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The alkane 2,2,4 trimethylpentane can be used as a fuel in an ordinary engine designed for gasoline. In fact it has an "octane rating" of 100. In the fuel industry it is called iso-octane. Write a balanced equation for the combustion of this alkane with oxygen gas. Assume that the products are carbon dioxide and water. Answer the following question: If ONE mole of iso-octane is burned, how many mols of water are formed?
a. 12
b. 10
c. 9
d. 7
e. 5
What is the concentration (inM) of the chloride ion when 18.9 mL of a 0.606M solution of barium chloride is combined with 15.1 mL of a 0.62 M solution of aluminum chloride? Assume the volumes are additive
weak base so you must consider other equilibria. (Ksp(ZnC2O4)=7.5X10^-9, Kb1=1.8X10^-10, Kb2=1.8X10^-13). Solve using systematic treatment of equilibrium.
When a glow stick is placed in a freezer, its chemiluminescence lasts a significant time longer. How might this come about?
An antacid tablet containing calcium carbonate as an active ingredient required 26.8mL of .112 M HCL for complete neutralization. What mass of CaCO3 did the tablet contain?
The decay rate for carbon 14 in the sample is 14.2 dis/min per graham carbon. In what year was the coffin most likely made? ( Assume the half life of carbon-14 is 5730 years and that the decay rate for carbon 14 in living organisms is 15 dis/min p..
The elemental mass percent composition of malonic acid is 34.63% C, 3.87% H, and 61.50% O. Determine the empirical formula of malonic acid. Express your answer as a chemical formula.
A 28.0-g sample of nitrogen gas combines completely with 6.0 of hydrogen gas to form ammonia. What is the mass of ammonia formed.
Zn (s) + 2 HCl (aq) = H2 (g) + ZnCl2 (aq) If 1.26 L of H2 gas are formed at STP, how many g of HCl reacted
Calculate the mass of butane needed to produce 89.8g of carbon dioxide. express the mass of butane numerically
what should this person do from this point on to get a reasonable yield of 1-octanol?
A solution containing 80 g of KCl in 200 g of water at 50 0 C is cooled to 20 0C, a) How many grams of KCl remained in solution at 20 0C and b) How many grams of KCl crystallized out
For each reaction, calculate the mass (in grams) of the product formed when 10.1g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.
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