Question

Help me.

SS below.





Or let the math kill me.

Answer 1

@QuestionCoveBot Egghead, you said you could help me.

Answer 2

which one there to many

Answer 3

Anyways, I need help with all. ;c Someone to check over my work as I go along.

Answer 4

nvm

Answer 5

So for number one.
\[ 2H _{2} + O _{2} \rightarrow H _{2}O\]

H=2 H=2

O=2 O=1

H=4 H=4

O=2 O=2

Right?

Answer 6

I don't know what I am supposed to put before O on the Reactant side.

Answer 7

Are you trying to figure out how much of what makes what? Like how much H2 and O2 makes water?

Answer 8

No, we have to balance the equations and stuff.

Answer 9

Ah okay. Makes more sense. So... I hope you know how much O2 and H2 makes water? I am confused on what you mean by "balance".

Answer 10

Errrr, It isn't balanced when we get it so then we have to balance the chemical equation. That is why there are blank spots.

Answer 11

So your saying... that we have to add the exact amount of H2 and O2 to balance the equation?

Answer 12

Not nessecarily, Idk how to explain it. ;c

Answer 13

Okay, well...

you know how much O2 goes with H2 to make H2O?

Answer 14

Yeah?

Answer 15

it's \[H _{2}O _{1}\]

Answer 16

I'm sorry, I have to get off for a little. I'll be back later. Maybe @carmelle can help.

Answer 17

Ok ;c

Answer 18

All you have to do is add the amount of chemical for all blanks that makes the end result.

Answer 19

Not entirely, it's much more than that from what I've learned.

Answer 20

Hmm okay. What else do you have to do then, other than adding the amount of chemical to the blanks?

Answer 21

Ahhh, long story ;c

Answer 22

Just go ahead and tell it. xD

Answer 23

If you can understand my notes, I would show you but I can't bc I can't understand it xD

Answer 24

\(\color{#0cbb34}{\text{Originally Posted by}}\) @Astrid1
If you can understand my notes, I would show you but I can't bc I can't understand it xD
\(\color{#0cbb34}{\text{End of Quote}}\)
ss the notes.

Answer 25

OKay.

Answer 26

Sorry, The latency sucks on my computer rn.

Answer 27

It's okay. I can see it well enough.

Answer 28

Okay/

Answer 29

where the question

Answer 30

@snowflake0531

Answer 31

it's making the chemical be more even, like making it into one if that makes any sense.

Answer 32

I know.

Answer 33

like the number down below, that should be it if im thinking straight :)

Answer 34

Number down below? o-o

Answer 35

=w= the first one is 2h2+_O2=_h2o

Answer 36

like how manny H2Os can you make if you have 2 H2

Answer 37

technically 4 H's

Answer 38

Yeah, I wasn't paying attentioj to this, EXT keeps stealing my emojis.

But yeah Ik 4.

Answer 39

so if you have 4 h's how many O's do you need to make an even amount of h2os

Answer 40

2?

Answer 41

o: yes

Answer 42

So now that we balanced out
4H + _2O = 4H 2O
What times 2O equals 2O

Answer 43

:> you forgot the little- 2 but mk xD means the same thing

Answer 44

I'm just putting the small numbers in front of it, so it looks like math

Answer 45

Yeaaa.

Answer 46

So, for the first one, the first blank is 1, the second blank is 2

Answer 47

So for the second one, we have
_Mg + _2O = __ Mg O

Answer 48

You can first automatically see that there are two Os for the first one, so you multiply the right hand side of the equation by 2
_Mg+ _1_ 2O = 2MgO

Answer 49

But then, because of this, there are 2 Mgs, which brings you to have to multiply the first one by 2

So the blanks are 2, 1, and 2

Answer 50

:> you let her do the work- please so she can learn how to do it o:

Answer 51

Because she doesn't know how to do it, I'm explaining to her, so she can read it through to understand

Answer 52

mk... Hard to understand but Okay...

Answer 53

I got tagged to this post but it seems like that reply was deleted.

What part of balancing chemical equations are you still confused about?

Answer 54

\(\color{#0cbb34}{\text{Originally Posted by}}\) @Astrid1
So for number one.
\[ 2H _{2} + O _{2} \rightarrow H _{2}O\]

H=2 H=2

O=2 O=1

H=4 H=4

O=2 O=2

Right?
\(\color{#0cbb34}{\text{End of Quote}}\)


I have no idea what you're counting and why you have re-written the same elements multiple times

Let's start all over again

This is what we're given
\(\sf 2 H_2 + \text{__}O_2 \to \text{__}H_2O\)

What do we have on the left hand side of the arrow?

We have \(\sf 2 H_2\) and \(\sf O_2\)

How many H's are there in \(\sf H_2\)
There are 2 H's in \(\sf H_2\)

But how many \(\sf H_2\) do we have? We have \(\sf 2 H_2\) so that means we have a total of 4 H's

How many O's do we have in \(\sf O_2\)

We have 2 O's in \(\sf O_2\)

Answer 55

Now let's look at the right hand side after the arrow

We have \(\sf H_2O\)

How many H's do we have?
We have 2 H's

How many O's do we have?
We have 1 O

Answer 56

Now let's compare the left side to the right side



Do you see how we have 4 H's on the left side but only 2 on the right side?

We also have 2 O's on the left side but only 1 on the right side


So what number do you need to multiply the \(\sf H_2O\) by so that way you can double it so you have the same number of H's and O's on both sides