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A 350.0 gram sample of copper is initially at 25.0 °C. It absorbs 12.50 kJ of heat from its surroundings. What is its final temperature, to the nearest tenth of a degree?
A student is concentrating a solution having a polypeptide of modest molecular weight by pressure filtration through a membrane. The solute concentration on the feed side of the membrane is 0.10 M and the temperature is twenty five degree celsius.
A 0.4780-g sample of impure Ca(OH)2 is dissolved in enough water to make 57.00 mL of solution. 20.00 mL of the resulting solution is then titrated with 0.1140-M HCl.
A chemical firm was hired to monitor a nearby lake for possible mercury contamination. Several samples were taken at different locations around the lake, including water samples.
if molarity of a 2000ml solution is 4.0M NaCl, how many moles of NaCl are dissolved in that solution.
What would the theoretical yield in moles be and how would you calculate that? What would the theoretical yield in grams be and how would you calculate that?
How long would it take for a radioactive isotope with a half life of 2 weeks to lose at least 70% of its radioactivity? Describe two clinical uses of Radioactivity.
Given the following reaction: 2 O2 + CH4 CO2 + 2 H2O What mass of CH4 is required to completely react with 100 grams of oxygen.
How much heat (in kJ ) is required to warm 13.0 of ice, initially at -13.0, to steam at 114.0? The heat capacity of ice is 2.09 and that of steam is 2.01
If a reaction mixture initially contains 486 of and 261 of , what is the mole fraction of when equilibrium is reached.
A flask contains 0.330 mol of liquid bromine, Br2. Determine the number of bromine molecules present in the flask.
Consider 20.0 moles of CO2 in a 1.0 liter container at 300.0 K. What is the pressure predicted by the van der Waals equation.
An aqueous antifreeze solution is 48.5% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.062 g/cm3. Calculate the molality, molarity and mole fraction of ethylene glycol
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