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(a) What is the kinetic energy in joules of an 850-lb motorcycle moving at 66 mph?
(b) By what factor will the kinetic energy change if the speed of the motorcycle is decreased to 33mph?
(c) Where does the kinetic energy of the motorcycle go when the rider brakes to a stop?
A gas occupying a volume of 395 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?
Aromatic Compounds :sample question, Both naphthalene and azulene have 10 pie electrons and are aromatic. Pentalene is apparently antiaromatic and is unstable even at -100 degrees C.
When ice melts, it absorbs 0.33 kJ per gram. How much ice is required to cool a 13.0 oz drink from 74 degree F to 31 degree F
calculate the amount of energy as heat by the freezing of 13.3 g of a liquid substance. given that the substance has a molar mass of 82.9g/mol and a molar enthalpy of fusion of 4.60 kj/mol.
PH of Acetylsalicylic Acid, The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with a Ka = 3.3x10-4
What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2 (balanced with lowest whole-number coefficients)?
Metallic copper is formed when aluminum reacts with copper(II) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al react with 319 g of CuSO4?
If the diameter of a sodium atom is 3.14×10-8 cm, how many sodium atoms would fit along a line exactly 6.00 inch long?
Calculate the number of grams of HC2H3O2 needed to make 450 mL of 0.322 M solution.
Calculate the number of moles of solute present in eahc other following solutions: a) 60.0g of an aqueous solution that is 1.25 percent KI by mass, b) 250g of an aqueous solution that is 0.460 percent NaCl by mass, c) 0.600L of 1.25M H2SO4.
Explain the chemical process that occurred in his muscle cells to cause this discomfort. Explain the chemical reaction that has taken place in the body after exercise.
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21
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