Determine the molecular formula of the following given the imperial formula and molecular mass A.EF=NO2, 92.5g=molecular massB.EF=NaPO3, 305.9g=molecular mass
1. Determine the molecular formula of the following given the imperial formula and molecular mass A.EF=NO2, 92.5g=molecular massB.EF=NaPO3, 305.9g=molecular mass
pa answer din po please hindi ko din alam
2. Determine the molecular formula of the following given the empirical formula and molecular mass.A.EF = NO2, 92.5g= molecular massB. EF = NaPO3, 305.9g= molecular mass
Hopefully, I can help your study for this answer, God Bless!
Answer:
A.
Solution:
Step 1: Represent a molecular formula.
molecular formula = (NO2)n
Step 2: Calculate the empirical mass.
empirical mass = (14.01 g × 1) + (16.00 g × 2)
empirical mass = 46.01 g
Step 3: Divide the molecular mass by the empirical mass.
n = molecular mass/empirical mmas
n = 92.5 g/46.01 g
n = 2
Step 4: Multiply the subscripts by the value of n to obtain the molecular formula.
molecular formula = (NO2)2
molecular formula= (N204)
B.
Solution:
Step 1: Represent a molecular formula.
molecular formula = (NaPO3)n
Step 2: Calculate the empirical mass.
empirical mass = (23 g × 1) + (31 g × 1) + (16g x 3)
= 23g + 31g + 48g
empirical mass = 102 g
Step 3: Divide the molecular mass by the empirical mass.
n = molecular mass/empirical mmas
n = 305.9 g/102 g
n = 3
Step 4: Multiply the subscripts by the value of n to obtain the molecular formula.
molecular formula = (NaPO3)3
molecular formula= (Na3P3O9)
3. 2. Determine the molecular formula of the following given the empirical formulaand molecular mass.A. EF = NO2, 92.5g = molecular massB. EF =NaPO3, 305.9g = molecular mass
Hopefully, I can help your study for this answer, God Bless!
Answer:
A.
Solution:
Step 1: Represent a molecular formula.
molecular formula = (NO2)n
Step 2: Calculate the empirical mass.
empirical mass = (14.01 g × 1) + (16.00 g × 2)
empirical mass = 46.01 g
Step 3: Divide the molecular mass by the empirical mass.
n = molecular mass/empirical mmas
n = 92.5 g/46.01 g
n = 2
Step 4: Multiply the subscripts by the value of n to obtain the molecular formula.
molecular formula = (NO2)2
molecular formula= (N204)
B.
Solution:
Step 1: Represent a molecular formula.
molecular formula = (NaPO3)n
Step 2: Calculate the empirical mass.
empirical mass = (23 g × 1) + (31 g × 1) + (16g x 3)
= 23g + 31g + 48g
empirical mass = 102 g
Step 3: Divide the molecular mass by the empirical mass.
n = molecular mass/empirical mmas
n = 305.9 g/102 g
n = 3
Step 4: Multiply the subscripts by the value of n to obtain the molecular formula.
molecular formula = (NaPO3)3
molecular formula= (Na3P3O9)
4. Activity 1. Molecular MassCompute the molecular mass of the given compounds.
Answer:
the answer is in the picture
5. what is the main difference among the formula mass molecular mass and molar mass
Molecular weight is the mass of one molecule of a substance while the molar mass is the mass of one mole of a substance.
6. what is the molecular mass of C12O7
Explanation:
Molar mass of C1207 is 14496.9149 g/mol
Convert between C1207 weight and moles
7. composition of molecular mass
Percent composition is calculated from a molecular formula by dividing the mass of a single element in one mole of a compound by the mass of one mole of the entire compound. This value is presented as a percentage
8. The molecular mass of an organic acid that occurs in leafy vegetables, whose empirical formula is HCO2 is twice its empirical mass. What is the molecular mass of the acid?
Answer:
molecular mass = 90.04 g/mol
Explanation:
Calculating the empirical mass
empirical mass = (1.008 g/mol × 1) + (12.01 g/mol × 1) + (16.00 g/mol × 2)
empirical mass = 45.02 g/mol
Calculating the molecular mass
molecular mass = 2 × empirical mass
molecular mass = 2 × 45.02 g/mol
molecular mass = 90.04 g/mol
#CarryOnLearning
9. What is the molecular mass/ molar mass of dichlorine heptoxide?
Answer:
Dichlorine Heptoxide
Explanation:
pa follow pii, thanks:)
10. What is the empirical and molecular formula of a substance containing 43.64% phosphorus and 56. 36% oxygen by mass? Its molecular mass is 141.9g
SOLUTION: (Empirical Formula)
Step 1: Assume that the mass of a compound is 100 g.
[tex]\begin{aligned} & mass_{\text{P}} = \text{43.64 g} \\ & mass_{\text{O}} = \text{56.36 g} \end{aligned}[/tex]
Step 2: Calculate the number of moles of each element.
[tex]\begin{aligned} & n_{\text{P}} = \text{43.64 g} \times \frac{\text{1 mol}}{\text{30.97 g}} = \text{1.409 mol} \\ & n_{\text{O}} = \text{56.36 g} \times \frac{\text{1 mol}}{\text{16.00 g}} = \text{3.5225 mol} \end{aligned}[/tex]
Step 3: Represent an empirical formula.
[tex]\text{empirical formula} = \text{P}_x\text{O}_y[/tex]
Step 4: Divide the moles of each element by the least number of moles.
In this case, the least number of moles is 1.409 mol.
[tex]\begin{aligned} & x = \frac{\text{1.409 mol}}{\text{1.409 mol}} = 1 \\ & y = \frac{\text{3.5225 mol}}{\text{1.409 mol}} = 2.5 \end{aligned}[/tex]
Step 5: Multiply the subscripts obtained by a certain number to become whole number.
Since the decimal part of 2.5 is 0.5, we need to multiply all the subscripts by 2. Therefore,
[tex]\begin{aligned} & x = 1 \times 2 = 2 \\ & y = 2.5 \times 2 = 5 \end{aligned}[/tex]
Step 6: Write the empirical formula.
[tex]\text{empirical formula} = \boxed{\text{P}_2\text{O}_5}[/tex]
Hence, the empirical formula of a substance is P₂O₅.
-----------------------------------------------------
SOLUTION: (Molecular Formula)Step 1: Represent a molecular formula.
[tex]\text{molecular formula} = (\text{P}_2\text{O}_5)_n[/tex]
Step 2: Calculate the empirical mass.
[tex]\begin{aligned} \text{empirical mass} & = \text{2(30.97 g) + 5(16.00 g)} \\ & = \text{61.94 g + 80.00 g} \\ & = \text{141.9 g} \end{aligned}[/tex]
Step 3: Divide the molecular mass by the empirical mass to find the value of n.
[tex]\begin{aligned} n & = \frac{\text{molecular mass}}{\text{empirical mass}} \\ & = \frac{\text{141.9 g}}{\text{141.9 g}} \\ & = 1 \end{aligned}[/tex]
Step 4: Multiply the subscripts by the value of n to obtain the molecular formula.
[tex]\begin{aligned} \text{molecular formula} & = (\text{P}_2\text{O}_5)_1 \\ & = \boxed{\text{P}_2\text{O}_5} \end{aligned}[/tex]
Hence, the molecular formula of a substance is P₂O₅.
11. 1.) What is the molecular mass of 2NaCI ? 2.) What is rhe molecular mass of Pb(NO3)2 ?3.) What is the molecular mass of 15CO2 ?
1. 58.44 g/mol
The molar mass of sodium chloride is 58.44 g/mol.
2. 331.2 g/mol
3. The molecular mass of carbon dioxide is 44.01amu. The molar mass of any compound is the mass in grams of one mole of that compound. One mole of carbon dioxide molecules has a mass of 44.01g, while one mole of sodium sulfide formula units has a mass of 78.04g.
12. The molecular formula of aspartame is c14h18n2o5. what is the molecular mass of aspartame
Answer:
Aspartame
Molar mass
294.3 g/mol
Explanation:
Hope it helps.<333
13. DIFFENTIATING MOLECULAR MASS AND FORMULA MASSpahelp pls
Answer:
The formula mass (formula weight) of a molecule is the sum of the atomic weights of the atoms in its empirical formula. The molecular mass (molecular weight) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the molecular formula.
14. why does methane boil at a very low temperature it is because the methane hasA. lower molecular massB. higher molecular massC. lower empirical massD. higher molecular mass
Answer: C. lower molecular mass
Explanation: Because methane (CH4) is a non-polar molecule the molecules are held together only by London Dispersion Forces which are very weak and easy to break. These bonds break when methane boils and because they are weak, it boils at a
low temperature.
15. solving for Molecular Mass
Answer:
Multiply the subscript (number of atoms) times the atomic mass of that element and add the masses of all of the elements in the molecule to get the molecular
16. find the molecular mass of glucose which has a molecular formula (C6H1206)
Answer:
180 g
Step-by-step explanation:
17. what is the molecular formula of C2H4 and molecular mass of 88 g
Answer:
Good morning guys sa inyo
18. Calculate the molecular mass of NH3.
Answer:
17.031 g/mol
Explanation:
Yan lang po hope it helps paki brainliest po
19. What's MoreActivity 1. Molecular MassCompute the molecular mass of the given compounds.Pa help nmn po
Answer:
I'm sorry I'm best in math but di ka matututo Kong I bebrainly mo
Explanation:
isagot mo Po Kong ano sa tingin mo dahil sa brainly di Po lahat ay tama
20. compare and contrast molar mass and molecular mass
Answer:
Moreover, the main difference between both is that "molar mass gives the mass of a mole of a particular substance". Whereas "molecular weight is the mass of a molecule of a particular substance". While the definition and units are different for molar mass and molecular weight, the value is the same
I hope it helps, correct my answer if wrong.
21. What is the molecular mass of 8SO4?
Answer:
[tex]\bold{What \: \: is \: \: the \: \: molecular} \\ \bold{mass \: of \: 8SO_{4} ? } \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: [/tex] 768.5008 g/mol22. diselenium pentasulfide molecular mass?
Answer:
Molecular Weight143.1Computed by PubChem 2.1 (PubChem release 2021.05.07)Hydrogen Bond Donor Count0Computed by Cactvs 3.4.8.18 (PubChem release 2021.05.07)Hydrogen Bond Acceptor Count2Computed by Cactvs 3.4.8.18 (PubChem release 2021.05.07)Rotatable Bond Count0Computed by Cactvs 3.4.8.18 (PubChem release 2021.05.07)Exact Mass143.86066Computed by PubChem 2.1 (PubChem release 2021.05.07)Monoisotopic Mass143.86066Computed by PubChem 2.1 (PubChem release 2021.05.07)Topological Polar Surface Area64.2 ŲComputed by Cactvs 3.4.8.18 (PubChem release 2021.05.07)Heavy Atom Count3Computed by PubChemFormal Charge0Computed by PubChemComplexity18.3Computed by Cactvs 3.4.8.18 (PubChem release 2021.05.07)Isotope Atom Count0Computed
qhello copy that thats the Answer:) hope it helps
23. how is molecular mass calculated?
Answer:
Molecular mass is calculated by adding up the atomic masses of all the atoms in a molecule. The atomic mass of an element is the number of protons and neutrons in the nucleus of an atom of that element. These values can be found on the periodic table of elements. To calculate the molecular mass, you need to know the chemical formula of the molecule, which tells you how many atoms of each element are present in the molecule. Once you know this, you can look up the atomic mass of each element on the periodic table and add them together to find the molecular mass of the molecule.
For example, if you wanted to calculate the molecular mass of water (H2O), you would look up the atomic mass of hydrogen (1.008 amu) and oxygen (16.00 amu) on the periodic table and add them together:
1.008 amu + (2*16.00 amu) = 18.02 amu
So, the molecular mass of water is 18.02 amu.
Answer:
Determine the molecular formula of the molecule. Use the periodic table to determine the atomic mass of each element in the molecule. Multiply each elements atomic mass by the number of atoms of that element in the molucule.
PA BRAINLEST POH THANK YOU POH, HOPE IT'S HELP#CARRYONLEARNING24. Calculate the molecular mass of sulphur
Answer:
32.065Explanation:
The atomic weight of sulfur atom = 32g. ∴ Molar mass of sulfur = 256g25. what is the molecular mass of NHCO3
Answer:
Molar mass of NaHCO3 = 84.00661 g/mol.
Explanation:
This compound is also known as Baking Soda or Sodium Bicarbonate. Convert grams NaHCO3 to moles or moles NaHCO3 to grams. 22.98977 + 1.00794 + 12.0107 + 15.9994*3
Answer:
84.007 g/mol
Formula: NaHCO₃
IUPAC ID: Sodium hydrogen carbonate
Molar mass: 84.007 g/mol
Density: 2.2 g/cm³
Molar entropy: 102 J/(mol⋅K)
Soluble in: Water
Explanation:
hope it helps:))
26. A compound is 75.46% carbon, 4.43% hydrogen, and 20.10% oxygen by mass. It has a molecular mass of 318 g/mol. What is the molecular formula for this compound if it has a molecular mass of 318 g/mol? Select the correct response
[tex] \huge\red{\overbrace{\underbrace{\tt\blue{\:\:\:\:\:\:\:\:ANSWER:\:\:\:\:\:\:\:\:}}}} [/tex]
[tex] \sf \pink{––––––––––––––––––––––––––––––––––––––––––––––––}[/tex]
Get the mass of each element by assuming a certain overall mass for the sample (100 g is a good mass to assume when working with percentages).
(.7546) (100 g) = 75.46 g C(.0443) (100 g) = 4.43 g H(.2010) (100 g) = 20.10 g OConvert the mass of each element to moles.
(75.46 g C) (1 mol/ 12.00 g C) = 6.289 mol C(4.43 g H) (1 mol/ 1.008 g H) = 4.39 mol H(20.10 g O) (1 mol/ 16.00 g O) = 1.256 mol OFind the ratio of the moles of each element.
(1.256 mol O)/ (1.256) = 1 mol O(6.289 mol C)/ (1.256) = 5.007 mol C(4.39 mol H)/ (1.256) = 3.50 mol HUse the mole ratio to write the empirical fomula.
Multiplying the mole ratios by two to get whole number, the empirical formula becomes:
C10H7O2Find the mass of the empirical unit.
10(12.00) + 7(1.008) + 2(16.00) = 159.06 g/molFigure out how many empirical units are in a molecular unit.
(318.31 g/mol) / (159.06 g/mol) = 2.001 empirical units per molecular unitWrite the molecular formula.
Since there are two empirical units in a molecular unit, the molecular formula is:
C20H14O4[tex] \sf \pink{––––––––––––––––––––––––––––––––––––––––––––––––}[/tex]
[tex] \rm{⚘JichuSooya03⚘}[/tex]27. what is the molecular formula of a compound that has 85.7% carbon and 14.3% hydrogen by mass, if the molecular mass is 28g/mol
SOLUTION:
Step 1: Assume that the mass of a compound is 100 g.
[tex]\begin{aligned} & mass_{\text{C}} = \text{85.7 g} \\ & mass_{\text{H}} = \text{14.3 g} \end{aligned}[/tex]
Step 2: Calculate the number of moles of each element.
[tex]\begin{aligned} & n_{\text{C}} = \text{85.7 g} \times \frac{\text{1 mol}}{\text{12.01 g}} = \text{7.136 mol} \\ & n_{\text{H}} = \text{14.3 g} \times \frac{\text{1 mol}}{\text{1.008 g}} = \text{14.2 mol} \end{aligned}[/tex]
Step 3: Represent an empirical formula.
[tex]\text{empirical formula} = \text{C}_x\text{H}_y[/tex]
Step 4: Divide the moles of each element by the least number of moles.
In this case, the least number of moles is 7.136 mol.
[tex]\begin{aligned} & x = \frac{\text{7.136 mol}}{\text{7.136 mol}} = 1 \\ & y = \frac{\text{14.2 mol}}{\text{7.136 mol}} \approx 2 \end{aligned}[/tex]
Step 5: Write the empirical formula.
[tex]\text{empirical formula} = \text{CH}_2[/tex]
Step 6: Represent a molecular formula.
[tex]\text{molecular formula} = (\text{CH}_2)_n[/tex]
Step 7: Calculate the empirical mass.
[tex]\begin{aligned} \text{empirical mass} & = \text{12.01 g/mol + 2(1.008 g/mol)} \\ & = \text{14.03 g/mol} \end{aligned}[/tex]
Step 8: Divide the molecular mass by the empirical mass to find the value of n.
[tex]\begin{aligned} n & = \frac{\text{molecular mass}}{\text{empirical mass}} \\ & = \frac{\text{28 g/mol}}{\text{14.03 g/mol}} \\ & \approx 2 \end{aligned}[/tex]
Step 9: Multiply the subscripts by the value of n to obtain the molecular formula.
[tex]\begin{aligned} \text{molecular formula} & = (\text{CH}_2)_2 \\ & = \boxed{\text{C}_2\text{H}_4} \end{aligned}[/tex]
Hence, the molecular formula of a compound is C₂H₄.
28. molecular mass of C3H5N3O9
Answer:
227.0865 g/mol
Melting point: 14 °C
Density: 1.6 g/cm³
Formula: C3H5N3O9
227.0865 g/molMelting point: 14 °C
Density: 1.6 g/cm³
Formula: C3H5N3O9
29. molecular mass .compute the molecular mass of the given compounds .write your answer on a separate sheet of paper brainly
Explanation:
It's easy to find the molecular mass of a compound with these steps:
•Determine the molecular formula of the molecule.
•Use the periodic table to determine the atomic mass of each element in the molecule.
•Multiply each element's atomic mass by the number of atoms of that element in the molecule.
30. Activity 1. Molecular Mass Compute the molecular mass of the given compounds. Write your answer on a separate sheet of paper.
Answer:
Pb(NO3)2
Pb 1 x 207 = 207 g/mol
N 2 x 14 = 28 g/mol
O 6 x 16 = 96 g/mol
molecular mass =>331g/mol
(NH4)2SO4
N 2 x 14 = 28 g/mol
H 8 x 1 = 8 g/mol
S 1 x 32 = 32 g/mol
O 4 x 16 = 64 g/mol
molecular mass. => 132 g/mol
