What mass, in g, of vitamin C is present in a sample containing 0.00002979 moles of vitamin C?
DATA: Vitamin C = C6H8O6 H = 1.01 g/mol C = 12.01 g/mol O = 16.00 g/mol
What mass, in g, of vitamin C is present in a sample containing 0.00002979 moles of...
Calculate the grams of ethane present in a sample containing 0.7080 moles if the molar mass of ethane is 30.067 g/mol.
please help A 1.470 g sample of an organic acid containing C, H and was combusted to determine the empirical formula. The combustion produced 3.810g of carbon dioxide (44,01 g/mol) and 1.820g of water(18.02 g/mol). Determine the number of moles of carbon in the compound, C- 12.01 g/mol H-1.01 g/mol 0-16.00 g/mol If 12.76 g of potassium phosphate reacts with excess lead(II) nitrate, a white precipitate of lead(11) phosphate forms in a solution of potassium nitrate. Write a balanced equation....
Nr of moles of C= mass of C/ molar mass of C Molar mass of C =12.o1 g= A In this case, A has measure unit in grams. But measure unit for A is Dalton or amu. Is the measure unit for A Dalton, amu, or grams? When I compute No of moles for carbon , I use A= 12.01 g, not A=12.01 amu. For exemple: for mass of C=24 g C Molar mass for: CO= A for C +A...
Strychnine is a poisonous alkaloid with a molecular formula of C21H22N2O2. What is the molar mass of strychnine (g/mol)? Give your answer to 4 significant figures. (Use C = 12.01 g/mol, H = 1.01 g/mol, N = 14.00 g/mol and O = 16.00 g/mol). Do not use scientific notation, do not include units in your answer, just write the number).
Ascorbic acid also known as Vitamin C, is an organic compound containing C, H and O. The combustion of a 28.1 g sample of ascorbic acid produces 42.1 g CO2 and 11.5 g H2O. Determine the empirical and molecular formula of ascorbic acid. The molar mass is 176 g/mol.
Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.81×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.81×10−4 mol of ascorbic acid. Express the mass in grams to three significant figures.
Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.85×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.85×10−4 mol of ascorbic acid. Express the mass in grams to three significant figures.
Series 100 contains carbon, hydrogen and oxygen, and has a molecular weight of 136 g/mol. In the combustion of a 5.000 g sample, 12.943 g of Co, and 2.655 g H2O were produced. From the above data, calculate the empirical and molecular formulas of your unknown sample. Use the following atomic weights: C = 12.01 H = 1.01 0 = 16.00 N = 14.01
Calculate the number of molecules present in each of the following samples. (a) 0.650 mol acetylene, C2H2, a fuel used in welding (b) How many molecules are in a snowflake containing 9.00 10-5 g of H2O (c) a 100. mg tablet of vitamin C, C6H8O6 NOTE THE UNITS OF mg. (d) how many ATOMS are in the vitamin C sample in part (c)? (d) how many ATOMS of oxygen are in the vitamin C sample in part (c)?
Need help with the following 1) Moles of I2 added & the moles vitamin C titrated 2) Grams of vitamin C in the sample & Grams of vitamin C in the tablet 3) The average g/tablet Trial 1 2song 10.4oolg rome loml T Part B: Vitamin C Tablet tablet strength mass tablet dilution volume volume titrated volumel, initial volume la final volumely added moles lz added moles vitamin C titrated g vitamin C in sample g vitamin C in tablet...