Element | mass | mole | simpest ratio | |||
Carbon | 15.87 | 15.87/12 =1.32 |
1.32/1.32 = 1 |
|||
Hydrogen | 2.22 | 2.22/1 => 2.22 |
2.22/1.32 = 1.68 |
|||
Nitrogen | 18.50 | 18.5/14 => 1.32 | 1.32/1.32 = 1 | |||
Oxygen | 63.41 | 63.41/16 = 3.96 | 3.96/1.32 = 3 |
C :. H : O : N
1: 1.68 : 3: 1
3 : 5 : 9. : 3
Empirical formula = C3H5N3O9
B) balanced chemical reaction
4C3H5N3O9 -----> 12CO2 + 6N2 + O2 + 10 H2O
The detonation (decomposition) of nitroglycerin produces the following carbon dioxide, nitrogen, oxygen and water vapor gases....
A hydrocarbon undergoes combustion analysis, and 4.40 g carbon dioxide and 2.70 g water vapor is obtained. What is the empirical formula of the hydrocarbon? (5 points) What is the difference between an empirical and molecular formula, including an example? (2 points)
Suppose a substance has been prepared that is composed of carbon, hydrogen and nitrogen. When 0.1156 gram of this compound is reacted with oxygen, 0.1638 gram of carbon dioxide (CO2) and 0.1676 gram of water (H2O) are collected. If all the carbon in the compound is converted to CO2 Determine the mass of Carbon and Hydrogen in the sample. Calculate the percentage composition of Carbon, Nitrogen and Hydrogen in the substance. Calculate the mass of nitrogen in the substance. Calculate...
Suppose a substance has been prepared that is composed of carbon, hydrogen and nitrogen. When 0.1156 gram of this compound is reacted with oxygen, 0.1638 gram of carbon dioxide (CO2) and 0.1676 gram of water (H2O) are collected. If all the carbon in the compound is converted to CO2 Determine the mass of Carbon and Hydrogen in the sample. Calculate the percentage composition of Carbon, Nitrogen and Hydrogen in the substance. Calculate the mass of nitrogen in the substance. Calculate...
Part II : Volume - Volume 1. Carbon monoxide burns in oxygen to form carbon dioxide. What volume of oxygen at 25°C and 760. mm Hg is required to react with 15.0 L of carbon monoxide (at STP)? 2. What volume of hydrogen and nitrogen are required to produce 20.0 L of ammonia (all gases at STP)? 3. Acetylene ( CH) burns in oxygen to form carbon dioxide and water. How many liters of oxygen (at STP) are needed to...
5. Compound X contains only carbon, nitrogen, hydrogen, oxygen and sulfur. Analysis experiments produced the following results: 1. 2.52 g of X burned in excess O2 produces 4.25 g of carbon dioxide and 1.02 g of water at 100% yield. 2. 4.14 g orx reacts to produce 1.785 g of sulfur trioxide at 85% yield. 3. 5.66 g orx reacts to produce 1.68 g of nitric acid at 75% yield. What is the empirical formula of compound X?
Baker’s yeast catalyzes the decomposition of hydrogen peroxide (dihydrogen dioxide) into oxygen and water. Directions: Add 10 mL of hydrogen peroxide to an Erlenmeyer flask. Add a few grains of yeast and watch the reaction. hydrogen peroxide- H2O2 yeast-? please write the unbalanced and balanced chemical equation
Bonus Question (20 points). Nitrogen dioxide gas reacts with water vapor to produce oxygen and ammonia gases. Suppose that 12.8 g of nitrogen dioxide gas reacts with 5.00 L of water vapor 375 °C and 725 tor? how many moles of nitrogen dioxide gas are there initially? b. how many moles of water vapor are there initially? e Balance the chemical reaction. Complete the following table after solving and NO + H2O - O d. What is the limiting reagent?...
13. The composition of Earth's atmosphere by volume is nitrogen, oxygen, 0.93% argon, 0.039% carbon dioxide, around 1% water vapor, and small amounts of other gases. a. 78%; 21% d. 49%; 49% b. 68%; 31% c22%; 77% c. 88%; 11%
MHE Reader Propane, C3Hs(&), reacts with oxygen gas to produce carbon dioxide gas and water vapor. a) b) 2. Write a balanced equation including states of matter for the reaction. If 4.55 g of propane reacts with excess oxygen under standard conditions, calculate the theoretical yields (in grams) for both carbon dioxide and water, and · the total amount of heat released/absorbed when the reaction is complete. c) Ethanol is currently being used as a replenishable fuel alternative/supplement because it...
The combustion of glucose (C6H120.) with oxygen gas produces carbon dioxide and water. This process releases 2.387 kJ per mole of glucose. When 3.348 mol of oxygen react in this way with glucose, what is the energy released in Calories (big C calories). Input your answer as a number without units lint: write a balanced equation for the combustion process)