Question

all done

Answer 1

First you have to balance the chemical equation. Can you do that ?

Answer 2

yeet
= Yes

Answer 3

good for you. But i want to know if studydeep knowz how to balance the equation.

Answer 4

copypaste.. from where ??

Answer 5

this is the best step by step

Answer 6

ok....

Answer 7

sorry for the late reply but how do i do that?

Answer 8

\[\rm \color{red}{NaHCO_3 }\rightarrow \color{blue}{ Na_2CO_3+H_2CO_3}\]\[\rm \color{red}{Reactant} ~~~~~~~~~~ \color{blue}{Product}\]
write down all the elements that are present in this chemical equation
\[\rm \color{red}{Reactants}\]\[\rm\color{red}{ Na}\]\[\rm \color{Red}{H}\]\[\rm \color{Red}{C}\]\[\rm\color{Red}{ O}\]
\[\rm \color{blue}{Products}\]\[\rm\color{blue}{ Na}\]\[\rm \color{blue}{H}\]\[\rm \color{blue}{C}\]\[\rm\color{blue}{ O}\]
look at he equation and see how many sodium hydrogen are present at each side

Answer 9

let me do the product side for you to give you an idea ...
\[\rm \color{blue}{Products}\]\[\rm\color{blue}{ Na~~~~2}\]\[\rm \color{blue}{H~~~~~~2}\]\[\rm \color{blue}{C~~~~~~2}\]\[\rm\color{blue}{ O~~~~~~6}\]

there are 2 sodium atom on right side
2 hydrogen atom
2 carbon
and 6 oxygen \[\rm O_3 ~~and O_3= 6 ~~oxygen\]

Answer 10

ok i see i think... how do i put this into a balanced chemical equation?

Answer 11

\[\rm \color{red}{NaHCO_3 }\rightarrow \color{blue}{ Na_2CO_3+H_2CO_3}\]\[\rm \color{red}{Reactant} ~~~~~~~~~~ \color{blue}{Product}\]

\[\rm \color{red}{Reactants}\]\[\rm\color{red}{ Na~~~1}\]\[\rm \color{Red}{H~~~1}\]\[\rm \color{Red}{C~~~1}\]\[\rm\color{Red}{ O~~~~3}\]
\[\rm \color{blue}{Products}\]\[\rm\color{blue}{ Na~~~~2}\]\[\rm \color{blue}{H~~~~~~2}\]\[\rm \color{blue}{C~~~~~~2}\]\[\rm\color{blue}{ O~~~~~~6}\]

The number of each atoms needs to be same on both sides
so.. if you multiply the reactants by 2 you will get
\[\rm \color{red}{\color{black }{2}NaHCO_3 }\rightarrow \color{blue}{ Na_2CO_3+H_2CO_3}\]
\[\rm \color{red}{Reactants}\]\[\rm\color{red}{ Na~~~\cancel{1} ~~2}\]\[\rm \color{Red}{H~~~\color{red}{\cancel{1}}~~~2}\]\[\rm \color{Red}{C~~~\cancel{1}~~~2}\]\[\rm\color{Red}{ O~~~~\cancel{3}~~~6}\]

The equation is now balanced.

Answer 12

ok I see...
now I know that Percent yield = (actual yield)/(theoretical yield) * 100

is the actual yield 1.57 g?
and how do I find theoretical yield?

Answer 13

in the mean time.. im just going to repost to see if anyone can help with the theoretical yield part.. but if you are still willing to help just comment back on this post :)