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A set of two gas bulbs, with volumes of 500 mL and 300 mL, are connected by a closed stopcock. The 500 mL bulb contains 450 torr of Ne gas, and the 300 mL bulb contains 150 torr of Cl2 gas. When the stopcock is opened and the system comes to equilibrium, what is the total pressure in the system?
A) 338 torr
B) 540 torr
C) 263 torr
D) 600 torr
E) 300 torr
HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.00 L of solution
Name the product of reaction, Give and name the products when 3-t-butyl 2,4-dimethyl 1-hexene reacts iwth the following assume the proper catalysts are present
Assume that the specific heat of the solution is the same as that of pure water. Calculate delta(H) (in kJ/mol NH4NO3) for the solution proces.
The Temperature is a constant 400.0 K. Calculate won, the work done on the system, and report the answer in Joules.
A calorimeter contains 17.0 mL of water at 15.0 degrees celcius When 1.40 g of (a substance with a molar mass of 69.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)->X(aq)
The reactant concentration in a zero-order reaction was 8.00×10-2 after 100 and 4.00×10-2 after 370 .
what is the valence molecular orbital configuration (according to MO theory) of homonucleic diatomic species where the atoms have an atomic number greater than seven?
a solution is prepared by dissolving 23.7g of CaCl2 in 375g of water. The density of the resulting solution is 1.05g/mL.
Calculate the amount (in grams) of N-methylmaleimide and 9-(hydroxymethyl)anthracene that are required in a reaction utilizing 0.5mmol 9-(hydroxymethyl)anthracene (208.26 g/mol) and 3 molar equivalents of N-methylmaleimide (111 g/mol)
Dry ice, CO2 (s), has a melting temperature of -78o C and will not form a liquid unless atmospheric pressure exceeds 5.1 atm. The following reaction is conducted at -90o C and 101.325 kPa: CO2 (g) ? CO2 (s)
A 343 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 625 mmHg. Calculate the moles of Ar present.
How many grams of a stock solution that is 85.5 percent H2SO4 by mass would be needed to make 150 grams of a 45.0 percent by mass solution?
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