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Create a data table to record your data from the procedure. Be sure that the data table is neat and organized and that all measurements have the correct significant figures and units. Write the complete balanced equation for the reaction that occurred in this lab. Hint: H2CO3 is not a final product of the double-replacement reaction; it breaks down (decomposes) immediately into two products.
A compound of iodine and cesium contains 69.75 g of metal and 66.20 g of nonmetal. How many grams of cesium are in 38.52 g of compound? How many grams of iodine
A scuba diver 40 ft below the ocean surface inhales 50.0 mL of compressed air mixture in a scuba tank at a pressure of 3.00 atm and a temperature of 8 degrees C
0.000333 g fluorescein (332.32 g/mol) is dissolved in 225 mL solution of ethanol. The density of ethanol is 0.785 g/mL. What is the concentration of the solution in molarity (M)
A 2.48 L sample of He at 739 torr is mixed with 6.08 L of Ar at 325 torr both at 25 degrees C is placed in a 4.80 L container at 25 degrees C. What is the partial pressure in atm of He
Which proton(s) in 1-phenylethanol corresponds to the tall singlet at about 7.40 ppm in the 1H NMR?
Propanoic acid, HC3H5O2, ionizes in water and has a Ka=1.34x10^-5. What is value of Kb for the propanoate ion
Write a balanced equation for the conversion of C6H5CHOHCH3 to methyl ketone in the presence of I2 and NaOH. Identify which is being oxidized and which is being reduced.
Graphite is a semi-metal composed of sheets of fused benzene rings. There are no bonds between sheets, only van der Waals interactions
an 18.0-g sample of magnesium is completely burned in the presence of air to form magnesium oxide. what is the mass of
A test solution contained 2 mL of 0.10 M Ag+. A silver strip was dipped into the test solution, and a cell potential of 0.0592 V was measured against an Ag/Ag+(1.0M) reference half-cell.
A chemist prepares a sample of hydrogen bromide and finds that it occupies 252 mL at 70C and 464 Torr. What volume would it occupy at 0C at the same pressure.
Consider the dissolution of CaCl2. CaCl2(s) Ca2+(aq) + 2 Cl-(aq) ΔH = -81.5 kJ A 13.2 g sample of CaCl2 is dissolved in 106 g of water, with both substances at 25.0°C.
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