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A patient weighs 146 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25.0 mg of drug per mL of solution. How many mL of the drug should the patient receive? [Use: 1 pound = 454 g]
Discuss two ways that ammonium compounds decompose when they are heated. What chemical reaction is involved in the thermal decomposition of ammonium persulfate?
The barometric pressure in a cavern was measured using a mercury barometer. A value of 74.2 cm of Hg was obtained. How many atmospheres is this
Consider a gas at 1.00 atm in a 5.00 L container at 20 degrees celsius. What pressure does the gas exert when transferred to a volume of 2.77 L at 43 degrees celsius?
What is the concentration of the Pb(NO3)2 in the voltaic cell pictured above when Ecell=0.524V at room temperature?
The last step in the uranium decay series is Po-210 going to Pb-206 plus the emission of an alpha particle. Listed are the masses of the involved items: Po-210: 209.9829 AMU Pb-206: 205.9745 AMU alpha: 4.00260 AMU Find the energy in Joules release..
How many moecules of N2 are needed to react with 30 molecules of H2?
The entry of Na+ provides a free-energy input of 10.8 kJ/mol under typical cellular conditions (external [Na+] = 143 mM, internal [Na+] =14 mM and a membrane potential = -50 mV). What is the ratio of glucose concentration outside and inside cells?
The volume of a gas is 2.50 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume is changed to 9.41 L
If a pure R isomer has a specific rotation of -120.0 degrees, and a sample contains 81.0% of the R isomer and 19% of its enantiomer, what is the observed specific rotation of the mixture
A sample of 1.0 mole of a perfect gas with cp= 20.8 J K-1 is initially at 3.25 atm and 310K. If it undergoes reversible adiabatic expansion until its pressure reaches 2.50 atm. Calculate the final volume and temperature and the work done.
(b) calculate the moles of each gas before the reaction (c) determine the limiting reactant (d) calculate the moles of ammonia produced (e) calculate the partial pressures of all species in the system (f) the total pressure in the system
Using your mean experimental value of R =20 ,and of n= 1.00, calcuate the molar volume of your H2 at STP (standar T=273 K,P= 760mm Hg),using the ideal gas law
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