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A calorimeter contains 32.0mL of water at 11.5 ?C. When 1.60g of X (a substance with a molar mass of 50.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)?X(aq) and the temperature of the solution increases to 30.0 oC. Calculate the enthalpy change, ?H, for this reaction per mole of X. Ignore any heat transfer to or from the calorimeter.
Calculate the expected theoretical yield of aspirin based on exactly 1 g of salicylic acid and 3.50 mL of acetic anhydride (density = 1.082 g mL-1).
Analysis of corrosion mechanisms and preventative measures
At noon on a clear day, sunlight reaches the earth\'s surface at Madison, Wisconsin, with an average power of approximately 5.00 kJ·s-1·m-2. If the sunlight consists of photons with an average wavelength of 510.0 nm
A 25.0 g sample of pure iron at 85.0°C is dropped into 75 g of water at 40.0°C. What is the final temperature of water-iron mixture?
The fourth solution is 10 ml of DI water and 10 ml of solution three 5) The fifth solution is 10 ml of DI water and 10 ml of solution four I'm pretty sure we're supposed to use the C1V1=C2V2 formula
the density of titanium is 7.51 g/cm^3. What is the volume (in cubic inches) of 3.5 lb of titanium?
How do you arrange PV=nRT to give equation relating pressure to concentration and use it to modify Beer's Law to apply to gas pressure? Write a formula that relates absorbance to gas pressure.
Solving this question helps the student to understand how to find the limiting reactant and how much product is produced and What mass of product may be produced?
An unknown gas effuses at a rate of 86.6 mol/hr. Under similar conditions, I2 effuses at a rate of 30.4 mol/hr. What is the molar mass of the compound.
Draw the Lewis structure of tartaric and malic acids in a way that shows the geometry of the acid functional groups. Indicate the hybridization of each carbon
What are the RATE LAW and k VALUE (with units) for the reaction? Assume conc. in moles per liter T or F. Feezer burn involves solid water conversion to vapor then back again.
Oxygen and sulfur combine to form a variety of differenet sulfur oxides. Some are stable molecules and some, including S2O2 and S2O3, decompose when they are heated
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