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To calculate the formula mass of C4H9OH (butanol), you need to sum the atomic masses of each element in the molecule. The formula consists of 4 carbon (C) atoms, 10 hydrogen (H) atoms, and 1 oxygen (O) atom. Using approximate atomic masses (C = 12.01 g/mol, H = 1.01 g/mol, O = 16.00 g/mol), the formula mass is calculated as follows: (4 × 12.01) + (10 × 1.01) + (1 × 16.00) = 58.12 g/mol. Thus, the formula mass of C4H9OH is approximately 74.12 g/mol.
What else can I help you with?
What is the mole ratio of O2 to C4H9OH?
To determine the mole ratio of O2 to C4H9OH, we need to look at the balanced chemical equation for the combustion of butanol (C4H9OH). The balanced equation is: [ C4H9OH + 6 O2 \rightarrow 4 CO2 + 5 H2O. ] From the equation, the mole ratio of O2 to C4H9OH is 6:1. Thus, for every mole of butanol, six moles of oxygen are required.
What is the formula for butanone?
The chemical formula for butanone is C4H8O. It is a ketone compound with a four-carbon chain and a ketone functional group.
What is the molar mass of 1-butanoic acid?
The molecular formula of 1-butanol is C4H9OH so the molar mass is: (12)(4)+(1)(9)+(16)(1)+(1)(1)= 74
How many times heavier is the molar mass than the empirical formula mass?
The molar mass of a compound is typically a multiple of its empirical formula mass, depending on the molecular formula. To determine how many times heavier the molar mass is than the empirical formula mass, you can divide the molar mass by the empirical formula mass. This ratio will yield a whole number that represents how many times the empirical formula fits into the molecular formula. For example, if the molar mass is 60 g/mol and the empirical formula mass is 15 g/mol, then the molar mass is 4 times heavier than the empirical formula mass.
What is the formula of the formula mass?
Mass = weight /gravity Density = Mass / Volume So, if you know the density and the volume, you can calculate the mass. Also, you can measure the mass by measuring the weight. On earth, mass and weight are equal.
What is C4H9OH?
C4H9OH is the chemical formula for butanol, which is an alcohol isomer that can exist in four different forms: n-butanol, sec-butanol, isobutanol, and tert-butanol. They are commonly used as solvents, fuel additives, and in organic synthesis.
What is the mole ratio of O2 to C4H9OH?
To determine the mole ratio of O2 to C4H9OH, we need to look at the balanced chemical equation for the combustion of butanol (C4H9OH). The balanced equation is: [ C4H9OH + 6 O2 \rightarrow 4 CO2 + 5 H2O. ] From the equation, the mole ratio of O2 to C4H9OH is 6:1. Thus, for every mole of butanol, six moles of oxygen are required.
Is c4h9oh amphoteric?
Yes, c4h9oh (butanol) is amphoteric, meaning it can act as both an acid and a base in chemical reactions.
What is the structural formula of a butanol molecule?
Assuming you want the structural formula of 'Butan-1-ol' it is CH3CH3CH3CH2OH
What is the balance equation for the complete combustion of 1-butanol?
C4H9OH + O2 → CO2 + H2O (Unbalanced)C4H9OH + 6O2 → 4CO2 + 5H2O (Balanced)The 'balanced' equation above is not correct, however the one below is!2C4H9OH + 12O2 → 8CO2 + 10H2O
What compound is an isomer of C4H9OH?
One isomer of C4H9OH is butanol. There are four isomers of butanol: n-butanol, sec-butanol, isobutanol, and tert-butanol.
What is the formula for butanone?
The chemical formula for butanone is C4H8O. It is a ketone compound with a four-carbon chain and a ketone functional group.
What is the molecular formula of methylpropane?
Ch3ch3cclch3
What is the molar mass of 1-butanoic acid?
The molecular formula of 1-butanol is C4H9OH so the molar mass is: (12)(4)+(1)(9)+(16)(1)+(1)(1)= 74
How many times heavier is the molar mass than the empirical formula mass?
The molar mass of a compound is typically a multiple of its empirical formula mass, depending on the molecular formula. To determine how many times heavier the molar mass is than the empirical formula mass, you can divide the molar mass by the empirical formula mass. This ratio will yield a whole number that represents how many times the empirical formula fits into the molecular formula. For example, if the molar mass is 60 g/mol and the empirical formula mass is 15 g/mol, then the molar mass is 4 times heavier than the empirical formula mass.
What is formula for mass?
There is no formula for mass. it is simply the weight measured in grams
What formula will be use to get average atomic mass on an isotopes?
mass formula
