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The following problem is based on the "Nutrition Facts" found on the wrapper of an energy bar, assuming a 2000 calorie diet. The energy bar contains 100 mg of sodium, which constitutes 4% of the maximum recommended daily intake of sodium. The maximum recommended amount of sodium per day, based on this label is______x10^______g. Use 2 sig. figs.
Calculate the heat evolved in kilojoules by the formation of the solution. Calculate the heat evoled per mole of sulfuric acid. Use n(changeH) = -(mCchangeT)
Calculate w (in kJ) when 137 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 345 K:
A procedural change would be essential if a boy want to determine the tomato juice's acidity by titrating a sample of juice with NaOH(sodium hydroxide) solution Briefly explain What change would you make to the procedure ?
What volumes of the stock solution will you have to pipet into the flasks to prepare standards and What mass of gas does the container contains If the volume of a container
A certain quantity of a gas occupies 61.3 mL at 68C. If the pressure remains constant, what would the volume of the gas be at 17C?
Alkenes and non conjugated dienes usually have absorption maxima below 200nm. Compounds that have conjugated multiple bonds have maxima at wavelengths longer than 200nm.
It is often necessary to do calculations using scientific notation when working chemistry problems. For practice, perform each of the following calculations
In the reaction below, how many liters of CO2 gas are produced from the combustion of 55.0 L of CH4 gas?
The specific heat of copper is 0.385 J/(g x ?C). If 34.2 g of copper, initially at 25 ?C, absorbs 4.689 kJ
A saturated solution of Mg(OH)2 is prepared and allowed to equilibriate at 25 degrees celcius. A 25.00 mL sample of the 25 degrees celcius solution is titrated with 0.00508M HCL solution. 1.38 mL of the HCL solution are required to fully react the..
Determine the molar mass of a covalent compound to be about 220gmol-. In another experiment you establish that its empirical formula
Calculate pFe2 at each of the following points in the titration of 25.00 mL of 0.02075 M Fe2 by 0.03616 M EDTA at a 6.00 pH:11.50 mL, The equivalence point
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