Asked by Masey
For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts.
2HgO(s)¨2Hg(l)+O 2 (g) 2\;{\rm{HgO}}\left( s \right)\; \rightarrow \;2\;{\rm{Hg}}\left( l \right) + {\rm{O}}_2 \left(1.40 kgHgO g \right)
2HgO(s)¨2Hg(l)+O 2 (g) 2\;{\rm{HgO}}\left( s \right)\; \rightarrow \;2\;{\rm{Hg}}\left( l \right) + {\rm{O}}_2 \left(1.40 kgHgO g \right)
Answers
Answered by
DrBob222
I can't make sense of your post but here is how you work the problem.
1. Write and balanced equation. You've done that.
2. Convert grams HgO (whatever that is) to mols. mols = grams/molar mass
3. Using the coefficients in the balanced equation, convert mols HgO to mols O2.
4. Now convert mols O2 to grams O2. grams = mols x molar mass
1. Write and balanced equation. You've done that.
2. Convert grams HgO (whatever that is) to mols. mols = grams/molar mass
3. Using the coefficients in the balanced equation, convert mols HgO to mols O2.
4. Now convert mols O2 to grams O2. grams = mols x molar mass