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A particular smoke detector contains 2.15 of , with a half-life of 458 . The isotope is encased in a thin aluminum container. Calculate the mass of in grams in the detector.
Which of the following is always true for a spontaneous process at constant temperature? A) Delta S system + Delta S surroundings = q/T B) Delta
Find the molecular mass of sucrose and determine how many molecules there are in 1kg of it.
Consider the reaction A+2B = C whose rate at 25 C was measured using three different sets of initial concentrations as listed in the following table: Trial Rate 1 0.25 0.010 7.5×10?4 2 0.25 0.
Zubrick and explain the meaning of the term 'salting out'. When might you want to do this? explain what we really are doing in this step and why it could not possibly be to salt-out the product at t
1.what advantage do calcium chloride pellets have over magnesium sulfate powder. 2.what advantage does decantation have over filtration for small volumes
When 2.25 g of sodium hydroxide (NaOH) was dissolved in 150.00 g of water a value of 11.00oC was obtained for ?T. Calculate the molarity of the sodium hydroxide solution. _______ Calculate the value
How many grams of Ba(BrO)2 could be produced through the complete reaction of 50 mL of .40 M HBrO? Use the balanced equation Ba(OH)2 + 2 HBrO = 4H2O + Ba(BrO)2
if titration of 20.0 mL of 1.50 M H2SO4 solution requires 25.0 mL of NaOH to reach equivalence point, what is the molarity of the NaOH titrant
When 210.0mL of 0.350M K2CrO4(aq) are added to 210.0mL of 1.10×10^?2M AgNO3(aq), what percentage of the Ag^+ is left unprecipitated
A 0.150 M Na2SO4 Has [Ag^+] = 9.7x10^-3 M. What is the value of Ksp for Ag2SO4 obtained with these data
Which of the following is always true for a spontaneous process at constant temperature. A) Delta S system + Delta S surroundings = q/T B) Delta S > 0 C) Delta S = q/T D) Delta system + Delta S s
MnSO4 (aq) is converted to MnO2(s) in a basic medium as oxygen gas is converted to hydroxide ion. In this case, is the sulfate ion a spectator ion
Calculate the change in pH of rainwater resulting from an increase in the Pressure of CO2 from 10^-3.5 atm to 10^-3.0 atm due to fossil fuel emissions
What is the formal charge on the indicated atom in each of the following species? sulfur in SO2 nitrogen in N2H4 each oxygen atom in ozone, O3
The molar heat capacity of Cu(s) at 1 atm pressure has been measured over a range of temperatures from close to 0 K to 400 K. Describe how you would obtain the standard molar entropy of Cu(s) at 298
Calculate the standard entropy of the condensation of chloroform at its boiling point, 335 K. The standard molar enthalpy of vaporization of chloroform at its boiling point is 31.4 kJ x mol-1.
Calculate the change in molar entropy when 2.00 miles of ozone are compressed isothermally to one quarter of its original volume. Treat ozone as an ideal gas.
Consider the following generic chemical equation. 2A+4B ---> 3C. What is the limiting reactant when each of the following amounts of A and B are allowed to react? 2 mol A; 5 mol B 1.8 mol A; 4 mo
The temperature of 2.00 moles of Ne(g) is increased from 25 C to 200 C at constant pressure. Calculate the change in the entropy of Neon.
Write the balanced nuclear equation for the formation of 241/95 Am through beta decay
For a given transfer of energy, a greater change in disorder occurs when the temperature is high.
A lab student analyzed a nickel-en complex for ethylenediamine, en, content. A 0.353g sample of the synthesized Ni-en complex was dissolved in about 50 mL of water and titrated with 0.165 M HCl (aq)
A gaseous system undergoes a change in temperature and volume. What is the entropy change for a particle in this system if the final number of microstates is 0.828 times that of the initial number o
Use Slater's rules to calculate the shielding constant and effective nuclear charge for a 5s, 5p, and 4d electron in the tin atom. Which of these electron experience the lowest effective nuclear cha