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The reducing agent in this catalytic hydrogenation reaction was molecular hydrogen (H2), which was produced in situ during the course of the reaction.
a) During the course of the experiment, how did you know that molecular hydrogen (gas) had been formed?
b) Write a balanced chemical equation for the reaction that produced molecular hydrogen.
c) Was molecular hydrogen the limiting reactant? Why or why not (Hint: show the necessary calculations)?
Calculate the de Broglie wavelength of a neutron moving at 1.17% of the speed of light. _____m
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If 30.0 L of oxygen gas is cooled from 473 K to 274 K at constant pressure, what is the new volume of oxygen
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What is the standard change in Gibbs free energy of this reaction at 25 °C. Hint: The equilibrium constant is related to the change in Gibbs free energy
How many moles of methane occupy a volume of 2.00 l at 50.0*C and0.500 atm? (R=0.0821 atm*L/molxK)
how many grams of sodium acetate must be added to 1.00 L of a .200 M acetic acid solution to form a buffer of 4.20? Ka value for acetic acid is 1.8x10^-5.
A steel cylinder holds 150.0 mol argon gas at 25 degrees C and a pressure of 9.53Mpa. After some argon has been used, the pressure is 2.00Mpa at 19 degrees C. What mass of argon remains in the cylinder.
Ttotal ammonia concentration = 0.400 M. determine What is the concentration of NH 4 + ?
A truck driver used sand to soak up a 1 g spill of lindane (C6H6Cl6). He placed the contaminated soil in an open drum which then filled with 150 L of water during a rainstorm.
What will be the average atomic mass of element A if percentage abundance of these two isotopes are 48.17 % and 51.83 % respectively. ?
When relatively small amounts of magnesium burns, the fires are extinguished using commercially available dry powder. Why might this fire rekindle days later as someone tries to remove the residue with water?
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