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The empirical formula for d2h, which likely refers to deuterium (D) and hydrogen (H), is typically represented as CH2. In this context, "d2" indicates the presence of two deuterium atoms, which are isotopes of hydrogen. Therefore, the empirical formula simplifies to the ratio of the elements present, which is CH2, representing one carbon atom and two hydrogen atoms (or deuterium in this case).
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Can any one substance have the same empirical formula and molecular formula?
Yes, a substance can have the same empirical formula and molecular formula if it consists of the simplest whole number ratio of its elements, and that ratio also represents the actual number of atoms in a molecule. This occurs in compounds like water (H₂O), where the empirical formula (H₂O) and the molecular formula (also H₂O) are identical. However, this is not the case for substances with larger molecular structures, where the empirical formula would typically represent a reduced ratio of atoms compared to the molecular formula.
What is a molecular formula 264g with a empirical formula of C3H4O3?
To determine the molecular formula from the empirical formula (C₃H₄O₃) and the given molar mass (264 g), first, calculate the molar mass of the empirical formula: C (12.01 g/mol) × 3 + H (1.01 g/mol) × 4 + O (16.00 g/mol) × 3 = 88.11 g/mol. Next, divide the given molar mass by the empirical formula mass: 264 g / 88.11 g/mol ≈ 3. This means the molecular formula is three times the empirical formula, resulting in C₉H₁₂O₉.
How are the empirical and molecule formulas for a compound related?
The empirical formula of a compound represents the simplest whole-number ratio of the elements present, while the molecular formula indicates the actual number of atoms of each element in a molecule of the compound. The molecular formula can be a multiple of the empirical formula, meaning that it may contain the same elements in a proportion that is a whole number multiple of the empirical ratio. For example, if the empirical formula is CH₂, the molecular formula could be C₂H₄, C₃H₆, etc., depending on the actual number of atoms in the molecule.
Different molecules with the same empirical formula?
Empirical formulaCompoundMolecularformulaCH (92.2% C; 7.8% H)acetyleneC2H2benzeneC6H6CH2 (85.6% C; 14.4% H)ethyleneC2H4buteneC4H8CH2O (40.0% C; 6.7% H;53.3% O)formaldehydeCH2Oacetic acidC2H4OglyceraldehydeC3H6O3The molecular formula may be a multiple of the empirical formula.
Determine the molecular formula for the unknown if the molecular mass is 60.0 amu and the empirical formula is CH2O.?
To determine the molecular formula from the empirical formula CH2O and given molecular mass of 60.0 amu, calculate the empirical formula mass: (12.01 g/mol for C) + 2(1.01 g/mol for H) + 16.00 g/mol for O = 30.02 g/mol. Then divide the given molecular mass by the empirical formula mass to find the factor by which the empirical formula must be multiplied to get the molecular formula: 60.0 amu / 30.02 g/mol ≈ 2. Next, multiply the subscripts in the empirical formula by this factor to find the molecular formula: 2(C)2(H)2(O) = C4H4O2, giving the molecular formula as C4H4O2.
What is the molecular formula of a compound with an empirical formula of CH?
The molecular formula of a compound with an empirical formula of CH is likely to be CH, as there is only one carbon atom and one hydrogen atom in the empirical formula. In this case, the empirical formula is also the molecular formula.
What is empirical formula for C4H8?
CH2 is the empirical formula for C4H8 because it is an alkene and the empirical fomula for ALL alkenes are C(n)H(2n) n being the number of molecules!!! (^-^)
Calculate the empirical formula of a compound formed from 3 percent C 0.3 percent H and 96.7 percent you Which formula below correctly represents the empirical formula?
Chi a+
Can any one substance have the same empirical formula and molecular formula?
Yes, a substance can have the same empirical formula and molecular formula if it consists of the simplest whole number ratio of its elements, and that ratio also represents the actual number of atoms in a molecule. This occurs in compounds like water (H₂O), where the empirical formula (H₂O) and the molecular formula (also H₂O) are identical. However, this is not the case for substances with larger molecular structures, where the empirical formula would typically represent a reduced ratio of atoms compared to the molecular formula.
What is a molecular formula 264g with a empirical formula of C3H4O3?
To determine the molecular formula from the empirical formula (C₃H₄O₃) and the given molar mass (264 g), first, calculate the molar mass of the empirical formula: C (12.01 g/mol) × 3 + H (1.01 g/mol) × 4 + O (16.00 g/mol) × 3 = 88.11 g/mol. Next, divide the given molar mass by the empirical formula mass: 264 g / 88.11 g/mol ≈ 3. This means the molecular formula is three times the empirical formula, resulting in C₉H₁₂O₉.
Calculate the empirical formula of a compound formed from 3 percent c 3 percent h and 96 7 percent you which formula below correctly represents the empirical formula?
CHI3
What is an empirical formula c4h8 c2h4 ch c2h2?
CH2 is the empirical formula for C4H8 because it is an alkene and the empirical fomula for ALL alkenes are C(n)H(2n) n being the number of molecules!!! (^-^)
How are the empirical and molecule formulas for a compound related?
The empirical formula of a compound represents the simplest whole-number ratio of the elements present, while the molecular formula indicates the actual number of atoms of each element in a molecule of the compound. The molecular formula can be a multiple of the empirical formula, meaning that it may contain the same elements in a proportion that is a whole number multiple of the empirical ratio. For example, if the empirical formula is CH₂, the molecular formula could be C₂H₄, C₃H₆, etc., depending on the actual number of atoms in the molecule.
A compound contains 21.2%N 6.1%H 24.2% and 48.5%O What is it’s empirical formula?
The empirical formula of a compound that consists of 21.2%N, 6.1%H, 24.2% S and 48.5% O is N2H8SO4.
Different molecules with the same empirical formula?
Empirical formulaCompoundMolecularformulaCH (92.2% C; 7.8% H)acetyleneC2H2benzeneC6H6CH2 (85.6% C; 14.4% H)ethyleneC2H4buteneC4H8CH2O (40.0% C; 6.7% H;53.3% O)formaldehydeCH2Oacetic acidC2H4OglyceraldehydeC3H6O3The molecular formula may be a multiple of the empirical formula.
What is the empirical formula of a compound with the molecular formula C 12 H 8?
The empirical formula of a compound with the molecular formula C12H8 is CH2. This is determined by dividing the subscripts in the molecular formula by the greatest common factor (in this case, 4) to obtain the simplest whole-number ratio of atoms in the compound.
What is the empirical formula and molecular formula of a compound with a molar mass of 245.8g The composition is 19.53 C 2.44 H 13.02 O and 65.01 Br?
The molar mass of the empirical formula is calculated by summing up the molar masses of the elements in the given composition (which gives a molar mass of 281.6 g/mol). To find the empirical formula, divide the molar mass of the compound (245.8 g/mol) by the molar mass of the empirical formula (281.6 g/mol), which gives approximately 0.873. This means the empirical formula is BrC₆H₈O₃.
