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A mixture containing 40.0mL of 2.67*10-2 M Ca(NO3)2 and 60.0mL of 1.78*10-2 M Na2CO3 is prepared. Presume 100.0mL of solution is formed.
A. Compute the molar concentrations of Ca2+ and CO3 2- originally added in the 100.0mL solution.
B. Compute the mass of CaCO3 that precipitates. Ksp=3.84*10-9
The analysis of a compound shows that it contains 20.0% H and 80.0% C. The empirical formula is:
How much heat is required to raise the temperature of a stainless steel pot weighing 450 g and containing 270 g of water from 25 degrees Celsius to boiling if the specific heat capacity of stainless steel is 0.51 J/(g*degrees C)
A 0.831-g sample of SO3 is placed in a 1.00 L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2SO3 (g) 2SO2 (g) + O2 (g). At equilibrium the total pressure in the container is 1.300 atm.
When the O2 molecule is ionized to O2+, its bond becomes stronger; however, when the C2 molecule is ionized to C2+, its bond becomes weaker.
Explain why anhydrous sodium sulfate is used in the extraction experiment and write reactions that shows what happens. Organic layer has p-tert-Butylphenol
has freezing point depressiom constant of 42.8 C/molal .if you mix 29.67 grams of camphor with 4.28 grams of triose (C18 H32 O11), wht will be the new melting point of the mixture
The decomposition of hydrogen iodide on finely divided gold 150 C is zero enter with respect to HI. The rate defined below is constant at 1.20X10-4 mol/L -s
Write the lewis formula for the reactant and product species in the following chemical equation. Include nonbonding electrons. 2OH yields H2O2.
A mixture of two miscible solvents that may be used as the solvent for a recrystallization experiment would be which of the following
Calculate the pressure in atmospheres using both the ideal gas law and the van der Waals equation. For N2, a=1.35(L^2 x atm)/mol^2, and b=0.0387L/mo
A 3.0 L bulb containing He at 129 mmHg is connected by a valve to a 2.0L bulb containing Ar at 110 mmHg. Calculate the partial pressure of each gas and total pressure after the valve between the flask is opened.
what is the solubility of O2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O2 in air is 0.209 at both 12,000 ft and at sea level.
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