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Consider the following reaction at equilibrium:
2CO2(g) <--> 2CO(g) + O2(g) Change in H degree = -514kJ
a) increase partial pressure of CO2 at equilibrium
b) increase partial pressure of CO at equilibrium
c) decrease partial pressure of CO2 at equilibrium
d) increase the value of the equilibrium constant
e) decrease the value of the equilibrium constant
What is the molality of ethanol in a solution made by dissolving 14.6 g of ethanol, C2H5OH, in 53.6 g of water?
Which do you think would be larger and why? The first ionization energy, IE1, of Ne,The second ionization energy, IE2, of Na
The solvolysis product of 1-bromo-2,2-dimethylbutane with ethanol initially forms the expected carbocation but does not give any of the expected 1-ethoxy-2,2-dimethylbutane. Draw the rearranged cation that will eventually lead to the product.
Draw the mechanism for each reaction you will do today. Pyridinium tribromide releases molecular bromine, so molecular bromine is the brominating agent.
Determine how many grams will remain in 150 Years If we have 150.000 g of 137Ce now,?
What is the partial pressure of Br2 at equilibrium? What is the partial pressure of I2 at equilibrium? What is the partial pressure of IBr at equilibrium?
When caffeine is treated with HCl what solvent is the resulting compound more soluble in? Methylene chloride, chloroform, or water When carboxylic acid is treated with a base such as NaOH
How many grams of NaN3 are required to produce 340 L of nitrogen gas if the gas has a density of 1.25 g/L?
If you start with 1.000 g of sulfur (S8) and obtain 4.963 g of pure compound. What is the empirical formula of this compound?
An 85.0g sample of iron requires 954 J of heat to raise its temperature 25.0C. What is the specific heat of the iron?
The number of moles in 15.39 g of C2H6O (molar mass =46.1 g/mol) is ,You transfer a sample of gas at 17 degrees C from a volume of 4.71 L and 1.10 atm to a container at 37 degrees C.
Water at 0 degrees C was placed inside a vessel maintained at low pressure by a vacuum pump. After some of the water evaporated, the remainder froze. If 1.2g of water evaporated, how much ice was obtained? Use the heats of vaporization and fusion ..
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