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molecul Sumber of d with excess A gaseous compound of carbon, hydrogen and chlorine had the...
A gaseous compound of carbon, hydrogen and chlorine had the following composition: C = 24.78%; H...
A gaseous compound of carbon, hydrogen and chlorine had the following composition: C = 24.78%; H = 2.08 % and Cl = 73.14 %. A 1.26 g sample of this gas occupies a volume of 435 ml. at a pressure of 0.736 atm and temperature of 27°C. a) What is the empirical formula of the unknown gas (3 points) show all setup & work Answer: empirical formula = b) What is the molar mass of the unknow gas (3 points)...
omposition: C = 24.78%; H = 2.08 en and chlorine had the following composition: C =...
omposition: C = 24.78%; H = 2.08 en and chlorine had the following composition: C = 24.78% % and Cl = 73.14%. A 1.26 g sample of this gas occupies a volume of 292 mL at STP. a) What is the empirical formula of the unknown gas (3 points) show all setup & work Answer: empirical formula = b) What is the molar mass of the unknow gas (3 points) show all setup & work answer: molar mass = What...
a gaseous hydrogen and carbon containing compound is decomposed and found to contain 79.85% C and...
a gaseous hydrogen and carbon containing compound is decomposed and found to contain 79.85% C and 20.15% H by mass A.) What is the empirical formula of the compound? I already found the the empirical formula, its CH3 B.) at 43.0 °C and 0.984 atm, the gas occupies a volume of 1.8 L and has a mass of 2.04g. what is the molecular formula of the compound?
A 1.802 gram sample of unknown compound contains 0.721 grams of carbon, 0.121 grams of hydrogen...
A 1.802 gram sample of unknown compound contains 0.721 grams of carbon, 0.121 grams of hydrogen and 0.960 grams of oxygen. The compound has a molar mass of 180.2 g/mol. Determine the empirical formula of the compound and the molecular formula. Show all work.
CHAPTERS Practice Problems 6. An unknown gaseous hydrocarbon (compound composed of carbon and thydrogen only) conai...
CHAPTERS Practice Problems 6. An unknown gaseous hydrocarbon (compound composed of carbon and thydrogen only) conaists of 85.63% carbon by mass. A 0.335-g sample of the gas occupies a volume of 0.107 Lat STP (1 atm, oPC) What is the molecular formula of the gas7
A compound contains C, H, and Nonly. Analysis of a sample of the compound showed that...
A compound contains C, H, and Nonly. Analysis of a sample of the compound showed that it contained 38.6% C, 16.4% H and the rest Nitrogen. The molar mass of the compound is 62 g/mole. (A) What is the empirical formula of the compound? (B) What is the molecular formula of the compound? Show your setup and work, watch your sig figs. You must type your setup. work and result directly in the text answer box. BIV AA- IEE 3...
cyanidin a pigment found in many red berries, such as grapes, raspberries, and cranberries, contains carbon,...
cyanidin a pigment found in many red berries, such as grapes,
raspberries, and cranberries, contains carbon, hydrogen, and
oxygen. the complete combustion of a 0.80000g sample of this
compound in excess O2 produces 1.83856 g CO2 and 0.27604 g
H2O.
a) What is the empirical formula for cyanidin?
b) Given that the molar mass of cyanidin is 290 g/mol, what is
its molecular formula?
4. Cyanidin, a pigment found in many red berries, such as grapes, raspberries, and cranberries, contains...
A well-known toxic substance, composed of carbon, hydrogen, and nitrogen, was located nearby a student lying...
A well-known toxic substance, composed of carbon, hydrogen, and nitrogen, was located nearby a student lying unconscious in the laboratory. It is suspected that the student may have been poisoned by ingestion. 5.250-g of the suspect's compound was burned in pure oxygen to give 4.083-g of H20 and 14.242-g of CO2. (10 points) a) What is the empirical formula for the substance found near the student if it was the suspected nicotine compound? b) If the substance has a molar...
Part 2: Short Answer Directions: Answer each of the following questions. Be sure to use complete sentences where...
Part 2: Short Answer Directions: Answer each of the following questions. Be sure to use complete sentences where appropriate. For full credit be sure to show all of your work, UNITS and SF are important as well!!!1 balloon at a temperature of 35°C, how high can the temperature go (°C) before it will burst (5 1. A balloon will burst if the volume exceeds 4.57 L. If 2.96 L of helium are put into the points)? 2. A sample of...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got Mol-aria Why? Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. This is called Stoichiometry- (stoi-key-ah-meh-tree) Another way of looking at it is using the mole ratio from the balanced equation and information about one compound in the reaction to determine information about another compound in the equation. A mole ratio...
A gaseous compound of carbon, hydrogen and chlorine had the following composition: C = 24.78%; H = 2.08 % and Cl = 73.14 %. A 1.26 g sample of this gas occupies a volume of 435 ml. at a pressure of 0.736 atm and temperature of 27°C. a) What is the empirical formula of the unknown gas (3 points) show all setup & work Answer: empirical formula = b) What is the molar mass of the unknow gas (3 points)...
omposition: C = 24.78%; H = 2.08 en and chlorine had the following composition: C = 24.78% % and Cl = 73.14%. A 1.26 g sample of this gas occupies a volume of 292 mL at STP. a) What is the empirical formula of the unknown gas (3 points) show all setup & work Answer: empirical formula = b) What is the molar mass of the unknow gas (3 points) show all setup & work answer: molar mass = What...
CHAPTERS Practice Problems 6. An unknown gaseous hydrocarbon (compound composed of carbon and thydrogen only) conaists of 85.63% carbon by mass. A 0.335-g sample of the gas occupies a volume of 0.107 Lat STP (1 atm, oPC) What is the molecular formula of the gas7
A compound contains C, H, and Nonly. Analysis of a sample of the compound showed that it contained 38.6% C, 16.4% H and the rest Nitrogen. The molar mass of the compound is 62 g/mole. (A) What is the empirical formula of the compound? (B) What is the molecular formula of the compound? Show your setup and work, watch your sig figs. You must type your setup. work and result directly in the text answer box. BIV AA- IEE 3...
cyanidin a pigment found in many red berries, such as grapes,
raspberries, and cranberries, contains carbon, hydrogen, and
oxygen. the complete combustion of a 0.80000g sample of this
compound in excess O2 produces 1.83856 g CO2 and 0.27604 g
H2O.
a) What is the empirical formula for cyanidin?
b) Given that the molar mass of cyanidin is 290 g/mol, what is
its molecular formula?
4. Cyanidin, a pigment found in many red berries, such as grapes, raspberries, and cranberries, contains...
A well-known toxic substance, composed of carbon, hydrogen, and nitrogen, was located nearby a student lying unconscious in the laboratory. It is suspected that the student may have been poisoned by ingestion. 5.250-g of the suspect's compound was burned in pure oxygen to give 4.083-g of H20 and 14.242-g of CO2. (10 points) a) What is the empirical formula for the substance found near the student if it was the suspected nicotine compound? b) If the substance has a molar...
Part 2: Short Answer Directions: Answer each of the following questions. Be sure to use complete sentences where appropriate. For full credit be sure to show all of your work, UNITS and SF are important as well!!!1 balloon at a temperature of 35°C, how high can the temperature go (°C) before it will burst (5 1. A balloon will burst if the volume exceeds 4.57 L. If 2.96 L of helium are put into the points)? 2. A sample of...
POGIL-Stoichiometry How do chemists use balanced chemical equations? got bit D 23 mosquitoes? 10 He got Mol-aria Why? Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. This is called Stoichiometry- (stoi-key-ah-meh-tree) Another way of looking at it is using the mole ratio from the balanced equation and information about one compound in the reaction to determine information about another compound in the equation. A mole ratio...
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