A gaseous compound has the empirical formula CH2. Its density is 0.426 g/L at 0.465 atm and 373 K. What is the molecular formula of the gas? (R = 0.08206 L·atm/mol·K) A) C2H4 B) C3H6 C) C4H8 D) C5H10 E) C6H12
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A gaseous compound has the empirical formula CH2. Its density is 0.426 g/L at 0.465 atm...
The molecular formula of a compound having a molecular weight (56 g/mol) and an empirical formula CH2 is C4H8C3H6C2H2C10H20
An unknown gaseous hydrocarbon consists of 85.63% carbon by mass. A 0.100-g sample of the gas occupies a volume of 0.0533 L at STP. What is the identity of the gas? A. C4H8 B. C3H6 C. C2H4 D. C5H10 E. CH2
The empirical formula of a compound is known to be CH2, and its molar mass is 56 g/mol. What is the molecular formula of the compound? C3H20 C4H8 O C₂H4 CH2 O C₃H6
A hydrocarbon gas with the empirical formula CH2 has a density of 1.3 g/L. at 0 °C and 1.00 atm. A possible formula for the hydrocarbon is: CsH30 CH2 0 C₂H4 O Cato O Cato
Calculate the formula mass of a gas if 0.2091 g of the gas takes up 150.2 mL at 90.7 °C and 0.8 atm. Hint: Remember to convert mL to L and °C to K, R = 0.08206 L·atm/mol·K Hint: Answer includes 2 decimal places.
What is the molar mass of copper (II) sulfate, CuSO4? Select one: O A. 63.55.9 OB. 159.629 O C. 111.55 g D. 319.17 g O E. 16.00 9 An unknown compound is composed of the elements Nitrogen and Oxygen. The compound is analyzed and determined to be 30.45% and 69.55% 0. The molecular mass of the compound is found to be 02.01 g/mol. Determine the compound's molecuar formula and provide your answer below as Nxoy where x and y are...
. 0.275 L of solution is prepared by dissolving 2.50 g of an unknown molecular compound in enough water. The osmotic pressure of this solution is 1.98 atm at 27 °C. (R = 0.08206 L·atm/mol·K) a) Determine the molar mass of the molecular compound. (7 pts) b) If you need to prepare 0.275 L of AlCl3 solution with the same osmotic pressure of the above solution, what mass of AlCl3 (MW = 133.33 g/mol) would you need to weigh out?
A gaseous sample of a compound has a gas density of 0.647 g/L at 694 torr and 20 °C. What is the 4. molar mass of this compound? If this compound contains only nitrogen and hydrogen, and is 82.2% nitrogen by mass, what is its molecular formula? 5. What is the density in g/L of neon gas at STP?
A gaseous compound has a density of 1.32 g/L at 24.6 °C and 1.59 atm. What is the molar mass of the compound? Molar mass = _______ g/mol
A gaseous compound has a density of 1.60 g/L at 21.2 °C and 1.83 atm. What is the molar mass of the compound?