A compound is found to contain 37.23 % carbon, 7.827 % hydrogen, and 54.94 % chlorine...

A compound is found to contain 37.23 % carbon, 7.827 % hydrogen, and 54.94 % chlorine by mass. What is the empirical formula for this compound? To answer the question, enter the elements in the order presented above.

Thank You!!

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A gaseous hydrogen and carbon containing compound is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass.

A gaseous hydrogen and carbon containing compound is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass. The mass of 158 mL of the gas, measured at 556 mmHg and 25 °C, was found to be 0.275 g. What is the molecular formula of the compound?

6a. A compound is analyzed and is found to be composed of 36.93% carbon, 4.65% hydrogen,...

6a. A compound is analyzed and is found to be composed of 36.93% carbon, 4.65% hydrogen, and 58.42% fluorine. What is the empirical formula of this compound? (10 pts) 6b. If the molar mass of the compound described above is approximately195 g/mol, what is the molecular formula of the compound? (2 pts)

A certain volatile hydrocarbon (a binary compound of carbon and hydrogen) is found to be 92.3%...

A certain volatile hydrocarbon (a binary compound of carbon and hydrogen) is found to be 92.3% carbon by mass. In a seperate experiment, utilizing the Dumas method, a 4.00 mL pure liquid sample of this hydrocarbon is vaporized in a 125 mL Florence flask when the barometric pressure is 768.0 torr. After the exess gas escapes the temperature is measures as 98.0 C. The flask and contents are subsequenlty cooled to 25 C (densitry water at 25 C = 0.997044...

A compound containing only carbon and hydrogen is found to have an empirical formula with molar...

A compound containing only carbon and hydrogen is found to have an empirical formula with molar mass of 13. 0 g/mol. The compound 1. cannot be either C2H2 or C6H6 2. could be C6H6 but no C2H2 3. could be C2H2 , but not C6H6 4. could be C2H2 or C6H6 A compound containing only carbon and hydrogen is found to have an empirical formula with molar mass of 13. 0 g/mol. The compound 1. cannot be either C2H2 or...

A yellow substance was found to contain 54.5% Carbon, 9.10% Hydrogen and 34.6% Oxygen by mass....

A yellow substance was found to contain 54.5% Carbon, 9.10% Hydrogen and 34.6% Oxygen by mass. What is the molecular and empirical formula for the compound if it has a molar mass of approximately 135g/mole?

A compound containing only carbon and hydrogen has a carbon-to-hydrogen mass ration of 11.89. Which carbon-to-hydrogen...

A compound containing only carbon and hydrogen has a carbon-to-hydrogen mass ration of 11.89. Which carbon-to-hydrogen mass ratio is possible for another compound composed only of carbon and hydrogen? a) 2.50 b) 3.97 c) 4.66 d) 7.89 Why is the answer b?

A compound contains 0.643 grams hydrogen and 3.857 grams of carbon.

A compound contains 0.643 grams hydrogen and 3.857 grams of carbon. a) Find its empirical formula. b) Find its molecular formula if its molecular weight is 56.0 g/mol.

A compound contains only carbon, hydrogen, and oxygen. Combustion of 21.16 mg of the compound yields...

A compound contains only carbon, hydrogen, and oxygen. Combustion of 21.16 mg of the compound yields 48.04 mg of CO2 and 16.4 mg of H2O. The molecular weight of the compound is 114.1g/mole. What are the empirical and molecular formulas of the compound.

A compound contains only carbon, hydrogen, and oxygen. Combustion of 54.05 g of the compound yields...

A compound contains only carbon, hydrogen, and oxygen. Combustion of 54.05 g of the compound yields 79.22 g of CO2 and 32.43 g of H2O. The molar mass of the compound is 120.104 g/mol. *Each part of this problem should be submitted separately to avoid losing your work* 1. Calculate the grams of carbon (C) in 54.05 g of the compound: grams 2. Calculate the grams of hydrogen (H) in 54.05 g of the compound. grams 3. Calculate the grams of oxygen...

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157g of the compound produced...

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157g of the compound produced 0.213g CO2 and 0.0310g of H2O. In another experiment, 0.103g of the compound produced 0.0230g of NH3. What is the emerical formula of the compound? In a seperate experiment, the molar mass is found to be 454.3 g/mol. what is the molecular formula of the compound? hint: assume that all carbon ends up in CO2 and all hydrogen ends up in H2O.Also assume that...

Subjects