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Arrange the following solutions in order of decreasing freezing point: 0.20 m Fe(OH)2, 0.15 m C6H12O6, 0.10 m K3PO4, 0.15 m CH3CH2COOH, 0.35 m LiI. (Enter just the formulas in your answer. Use the appropriate <, =, or > symbol to separate substances in the list.)
C3H8(g) + 5 O2(g) ? 3 CO2(g) + 4 H2O(g) Calculate the overall enthalpy change for this reaction using standard bond enthalpies.
Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and relative abundance of 69.17%. Use the atomic weight of copper to determine the mass of the other copper isotope. Express your answer using four significant figures
Pretend you started with 3.15 g of Panacetin, and you isolated 822 mg of sucrose. What is the percent composition of sucrose in Panacetin?
A vitamin tablet contains 789 mg of vitamin C (C6H8O6). How many vitamin C molecules are contained in the tablet? Enter your answer in scientific notation.
Calculate ?G°rx (in kJ) at 582.77 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ).
why is a solution containing dissolved brass made basic with concentrated NH3 and again with acidified CH3COOH?
Determine the boiling point of an aqueous solution that is 2.30 m ethylene glycol (C2H6O2); Kb for water is 0.52 degrees celsius/m.
A certain ionic lattice consists of a ccp sublattice of cations. The anions occupy all of the tetrahedral sites. What is the empirical formula of the compound
The vapor pressure at 300 K is 856 torr. If 12.0 g of CCl3F is enclosed in a 1.0 L container, will any liquid be present? How much?
What is the wavelength of light whose energy is 1000.4 J?
Draw the structure of a compound with the following analytical data: a mw of 72 g/mol, no silver mirror in a Tollen's test, and a yellow precipiate formed in an iodoform test.
used as a fixer in the field of photography. Calculate the percentage composition, by mass, of each element in sodium thiosulphate.
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