Calculate the mass defect for 239U239U, which has a mass of 239.05429 amuamu . (The mass of 11H11H is 1.00783 amuamu, and the mass of a neutron is 1.00866 amuamu .)

The mass defect for U-239 is 1.93909 amu.

Explanation:

The mass defect can be calculated using the following equation:

Where:

: is the proton mass = 1.00783 amu

: is the neutron mass = 1.00866 amu        

M: is the mass of U-239 = 239.05429 amu

Z: is the number of protons = 92

N: is the number of neutrons = A - Z

A: is the atomic mass number = 239

Therefore, the mass defect for U-239 is 1.93909 amu.

I hope it helps you!                                                        

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

confused

confused             hewdejdnjnjsnd