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You add 5.6 g iron to 28.20 mL of water and observe that the volume of iron and water together is 28.91 mL. Calculate the density of iron.
These electrons cause the emissions of secondary electrons-called auger electrons-from the metal surface. The kinetic energy of the auger electrons depends on the composition of the surface
What is the number of moles of an ideal gas, if the volume is 67 mL, the pressure is 716 mmHg and the temperature is 34 0C?
An 80.0-gram sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 6275 J. What is the specific heat of the gas
Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction
What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.113 moles/liter in a sealed container and no product was present initially
An oil is partially hydrogenated, What happens to some of the cis double bonds during hydrogenation?
The leaves of a Rhubarb contain high concentrations of diprotic oxalic acid (HOOCCOOH) and must be removed before the stems are used to make rhubarb pie. If pKa1=1.23 and pKa2=4.19, what is the pH of a .0282 M solution of oxalic acid
By how many volts will the potential of an ideal Mg+2 ion selective electrode change if the electrode is removed from a 1 x 10-4 M MgCl2 solution and replaced with a 1 x 10-2 M MgCl2 solution
A solution of .312 M KOH is used to neutralize 15.0 mL of a .186 M H3PO4 solution. what volume, in milliliters, of the KOH is required to reach the endpoint. H3PO4(aq)+3KOH(aq)>K3PO4(aq)+3H2O(l)
if i have 0.621 mole of potassium chlorate that decomposes by heat, what is the amount of the oxygen in moles?
A sample of sodium reacts completely with 0.568 (kg) of chlorine, forming 936 (g) of sodium chloride. What mass of sodium reacted
If 16.0 mL of .150 M HCL is needed to neutralize all the NH3 from a 2.25-g sample of organic material, calculate the mass percentage of nitrogen in the sample.
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