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The volume of a component is to be measured by a process whose uncertainty is 0.05 ml.
a. If 25 independent measurements are made and the average of these is used to estimate the volume, what will the uncertainty be?
b. How much more precise is the average of 25 measurements than a single measurement?
Draw additional molecules of sulfanilamide and hypothesize the intermolecular interactions that are most important for providing a stable and selective crystal structure
What volume of gold would be equal in mass to a piece of copper with a volume of 140.0 mL? The density of gold is 19.3 g/mL; density of copper is 8.96 g/mL
suppose you wanted to dissolve 106 g of Na2CO3 in enough H2O to make 6.00L of solution what is the molar mass of Na2CO3.
The steam reforming of methane is widely used in industry to make hydrogen, as given in the following reaction:CH4(g) + H2O(g) ? CO(g) + 3H2(g) a) Calculate the (approximate) enthalpy change
A solution contains 4.56 g of KCl in 175 mL of solution. if the density of the KCl solution is 1.12 g/mL, what are the mass percent (m/m) and moarity (M) for the KCl solution
An evaluation of R was performed, following the procedure described in this module. The barometric pressure was 736 torr, the temperature was 295k and volume of hydrogen gas collected was 35.6 mL.
What is the total pressure in the vessel just after the reagent gases are added (assume ideal behavior) and what are the mole ratios of the reagent gases in the vessel before the reaction begins?
The solubility of O2 in water is 6.5 mg/L at an atmospheric pressure of 1.0 atm and temperature of 40 degrees C. Calculate the Henry's Law constant of O2 at 40 degree C. The mole fraction of O2 in air is .209
Use the Nernst equation to calculate the expected potential in the battery in parts 2(d) and 2(e) when the following concentrations are present: [Cr2O72?] = 3.7 x 10?3 M ; [Cr3+] = 0.0112 M
The specific heat of Al and water are 0.90 J/(goC) and 4.184 J/(goC), respectively. Calculate the equilibrium temperature.
There is 12.0 g CCl3F in a 1.1 L container at 856 torr and 300 K. What is the mass of the liquid left over?
Its normal boiling point is 111.0oC and its molar heat of vaporization is 35.9 kJ/mol. What would be the vapor pressure (in torr) of toluene at 75.00oC?
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