Question

Could someone help me with this chemistry question, I don't know where to start ?

Answer 1

@aaronq @radar I know I have to use E=mc^2 but I'm confused on what to use for the m

Answer 2

hm i'm not very familiar with nuclear chemistry, but its asking for the change in energy, so i would do: \(\Delta m=m_{Products} -m_{reactants}\)

the find the energy in \(\Delta m\) with E=mc^2

Answer 3

thats what I am doing, but idk if im doing the difference in mass right

Answer 4

i keep getting the answer wrong

Answer 5

can you post what you're doing?

Answer 6

umm im just doing it on my calculator. but its the mass of the right side with the He and H - the mass of the left side (i didn't use the mass of the neutron ) times Avogadro No and 1.66053886x10^-27 kg then speed of light

Answer 7

\(\Delta m\)=(4.00260+1.00782)-(2.01410+3.01603)=-0.01971 amu

while you have to convert to kg, i don't think you need to multiply by avogadro's, the masses given are already in grams.

Answer 8

but it need its in J/mol

Answer 9

how do i get the mol

Answer 10

sorry i mean g/mol, those are molar masses

Answer 11

oh ok so no avo number

Answer 12

nope.

Answer 13

i get 2.95 X 10 ^-12

Answer 14

it says Incorrect. Energy is released in this reaction. What does that tell you about the sign of ΔE? Also, you need to scale the energy up to correspond to the production of a mole of helium atoms, not just one helium atom.

Answer 15

did you plug it in as a negative number?

Answer 16

no

Answer 17

but what about the last part of what it says

Answer 18

i think it should be, from the difference of masses.

the last part of what you said doesn't make much sense because the mass of one helium atom is \(\dfrac{4~g}{6.022*10^{23}}\)= \(6.6*10^{-24}g\)

Answer 19

so do i multiply it by 4 and divide by 6.002 x10^23 when converting to g

Answer 20

i got it wrong again

Answer 21

could u help with another question instead

Answer 22

@aaronq

Answer 23

can't, i have to go. sorry

Answer 24

ok