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A particular natural gas consists, in mole percents, of 83.0% CH4 (methane), 11.2% C2H6 (ethane), and 5.80% C3H8 (propane). A 385-L sample of this gas, measured at 21C and 739 mmHg, is burned in an excess of oxygen gas.
CH4=-890.3C2H6=-1559.7C3H8=-2219.1kJ/mol
Use the octet rule to predict the formula of the simplest compound formed from hydrogen and selenium. Why
Calculate the millimoles of sodium hypochlorite used in the reaction: 2.3mL of a 5.25% solution (Clorox). Compare this value with the quantity of cyclohexanol to be used in the reaction. Would you describe the oxidant as being present in slight ex..
If 23mL of 6.4M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid.
An expanding gas does 150.0 J of work on its surroundings at a constant pressure of 1.01 atm. If the gas initially occupied 68.0 mL, what is the final volume of the gas.
What are some reasons why there would be a difference between the expected and actual values for the moles of copper oxide produced from heating copper in the air.
Crystalline potassium bromide has a rock salt structure and a density of 2.75 g/cm^3. Calculate its unit-cell edge length.
A 10.0cm long cylindrical glass tube, sealed at one end, is filled with ethanol. The mass of ethanol needed to fill the tube is found to be 11.48g . The density of ethanol is 0.789 g/mL.
Obtain expressions for the following partial derivatives for a diatomic ideal gas, assuming that its translational, rotational, and vibrational motions all behave classically.
Use the following balanced equation for the problem below: 2HCl + Na2CO3 = 2NaCl + CO2 + H2O If 35.0 gm of Na2CO3 is reacted with 18.0 gm of HCl, how many grams of CO2 are produced
the steam distillate contains a significant quantity of water, along with the cyclohexanone. how is the water removed from the steam distillate?
Because of porosity of the filter paper some of the CaC2O4*H2O precipitate passes through the filter paper. Will the reported percent of the limiting reactant in the original salt mixture be reported too high or too low
Calculate the enthalpy change (in J) when a 4.08 g sample of water at 26.4 °C and 1 atm is frozen to ice at -20.4°C and 1 atm.
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