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CH_2O The empirical formula is the simplest whole number ratio defining constituent atoms in a species. In all of these problems it is useful to assume 100 g of compund, and calculate the ATOMIC composition. So, in 100*g fructose, there are: (40.00*g)/(12.01*g*mol^-1) = 3.33*mol*C, (6.72*g)/(1.00794*g*mol^-1) = 6.66*mol*H, (53.29*g)/(15.999*g*mol^-1) = 3.33*mol*O, If we divide thru by the ...
Look up the molar mass of fructose, calculate the number of moles, and then divide by 0.15 kg of #"H"_2"O"# (since that is the solvent). Fructose does not dissociate so #i=1#. Once you have calculated #DeltaTb#, you can calculate the new boiling point to be. #T_b = 100 + DeltaTb#
You start by determining the empirical formula for the compound. Determine the mass in grams of each element in the sample. If you are given percent composition, you can directly convert the percentage of each element to grams. For example, a molecule has a molecular weight of 180.18 g/mol. It is found to contain 40.00% carbon, 6.72% hydrogen and 53.28% oxygen. Convert the percentages to grams ...
The molecular formula is "C"_6"H"_12"O"_6". This is the molecular formula for 6-carbon monosaccharides, such as glucose, fructose, and galactose. We first need to find the empirical formula, which represents the smallest whole number ratio of elements in the compound. After we determine the empirical formula, we determine the empirical molar mass. If the empirical molar mass is the same as the ...
What is the change in vapor pressure when 73.40 g fructose, C6H12O6, are added to 180.5 g water (H2O) at 298 K (vapor pressure of pure water at 298 K = 3.1690 kPa, molar mass of fructose = 180.156 g/mol, molar mass of water = 18.02 g/mol)?
Percent concentration by mass is defined as the mass of solute divided by the total mass of the solution and multiplied by 100%. So, c% = msolute msolution ⋅ 100%, where. msolution = msolvent + msolute. There are two ways to change a solution's concentration by mass. Adding more solute - making the solution more concentrated;
A compound that contains only nitrogen and oxygen is 30.4% N by mass; the molar mass of the compound is 92 g/mol. What is the empirical formula and the molecular formula of the compound? A sample of a compound containing the elements silver, carbon, and oxygen, has a mass of #"1.372 g"#.
-3.7^@"C" Your strategy here will be to determine the van't Hoff factor for sodium iodide, "NaI" calculate the molality of the solution calculate the freezing-point depression of the solution The idea is that the freezing point of a solution is lower than the freezing point of the pure solvent, which for water is 0^@"C" at normal pressure.
Approximately 60 \\ "g of" \\ C_6H_12O_6. We have the balanced equation (without state symbols): 6H_2O+6CO_2->C_6H_12O_6+6O_2 So, we would need six moles of carbon dioxide to fully produce one mole of glucose. Here, we got 88 \\ "g" of carbon dioxide, and we need to convert it into moles. Carbon dioxide has a molar mass of 44 \\ "g/mol". So here, there exist (88color(red)cancelcolor(black)"g ...
How many grams of fructose (#C_6H_12O_6#) must be dissolved in 882g of 12 acetic acid to raise the boiling point by 7.4°C?