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1. A 1.0 L sample of a gaseous compound of hydrogen, carbon, and nitrogen gave upon combustion 2.0 L of CO2, 3.5 L of H2O vapor, and 0.50 L of N2 (with all gas volumes measured at the same T and P). What is the empirical formula of the compound?
2. A 6.01 g sample of a gaseous carbon-hydrogen compound is found to contain 4.80 g C and 1.21 g H. At STP, 762 mL of the gas has a mass of 1.02 g. What is the molecular formula of the compound?
3. An adult takes about 15 breathes per minute with each breath having a volume of 500 mL. If the air that is inhaled is dry, but exhaled at 1 atm is saturated with water vapor at 37°C, what is the mass of water lost from the body in one hour. The vapor pressure of water at 37°C is 47.1 torr.
A 4.50-g sample of LiCl at 25.0 C dissolves in 25.0 mL of water also at 25 C. The final equilibrium temperature of the resulting solution is 60.8 C.
Fears of radiation exposure from normal use of such detectors are largely unfounded. Identify reasons why ^241Am smoke detectors are perfectly safe.
If 29.1 mL of 0.4 M NaOH is used to reach the endpoint when titrating 20.1 mL of acetic acid, what is the concentration of the acetic acid in moles/L
The enthalpy of formation of compound X is -612 kJ/mol, and the sole product of its combustion has a enthalpy of formation of -671 kJ/mol. What is the enthalpy of combustion of compound X?
Suppose you have a sample of sodium weighing 11.62 g. How many atoms of sodium are present in the sample?
The thallium (present as Tl2SO4) in a 6.05-g pesticide sample was precipitated as thallium(I)iodide. Calculate the mass percent of Tl2SO4 in the sample if 0.235g of TlI was recovered.
In one episode of the 1960s television sitcom, Gilligan's Island, the famous professor constructed voltaic cells to use as substitues for their radio's dead batteries.
the complete combustion of 1.043g of C9H8O in a bomb calorimeter( Ccal= 3.986 kj/c) produced an increase in temperature of 12.85C. Calculate the molar enthalpy of combustion of C9H8O, in kJ/mol.
What is the theoretical yield of hydrazine, in grams, prepared from the reaction of 150.0mL of 1.01 M NH3 (aq) with 50.0 mL of 1.25 M NaOCl (aq)?
Describe and explain the possible effect on your results of the following experimental errors or variations. (a) You stopped the steam distillation after collecting 3 mL of distillate
the atomic masses of 6Li and 7 Li are 6.0151 amu and 7.0160 amu. Calculate the neutral abundance of each isotope. The average atomic mass of Li is 6.941 amu
calculate the moles of CO2 you would theoretically expect from 0.203 grams of an alka-seltzer tablet at 700. torr and 285. K.
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