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Question- The Nuclear mass of Fe-56 is 55.9207 amu. Calculate the binding energy per nucleon for Fe-56. (units J/nucleon)
If possible just a brief explanation how you got the answer?
In a second experiment, a 1.217 g sample of a compound with the formula C6H14O(l) was burned in the same calorimeter. The temperature increased by 10.08 oC. Use these data, plus the information given below for CO2 and H2O, to estimate the standard..
If your titration solution is 0.431 M in NaOH, and the endpoint occurs at 13.20 mL of titrant, how many mmol of NaOH are required to reach the endpoint
gaseous dinitrogen pentaoxide decomposes into oxygen and nitrogen dioxide. if we start with a partial pressure of 200
If 3.0 L of oxygen gas at 177°C is cooled at constant pressure until the volume becomes 1.50 L, then what is the final temperature
the partial pressure of oxygen in air at sea level is 0.21 atm. using the data in table 13.2 together with henrys law
Which salts are more effective for cold and hot packs, KNO3, NH4NO3, MgSO4, CaCl2, MgCl2? which are most cost effective? Maximum and minimum T for both?
Explain why the extrapolated temperature is used to determine the maximum temperature of the mixture rather than the highest recorded temperature in the experiment.
The student's body temperature dropped from 40.0C to 37C. Presume the specific heat of the student to be 3.77 J/g*C, Explain what was the final temperature of the water
How many grams of sodium bicarbonate and sodium carbonate, respectively, are needed to make 3 liters of 0.075 M buffer,
Draw any resonance form and state whether it is more or less stable than the original. ( if this is explained i will reward all points)
The rate constant of a chemical reaction increased from 0.100s^-1 to 2.90s^-1 upon raising the temperature from 25.0 degree celcius to 43.0 degree celcius
Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 164.5 C to 179C, the rate constant increases by a factor of 4.27. What is the activation energy of this oxidation reaction
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