanation:
From the question given above, the following data were obtained:
Concentration of hydronium ion [H₃O⁺] = 4.950×10¯¹² M
pH =.?
The pH of a solution is defined by the following equation:
pH = –Log [H₃O⁺]
Thus, with the above formula, we can obtain the pH of the solution as follow:
Concentration of hydronium ion [H₃O⁺] = 4.950×10¯¹² M
pH =.?
pH = –Log [H₃O⁺]
pH = –Log 4.950×10¯¹²
pH = 11.3
Consider the reaction between solid C and O2 gas which makes CO2;
C+02 -> CO2
If we have a 14 L container of O2 gas at a pressure of 3.0 atm and a temperature of 298 K and we add 36 g of solid C to the
container, then how many grams of CO2 will be produced by this reaction?
Answer:
[tex]m_{CO_2}=75.6gCO_2[/tex]
Explanation:
Hello there!
In this case, according to the given information, it turns out mandatory for us to calculate the reacting moles of both C and O2 because we are given grams and pressure, temperature and volume, respectively:
[tex]n_C=36gC*\frac{1molC}{12gC}=3.0molC \\\\n_{O_2}=\frac{3.0atm*14L}{0.08206\frac{atm*L}{mol*K}*298K}=1.72molO_2[/tex]
Thus, since C and O2 react in a 1:1 mole ratio, we infer C is in excess, and the grams of CO2 can be calculated with the moles of O2:
[tex]m_{CO_2}=1.72molO_2*\frac{1molCO_2}{1molO_2}*\frac{44.01gCO_2}{1molCO_2} \\\\ m_{CO_2}=75.6gCO_2[/tex]
Best regards!
What the correct answer
Answer:
none
Explanation:
the correct option would be Ar 3d3 4s2
Distinguish between
real and virtuaI image
Answer:
(Basic )
Real
These are formed in the front side of the mirror.
Virtual
These are assumed to be formed at the backside of the mirror.
Type of lens used
Converging(real)
Diverging(virtual)
Image reception
Image can be appeared on a screen.(Real)
Image appears to be on the mirror or lens itself.
Interaction of light rays Actual Imaginary(Virtual)
Appearance of image
Inverted(Real)
Erect(Virtual)
Formed by
Concave mirror and convex lens.(Real)
Plane, convex mirror and concave lens.(Virtual)
Example
Image on the theater screen.(Real)
Reflection of any object or body on plane mirror.(Virtual)
When 125 mL of 0.150 M Pb(NO3)2 is mixed with 145 mL of 0.200 M KBr, 4.92 g of PbBr2 is collected. Calculate the percent yield.
Answer:
Y = 92.5 %
Explanation:
Hello there!
In this case, since the reaction between lead (II) nitrate and potassium bromide is:
[tex]Pb(NO_3)_2+2KBr\rightarrow PbBr_2+2KNO_3[/tex]
Exhibits a 1:2 mole ratio of the former to the later, we can calculate the moles of lead (II) bromide product to figure out the limiting reactant:
[tex]0.125L*0.150\frac{molPb(NO_3)_2}{L} *\frac{1molPbBr_2}{1molPb(NO_3)_2} =0.01875molPbBr_2\\\\0.145L*0.200\frac{molKBr}{L} *\frac{1molPbBr_2}{2molKBr} =0.0145molPbBr_2[/tex]
Thus, the limiting reactant is the KBr as it yields the fewest moles of PbBr2 product. Afterwards, we calculate the mass of product by using its molar mass:
[tex]0.0145molPbBr_2*\frac{367.01gPbBr_2}{1molPbBr_2} =5.32gPbBr_2[/tex]
And the resulting percent yield:
[tex]Y=\frac{4.92g}{5.32g} *100\%\\\\Y=92.5\%[/tex]
Regards!
12. NAD and NADPH are distinguished from each other by the
that's bonded to the sugar ring attached to the adenine.
O A. phosphate group
O B. adenine
O C. carbon dioxide
O D. nicotinamide
Answer:
A. phosphate group
Explanation:
I got it right in class!
Hope this Helps!! :))
Name a machine used to reap, thresh and clean the crop.
i will give brainliest who answers first
Answer:
combine harvester, or a combiner.
HELP PLEASE HURRY!!!
You have 12.51 grams of C2H6, how many moles do you have?
Answer:
How many grams C2H6 in 1 mol? The answer is 30.06904. We assume you are converting between grams C2H6 and mole. You can view more details on each measurement unit
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Hsvhpsvuwgycwhusvywgogwitcsuovsigsviyscyisvyos
Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.0 kg of SiO2 is allowed to react with 78.2 kg of carbon to produce 66.0 kg of silicon.
Required:
a. What is the theoretical yield for the reaction in Kg Si?
b. What is the percent yield for the reaction?
Answer:
(a): The theoretical yield of silicon is 72.33 kg.
(b): The percent yield of the reaction is 91.25 %.
Explanation:
Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.
Excess reagent is defined as the reagent which is left behind after the completion of the reaction.
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
For [tex]SiO_2[/tex]:
Given mass = 155.0 kg = 155000 g (Conversion factor: 1 kg = 1000 g)
Molar mass = 60 g/mol
Putting values in equation 1:
[tex]\text{Moles of }SiO_2=\frac{155000g}{60g/mol}=2583.3mol[/tex]
For carbon:
Given mass = 78.2 kg = 78200 g
Molar mass = 12 g/mol
Putting values in equation 1:
[tex]\text{Moles of carbon}=\frac{78200g}{12g/mol}=6516.67mol[/tex]
The chemical equation for the reaction of silicon dioxide and carbon follows:
[tex]SiO_2+2C\rightarrow Si+2CO[/tex]
By stoichiometry of the reaction:
1 mole of [tex]SiO_2[/tex] reacts with 2 moles of carbon
So, 2583.3 moles of [tex]SiO_2[/tex] will react with = [tex]\frac{2}{1}\times 2583.3=5166.4mol[/tex] of carbon
As the given amount of carbon is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.
Thus, [tex]SiO_2[/tex] is considered a limiting reagent because it limits the formation of the product.
For (a):By stoichiometry of the reaction:
1 mole of [tex]SiO_2[/tex] produces 1 mole of silicon
So, 2583.3 moles of [tex]SiO_2[/tex] will produce = [tex]\frac{1}{1}\times 2583.3=2583.3mol[/tex] of silicon
Since the molar mass of silicon = 28 g/mol
Putting values in equation 1:
[tex]\text{Mass of Si}=2583.3mol\times 28g/mol=72332.4g=72.33 kg[/tex]
Hence, the theoretical yield of silicon is 72.33 kg.
For (b):The percent yield of a reaction is calculated by using an equation:
[tex]\% \text{yield}=\frac{\text{Measured value}}{\text{Theoretical value}}\times 100[/tex] ......(2)
Given values:
Measured value of silicon = 66.0 kg
Theoretical value of silicon = 72.33 kg
Putting values in equation 1:
[tex]\% \text{yield}=\frac{66.0kg}{72.33kg}\times 100\\\\\% \text{yield}=91.25 \%[/tex]
Hence, the percent yield of the reaction is 91.25 %.
How many molecules of carbon dioxide would be formed if 6.75 g of propane is burned in the following reaction?
dont mind me here for the points
HELPP
There are 9.23 x 1023 molecules of water in a beaker, how many moles are there?
Answer:
Answer: There are 1.53 moles present in molecules of water in a beaker.
Explanation:
According to the mole concept, there are molecules present in 1 mole of a substance.
So, number of moles present in molecules are calculated as follows.
Thus, we can conclude that there are 1.53 moles present in molecules of water in a beaker.
Explanation:
Ibuprofen, a well‑known, non‑steroidal anti‑inflammatory drug, has chirality.
a. True
b. False
Answer:
A (True)
Explanation:
Because ibuprofen has a chiral carbon center (carbon bonded to 4 distinct groups of atoms).
This means that a mixture of ibuprofen can rotate plane-polarized light equally in both the clockwise and counterclockwise direction.
Answer:true
Explanation: ibuprofen is commonly used for most pain, aches ect
Aerobic respiration is the cellular process in which
A)
oxygen is added to citric acid, providing energy to the cell.
B)
oxygen is added to NAD+ to form NADH.
C)
oxygen is added to an organic fuel, providing energy to the cell.
D)
oxygen is added to ATP, providing energy to the cell.
Answer:
oxygen is add to ATP providing energy to the cell
