A 0.4647 g sample containing only carbon, hydrogen, and oxygen was burned to yield 0.8635 g...
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Balance each of the following chemical equations shown below: NH_ + HCl rightarrow NH_4Cl C_ H_ + O_2 rightarrow CO_2 rightarrow H_2O Sb + Cl_2 rightarrow SbCl_2 NI_3 rightarrow N_2 rightarrow I_2 Al_2(SO_)_2 + NaOH rightarrow Na_2SO_4 + Al(OH)_3
An organic compound consists only carbon (c), hydrogen (H) and oxygen (O). Elemental analysis of a sample of this compound weighting 0.20000 g shows that it contains 0.09232 g C and 0.00930 g H. The empirical formula of this compound is: a. C_5H_6O b. C_5H_6O_2 c. C_5H_6O_3 d. C_5H_6O_4 e. C_6H_6O f. C_6H_6O_2 g. C_6H_6O_3 h. C_6H_6O_4 i. None of the above; the correct ionic formula is ______. The amount of carbon dioxide (CO_2) formed upon burning 1894 g of...
Match the definition with the term ____ Transition from solid to liquid A. condensation ____ Transition from liquid to gas B. Boiling ____ Transition from solid to gas C. Freezing _____ Transition from gas to liquid D. Melting _____ Transition from liquid to solid E. Sublimation How many milligrams are in 8.22 moles of sodium hydroxide (molar mass = 39.997 g/mol). Be sure to show your work, correctly label your units and use the correct number of significant figures. A...
25. When 3.62 g of a compound containing carbon, hydrogen, and oxygen were burned completely in air, 5.19 g of Co, and 2.83 g of H2O were produced. What is the empirical formula of the compound?
A 0.158 g sample of a compound containing the elements carbon, hydrogen, oxygen, and sulphur was burned completely, yielding 0.110 g CO2 and 0.0677 g H2O. In a separate experiment, all the sulphur in another 0.158 g sample was converted to 0.292 g of BaSO4. What is the empirical formula of the unknown compound?
16. A 2.288 g sample of a hydrocarbon consisting of only carbon and hydrogen(NO oxygen burned in an excess of oxygen gas (O2), producing 6.277 g CO2 and 5.139 g H20. What is the empirical formula of the hydrocarbon? (5 points) (FW CO2 = 44.01; H2O = 18.02; H = 1.01; C =12.01: 0 = 16.00; O2 = 32.00)
A 1.0422 g sample of powdered aluminum is burned in a constant volume bomb calorimeter containing excess oxygen to form Al_2 O_3 (s) The calorimeter has a heat capacity of 8.775 kJ degree C^-1. The temperature of the calorimeter increases by 3.680 degree C. Determine the molar internal energy of combustion delta U and the molar enthalpy of combustion delta H for aluminum at 25 degree C. 4 Al (s) + 3 O_2 (g) middot 2 Al_2 O_3 (s)
For the following questions answer in the space provided: a. Balance the following equation: B_2 O_3 (s) + HF (l) rightarrow BF_3 (g) + H_2 O (l) b. Identify the oxidizing and reducing agent in the chemical reaction C d + Ni O_2 + 2H_2 O rightarrow Cd (OH)_2 + Ni (OH)_2 c. Calculate the density of carbon dioxide, CO_2 (g), at 100 degree C and 10.0 atm pressure
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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
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?