What is the molecular formula of a material for which complete combustion of a unknown mass gives #3.38*g# of #CO_2(g)#, and #0.69*g# of water. An #11.6*g# mass of this gas gives a volume of #10.0*L# at #0# #""^@C# of #10*L#?
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The ideal gas equation is the only foundation upon which we can examine the molecular formula. The combustion data you provided were not kosher; neither the mass of the combusted gas nor the water content of the combustions were disclosed.
OR
Nevertheless, I don't believe you have addressed all the relevant information in this query.
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The molecular formula is
This problem relates to the empirical formula/molecular formula.
I take it that you intended 0.69 grams of water.
Determine the molar ratios (c).
I like to compile the calculations into a table from this point on.
(d) Determine the gas's molar mass.
Since you don't specify the gas's temperature or pressure, I'll assume STP (1 bar and 0 °C).
(d) Determine the gas's formula.
The gas has a molecular mass of 26.3 u.
An integral multiple of the empirical formula mass is required for the molecular mass.
The empirical formula must be doubled in the molecular formula.
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The molecular formula of the material can be determined using the given information and stoichiometry.
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Find the moles of CO2 and H2O produced:
- Moles of CO2 = 3.38 g / 44.01 g/mol
- Moles of H2O = 0.69 g / 18.015 g/mol
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Determine the limiting reactant:
- Calculate the moles of C and H in CO2 and H2O.
- The smaller value is the limiting reactant.
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Calculate the moles of the unknown material:
- Use the moles of the limiting reactant and the stoichiometry of the reaction.
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Find the molecular formula:
- Divide the molar mass of the unknown material by the molar mass calculated in step 3 to find the molecular formula ratio.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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