If 1.80 g of a compound containing only Carbon and hydrogen occupies 1.4 L at 0.00°C and 775 mm Hg, what is the molecular formula of the compound?
A) CH4
B) C2H6
C) C2H4
D) C2H2
E) C3H6
molecular formula of the compound is C2H4
If 1.80 g of a compound containing only Carbon and hydrogen occupies 1.4 L at 0.00°C...
Please solve When 0.125 g of propane, a compound containing carbon and hydrogen only is reacted with excess oxygen, 0.375 g of CO_2 and 0.205 g of H2O are formed. The empirical formula of is: C4H10 C5H12 C2H6 C3H8 CH4
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 scientist decides to determine the molecular formula of a compound containing only carbon and hydrogen. The compound is first analyzed by combustion analysis. 2.257 g of the compound was found to produce 4.21 L of carbon dioxide gas at 1.0 bar, 298.15 K, and 1.92 g of water. Determine the empirical formula. The molecular formula is determined using data from the combustion analysis and the Dumas method. Given the Dumas method data below, determine the molecular formula of the...
3.A sample of a pure gas at 20 °C and 670 mm Hg occupies a volume of 562 cm3. How many moles of gas are in this sample? 4.An unknown compound contains only carbon and hydrogen. What is the volume (in L) of 1 mol of this gas at 100 °C and 760 mm Hg? 5.The same 1 mol sample of gas from the previous problem has a vapor density of 2.550 g/L. If the empirical formula of the compound...
Upon combustion, an unknown compound containing only carbon and hydrogen produces 40.29 g carbon dioxide and 16.49 g water. Determine the empirical formula of the unknown compound.
Combustion of an unknown compound containing only carbon and hydrogen produces 54.9 g of CO₂ and 45.1 g of H₂O. What is the empirical formula of the compound?
Combustion of a 1.025 g sample of a compound containing only carbon, hydrogen and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical and molecular formulas of the sample compound, if its molecular weight has been roughly determined to be 363 g/mol by mass spectrometer?
Determine the empirical formula of a compound containing 79.85% carbon, and 20.15% hydrogen. A. None of these choices is correct B. (CH2)n C. (CH3)n D. (CH4)n E. (CH)n
a combustion analysis of a 0.2104 g hydrocarbon sample (containing only hydrogen and carbon) yielded 0.6373 g carbon dioxide and 0.3259 g water. A separate experiment determined that the molecular weight of this compound is 58.7 g mol-1. from this data, determine both emperical and the molecular formula of this substance.
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the compound produced 61.024 g of CO2 and 24.981 g of H2O, what is the empirical formula of the compound? 2.)) If the molar mass of this compound is 72.1 g/mol, what is the molecular formula?