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Given K=1.03x10^-3 for H2S(g)=H2(g)+S2(g) at 750 degrees Celcius. How many moles of S2 would you have to have at equilibrium in a 3.68 liter box in which there are 1.63 moles of H2S and 0.864 moles H2
To treat a burn on your hand, you decide to place an ice cube on the burned skin. The mass of the ice cube is 12.9 g, and its initial temperature is -13.9 °C. The water resulting from the melted ice reaches the temperature of your skin,
What is the partial pressure of argon, in torr, in a container that also contains neon at 147 torr and is at a total pressure of 536 torr?
Using the information below, what is the most stable form of sulfur at 298K and 1atm? (no calculations needed) S(rhomic): V=0.016, delta H formation=0, delta G formation=0, Standard molar S=31.8, standard molar Cp=22.64 S(monoclinic)
Calculate the mass of propylene glycol that must be added to .360 kg of water to reduce the vapor pressure by 2.87 torr at 40 degrees celsius (Ph20 at 40 degrees = 55.3)
NaOH is added to K2CrO4 and K2Cr2O7 separately in test tubes and a color change is noted.
I am given the 10 ml of .200M Fe(NO3)3 and .25 ml of .00200 KSCN and 14.75 ml of .500 M of HNO3. How do I figure out the initial concentration of FE3+ and SCN-.
Mg3N2 + 6H2O ----> 3Mg(OH)2 + 2NH3 When 36.0g of H2O react, how many grams of NH3 are produced?
Determine how long will it take for a sample of N2O5 to decay to sixty percent of its initial value?
A calorimeter that contains 2500 g of surrounding water is used to measure the heat associated with the reaction of 520 g of a reactant. Calculate the energy, in joules per kilogram of reactant, associated with the reaction
Suppose 1.00 g of water (saturated liquid) evaporates isobarically at atmospheric pressure of 1.013x10^5 Pa. Its volume in the liquid state is 1.00 cm3 and its volume in the vapour state is 1671 cm3.
Calculate the pH of 1.00 L of a buffer that is 0.130 M HNO2 and 0.190 M NaNO2. What is the pH of the same buffer after the addition of 1.00 mL of 12.0 M HCl. (pKa of HNO2 = 3.40)
How many many molecules of XeF6 are formed from 12.9L of F2 (at 298K and 2.60atm). Asssume there is an excess of Xe
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