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A backpacker wants to carry enough fuel to heat 2.9 kg of water from 27 degrees C to 100.0 degrees C. If the fuel he carries produces 36 kJ of heat per gram when it burns, how much fuel should he carry? (For the sake of simplicity, assume that the transfer of heat is 100% efficient.)
At noon on a clear day, sunlight reaches the earth\'s surface at Madison, Wisconsin, with an average power of approximately 2.00 kJ·s-1·m-2. If the sunlight consists of photons with an average wavelength of 510.0 nm, how many photons strike a 5.40..
determine the trend in sizes of the ions o2-n3- f- and also explain why does the trend exist? also describe which of
Write the formula for the ion formed when each of the following elements loses its valence electrons?
A certain reaction A ? products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete
a volume 505 mL of air on a cold winter day at -15 degrees celcius is breathed into the lungs, where body temperature is 37 degrees celcius
A certain second-order reaction has a rate constant of 1.10×10-3 at 27 C and an initial half-life of 226 . What is the concentration of the reactant after one half-life?
An unknown sample (0.6855 g) containing KHP is titrated to the equivalence point with 9.75 mL of ).07892 M NaOH, How many moles of KHP present?
f gas reacts with nh3 gas to produce n2f4 tetrafluorohydrazine or dinitrogen tetrafluoridenbspand hfhydrogen fluoride.
assuming zinc is the limiting reagent how much zinc in grams do i need to fill a 1.0 liter balloon with hydrogen gas at
If 125 cal of heat is applied to a 60.0 g piece of copper at 25.0 C, what will the final temperature be? The specific heat of copper is 0.0920 cal/(g.C}) .
The half-life for the second order reaction of a substance A is 55 seconds when [A]o is 0.84 M. What time is needed for the concentration to decrease to 1/4 of the original value.
where C is a constant.The following table gives the equilibrium constant (Kp) at various temperatures for the reaction of nitrogen monoxide with oxygen gas that produces nitrogen dioxide
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