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The element copper has an atomic weight of 63.5 and consists of two stable isotopes copper-63 and copper-65. The isotope copper-63 has an atomic mass of 62.9 amu and a percent natural abundance of 69.1 %. The isotope copper-65 has a percent natural abundance of 30.9 %. What is the atomic mass of copper-65? amu
theoretically feasible in a solution that initially 0.250 M in each ion? c.) If separation is feasibe in eithee (a) or (b), what ranfe of anode potential (vs. SCE) should be used?
A sample of sodium reacts completely with 0.568kg of chlorine, forming 936g of sodium chloride. What mass of sodium reacted.
At 123?C, the pressure of a sample of nitrogen is 1.45 atm. What will the pressure be at 267?C, assuming constant volume?
total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 149 g of solution. The reaction
How much faster do ammonia (NH3) molecules effuse than carbon monoxide (CO) molecules? Enter the ratio of the rates of effusion.
Two moles of potassium chloride and three moles of oxygen are produced from the decomposition of two moles of potassium chlorate, KClO3(s). Write the balanced equation. How many moles of oxygen are produced from 12 moles of potassium chlorate?
Creat a spread sheet or matlab file with the following functionality: a/ The utility shoud use th P(in MPa) and T(in K) to calculate the ideal gas molar volume (in cm3/mol) at a reference state and two other states labeled ‘state1' and ‘state2'.
Define detection limit. Does a compound with high molar absorptivity have a higher or lower limit of detection than a compound with low molar absorptivity
Compute the number of moles of Chlorine atoms in 3.01×10^24 formula units of magnesium chloride,MgCl2 .
What mass of natural gas (CH4) must burn to emit 470. kJ of heat? CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g).
if a container of nitrogen, oxygen, carbon dioxide has a pressure of 2.00atm and the partial pressure of O2 is 312torr,
Determine the numbers of moles of iron that would be formed from 6.2 moles of CO (carbon monoxide) combining with excess of iron (III) oxide (Fe2O 3 )?
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