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When a student chemist transferred the metal to the calorimeter, some water splashed out of the calorimeter. will this technique error result in the specific heat of the metal being reported too high or too low? explain
A buffer that contains 0.255 M of acid, HA and 0.153 M of its conjugate base A-, has a pH of 3.39. What is the pH after 0.0115 mol of NaOH are added to 0.666 L of the solution
The solution to Equilibrium constant, A certain gas mixture held at 395C has the following initial partial pressures: P(Cl2) = 351.4 torr; P(CO) = 342.0 torr and P(COCl2) = 0.
Consider the voltaic cell below, which is symmetric except for the fact that [Cu2+] is 1.0 M on the left side and 0.01 M on the right. Which electrode is +, and what is Ecell?
How many kilojoules are released when 10.0g of steam condenses at 100 degrees C and cools to 0 degrees C?
Pure colored substances mostly exhibit a single peak (i.e. max) in the visible; therefore the simple rules of complementary colors apply. Mixtures are a little more complicated.
If acetic acid has a pure vapor pressure of 20 torr at 30 degrees C and acetaldehye has a pure vapor pressure of 1000 torr at 30 degrees C, a mixture of 12 moles of acetic acid
the system is not at equilibrium and will shift to the right to achieve an equilibrium state. not at equilibrium and will shift to the left to achieve an equilibrium state. at equilibrium. not at equilibrium and will remain in an unequilibrated sta..
The pH of a 0.100 M formic acid solution (HCHO2) is 2.38 at 25 °C. Determine the Ka and pKa of formic acid
what is the annual cost of operation in a 70°F room if the door is opened 10 times a day with an average heat gain per opening of 200 kJ? How much would it cost to keep the inside at 35° F
Calculate the solubility of silver chromate in 0.005 M Na2CrO4.
The student found that 8.67mL of NaOH solution was needed to titrate a 0.0544g sample of the acid to the equivalence point. Calculate the mass of unknown required for a 30.0mL titration.
A mixture of 1.07 g H2 and 1.50 g He is placed in a 1.00-L container at 30.°C. Calculate the partial pressure of each gas and the total pressure.
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