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A standard dextrose intravenous (IV) drip solution is 50.0% glucose by weight and has a density of 1.161 g/cm3. What is the mass of glucose in 250.0 mL of this solution?please be thorough in explaining each step.... I'm horrible at conversions
What is the rate constant of a first-order reaction that takes 367 seconds for the reactant concentration to drop to half of its initial value
The molar heat of fusion of tungsten is 33.7kJ/mol. What mass of tungsten can be melted by the addition of exactly 150cal at its melting point
a volume 505 mL of air on a cold winter day at -15 degrees celcius is breathed into the lungs, where body temperature is 37 degrees celcius
In the experiment you used a less amount of sulfuryl chloride than it is theoretically required for converting all the starting 1-chlorobutane to the dichlorinated products. Why
Draw the major organic product of the reaction. Indicate the stereochemistry via wedge/dash bonds, including explicit H and D atoms
At 25 C and 1.0 atm pressure, what is the minimum quantity of dry air needed to combust 1.1 L of CH4 (g) completely to CO2(g). Remember that oxygen is present in the atmosphere to the extent of 209480 parts per million.
when air pollution is highozone can reach .60 ppm. how many molecules of ozone are present per liter of polluted air if
S2- depicts the particle by placing atoms on the grid and connecting them with bonds. comprise all lone pairs of electrons and nonbonding electrons. Demonstrate the charge of the atom.
For a reaction of hydrogen with iodine, the rate constant is 2.45*10^-4 L mol-1 s-1 at 302 C and 0.950 L Mol-1 s-1 at 508 C.
Calculate the equilibrium constant (Keq) for the reaction of equimolar amounts of acetophenone and sodium hydroxide to generate the enolate.
consider the following reactionch4g 2 h2sg ----gt cs2g 4 h2ga reaction mixture initially contains 0.50 m ch4 and 0.75
At a certain temperature the equilibrium constant for the subsequent chemical equation is 2.80. At this temperature, compute the number of moles of NO2(g) that must be added to 2.52 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.
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