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As an employee in a pediatrician's office, you are asked to prepare a half-page information sheet for parents to teach children how to obtain a clean catch urine sample for bacteriologic culture. One set of instructions is needed for girls and another set of instructions for circumcised boys and a third set for uncircumcised boys.
when heated, sulfuric acid will decompose into sulfur trioxide and water
Why does tellurium have an endothermic electron affinity. In other words, why would it take energy to add an electron to it
student placed 18.5 of glucose in a volumetric flask added enough water to dissolve the glucose by swirling then
There were two "oil shocks" in the seventies, one in 1973 and another in 1979. Explain what caused the shocks and what effect it had on the American public and economy. Please suggest a realistic way our country can save ourselves from this type..
how many grams of methanol must be added to 7.50 kg of water to lower its freezing point to -13.0 degrees c? for each
Explain Cyclopentadiene reacts as a diene in the the Diels-Alder reaction a great deal faster than does 1,3 butadiene.
at 900K the following reaction has kp=.345: 2SO2(g)+O2(g)-->2SO3(g) Partial pressures of SO2 is .150 and of O2 is .455. What is the equilibrium partial pressure of SO3?
The specific heat capacity of a certain monatomic solid is 0.392J*k^-1*g^-1. The chloride of this element (XCl2) is 52% chlorine by mass.
A student heated 1.0L of ethanol (density 0.789 g/L) with 1.0 mL ethanoic acid (density 1.049 g/mL) with a sulfiric acid catalyst and noticed a vinegar-like smell to the product as well as a fruity medicinal smell.
The air pollutant NO is produced in automobile engines because of the high-temperature reaction below. If the initial concentrations of N2 and O2 at 1000 K are both 1 M, what are the concentrations of NO, N2, and O2
A student adds an excess (more than she needs to react completely) of solid sodium hydrogen carbonate to a beaker containing exactly 675 mL of 0.220M coper(II)nitrate aqueous solution.
When 1.269 g of this compound (molar mass = 103.67 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.029 °C. What is the heat capacity (calorimeter constant) of the calorimeter
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