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C8h18

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Q: What is the molecular formula of a compound with an empirical formula of C4H9 and a gram formula mass of 114 grams mole?

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C6h12o6

C3h3

The molecular formula is C3h6.

First, add together the atomic masses of the elements:C- 12.0H- 1.00_______13.0Now put it into the following formula:x(added atomic mass) = molecular weight13.0x = 26.0Then find xx= 2Take the x value and multiply it with the number of atoms in the empirical formula/C1H1 * 2 = C2H2The final answer is the actual molecular formula C2H2 or Acetylene

First find empirical formula by assuming you have 100 grams of the compound -85.6 grams of Carbon and 14.4 grams of Hydrogen Divide both these amounts by their mass per mole. Carbon: 85.6/12 = 7.13 Hydrogen: 14.4/1.008 = 14.28 Now divide the larger answer by the smaller answer. 14.28 divided by 7.13 to get a ratio of 2 H for every one Carbon in the empirical formula Empirical formula = CH2

Related questions

the answer is: P4O10

C6h12o6

C4O2H8

C3h3

This compound may be dioxane - C4H8O2.

Cannot answer this question without knowing the EMPIRICAL formula.

The gram formula unit mass of the empirical formula C2H3 is twice the gram atomic mass of carbon plus three times the gram atomic mass of hydrogen, or about 27. The nearest integer to 162.27/27 is 6. Therefore, the molecular formula for the compound is C12H18.

You can only calculate the empirical formula because you do not have a mass of this compound given. To do the empirical formula assume 100 grams and change percent to grams. Get moles. 80 grams Carbon (1 mole C/12.01 grams) = 6.66 moles C 20 grams hydrogen (1 mole H/1.008 grams) = 19.84 moles H the smallest becomes 1 in the empirical formula and the other number is divided by it, Thus; H/C 19.84 moles H/6.66 moles C = 2.9, which we call 3 so, CH3 --------------- is the empirical formula To get the molecular formula tour question needed to read; How to calculate molecular formula from such ans such mass of compound with these percentages of elements, Which, of course, your question did not provide. Then you would have divided that given mass by the mass total of the elements of the empirical formula, got a whole number by which you would have multiplied the numbers of your empirical formula to get molecular formula.

A molecular formula is the same as or a multiple of the empirical formula. The first step will be to assume exactly 100 grams of the substance, then convert each of these masses to moles,

We assume 100 grams and turn those percentages into grams and find moles of species. 40 grams carbon (1 mole C/12.01 grams) = 3.33 moles C 6.72 grams hydrogen (1 mole H/1.008 grams) = 6.67 moles H 53.28 grams oxygen (1 mole O/16 grams) = 3.33 The smallest mole number is 1, so we have two small numbers. Divide the large number by the small. 6.67/3/33 = 2 so.............. CH2O is the empirical formula. You did not state that you had a quantity of this compound ( such as 60 grams, or whatever ), so the molecular formula can not be found from this info. C6H12O6 is of course the molecular formula. To find the molecular formula you need a mass of the compound aside from the simple percentages. Then you find, as we have done, the empirical formula. you divide the mass given by the mass of the empirical formula and then take that quotient and multiply it times the empirical formula. In this case (CH2O) * 6 = C6H12O6, the molecular formula

The molecular formula is C3h6.

First, add together the atomic masses of the elements:C- 12.0H- 1.00_______13.0Now put it into the following formula:x(added atomic mass) = molecular weight13.0x = 26.0Then find xx= 2Take the x value and multiply it with the number of atoms in the empirical formula/C1H1 * 2 = C2H2The final answer is the actual molecular formula C2H2 or Acetylene

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