Moles of Carbon dioxide ( CO2 ) = weight in gm / molar mass = 88 gm / 44 gm mol—1 = 2 mol
moles of H2O = 27 gm / 18 gm mol—1 = 1.5 mol
moles of carbon = moles of CO2 = 2mol
moles of Hydrogen = 2 x moles of H2O = 2 x 1.5 = 3 mol
C atoms = 2
H atoms = 3
Fill in the Blanks A 27.0 g sample of an unknown hydrocarbon was burned in excess...
A sample of 1.200 g of vitamin C is burned in the presence of excess of oxygen to yield 1.799 g of carbon dioxide and 0.491 g of water. Vitamin C contains only carbon, hydrogen, and oxygen 1) a) Calculate the mass percent composition of vitamin C b) Determine the empirical formula of vitamin C 2) Burning a 0.1500 g sample of a carbon-hydrogen-oxygen g CO2 and 0.1500 g H20. Show all work. compound in oxygen forms a) Calculate the...
1. A sample of a hydrocarbon weighing 4.99 grams was burned completely in excess oxygen, and 15.00 grams of carbon dioxide were obtained. What is the empirical formula of the compound? CHs CH4 О сн C3Hs
16. A 2.288 g sample of a hydrocarbon consisting of only carbon and hydrogen(NO oxygen burned in an excess of oxygen gas (O2), producing 6.277 g CO2 and 5.139 g H20. What is the empirical formula of the hydrocarbon? (5 points) (FW CO2 = 44.01; H2O = 18.02; H = 1.01; C =12.01: 0 = 16.00; O2 = 32.00)
2) A 1.000 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The mass of the carbon dioxide was 3.385 g, and the mass of the water was 0.692 g. What was the empirical formula of the hydrocarbon? A. C5H12 B. CsH6 C. CįH6 D. C H2 E. CįH star 1.00
solve the two questions 1. Vanillin, a flavoring agent, is made up of carbon, hydrogen, and oxygen atoms. When a sample of vanillin weighing 2.500g burns in oxygen, 5.79 g of carbon dioxide and 1. 18 g of water are obtained. What is the empirical formula of this compound? 5.79 Co Hoe 27.0% & 0.13 0.065 6.112 It, O2 wilker mass (inpuu 2- A 0.250 g sample of hydrocarbon undergoes complete combustion to produce 0.845 g of CO, and 0.173...
Under STP conditions, 100.0 mL of an unknown hydrocarbon gas was combusted in excess oxygen. The only products of the combustion were 300.0 mL of carbon dioxide and 400.0 mL of water vapor. a. What are the intermolecular forces common to hydrocarbon gases? b. Does the behavior of these gases tend to resemble ideal gas behavior? How might these gases be expected to deviate from this behavior? c. How many moles of carbon dioxide are produced in the combustion? d....
Methyl salicylate is a common "active ingredient" in liniments such as Ben-GayTM. It is also known as oil of wintergreen. It is made up of carbon, hydrogen, and oxygen atoms. When a sample of methyl salicylate weighing 5.384 g is burned in excess oxygen, 12.46 g of carbon dioxide and 2.571 g of water are formed. What is the simplest formula for oil of wintergreen? (Enter the elements in the order: C, H, O.) What is the empirical formula?
itm5 ; Combustion of 6.650 mg of an unknown sample yielded 6.648 mg water, and 16.24 mg carbon dioxide. Data analysis found that the sample was only composed of carbon, hydrogen, and oxygen. Part A How many moles of carbon were in the original compound? Part B How many moles of hydrogen were in the original compound? Part C Give the empirical formula of the unknown sample.
23. An important intermediate reaction in the industrial production process of nitric acid is shown. What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? NH3(g) + O2(g) → NO(g) + H2O (1) 24. A 10.00 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The...
6.0 grams hydrocarbon sample were made to react with oxygen gas to produce 17.6 grams of carbon dioxide according to the equation: CxHy(g) + O2(g) ---------- CO2(g) + H20(l) where x = subscript for C, y = subscript for H a. How many grams of C are there in 17.6 grams of CO2? b. How many grams of C are there in the hydrocarbon sample? c. How many moles of C are there in the hydrocarbon sample? d. How many...