Question

How many milliliters of sodium metal, with a density of 0.97 g/mL, would be needed to produce 53.2 grams of hydrogen gas in the single-replacement reaction below? Show all steps of your calculation as well as the final answer.

Na + H2O → NaOH + H2

Answer 1

@Abhisar can you check my explanation for this question?

Answer 2

Step:
1. Use the formula: Number of Moles=Mass(g)/Molar Mass(g/mol)
2. So then you have to plug in the numbers from the question to the formula, it should look like this 53.2/2=26.6
3. Then take a look at the Mole Ratio of Na:H2
4. The ratio is 2:1
5. x:26.6
6. Then you multiple to find the moles 26.6 X 2/1=53.2 moles
7. Next use this formula to solve for mass: Mass(g)=Molar Mass(g/mol) X Number of moles
8. Plug in the numbers to the equation from above to find the grams of Sodium 53.2*23.0=1223.6 grams of Sodium
9. Use this formula to determine the density: Density=Mass/Volume
10. Plug in the information from the question to the formula to find density: 1223.6/V=0.97
0.97V=1223.6
11. Then you come up with your answer!: V=1261.4 ml

Answer 3

Did u balanced the equation first ?

Answer 4

no i forgot, is it 2 Na + 2 HOH --> 2NaOH + H2

Answer 5

yep !

Answer 6

so do I do those steps after i balanced the equation

Answer 7

Getting it ?

Answer 8

how do i figure out how many grams of sodium metal is required to react with 1 gram of hydrogen gasw many

Answer 9

By comparing the ratios, i showed that in ur last question.

Answer 10

oh

Answer 11

let me go back to that

Answer 12

Sorry there is an error in the steps i mentioned !

Answer 13

\(\color{blue}{\text{Originally Posted by}}\) @Abhisar
\(\large \sf \ Step~1\)
Find how many grams of sodium metal is required to produce 1 gram of hydrogen gas
\(\color{blue}{\text{End of Quote}}\)

Answer 14

\(\color{blue}{\text{Originally Posted by}}\) @Abhisar
\(\large \sf \ Step~2\)
Find how many grams of sodium metal is required to produce 53.2 grams of hydrogen.
\(\color{blue}{\text{End of Quote}}\)

Answer 15

\(\color{blue}{\text{Originally Posted by}}\) @Abhisar
\(\large \sf \ Step~3\)
Convert the mass (grams) of sodium metal into volume (ml) by using given density.
\(\color{blue}{\text{End of Quote}}\)

Answer 16

2 moles of Na are required to produce 1 mole of Hydrogen, i.e 45.97 grams of Na is required to produce 2 gram of hydrogen.

Answer 17

so 22.98 grams of Na is required for producing 1 gram of hydrogen. Can u solve it futher ?

Answer 18

*further

Answer 19

let me see

Answer 20

i am stuck

Answer 21

Where ?

Answer 22

i just i don't know what do. should i set up and equation?

Answer 23

but i explained u everything in ur last question...

Answer 24

ok do one thing....rewrite the steps u know using the balanced equation.

Answer 25

\(\color{blue}{\text{Originally Posted by}}\) @superhelp101
Step:
1. Use the formula: Number of Moles=Mass(g)/Molar Mass(g/mol)
2. So then you have to plug in the numbers from the question to the formula, it should look like this 53.2/2=26.6
3. Then take a look at the Mole Ratio of Na:H2
4. The ratio is 2:1
5. x:26.6
6. Then you multiple to find the moles 26.6 X 2/1=53.2 moles
7. Next use this formula to solve for mass: Mass(g)=Molar Mass(g/mol) X Number of moles
8. Plug in the numbers to the equation from above to find the grams of Sodium 53.2*23.0=1223.6 grams of Sodium
9. Use this formula to determine the density: Density=Mass/Volume
10. Plug in the information from the question to the formula to find density: 1223.6/V=0.97
0.97V=1223.6
11. Then you come up with your answer!: V=1261.4 ml
\(\color{blue}{\text{End of Quote}}\)

Answer 26

correct these one

Answer 27

brb..then i'll check

Answer 28

correct what? i want to go back to my last question but idk how, do i just go on closed questions :/

Answer 29

1. Na + H2O → NaOH + H2
in mol grams
2. 23 + 18 → 40 + 2
3. You need 23 gr of Na to produce 2 gr of H2, and you will need = 53.2*23/2 = 611.8 gr of Na to yield 53.2 gr of H2

4. 611.8 * 0.97 = 593.45 ml of Na
is this right?

Answer 30

@Abmon98 what do i need to do?

Answer 31

1. Na + H2O → NaOH + H2
in mol grams
2. 23 + 18 → 40 + 2
3. You need 23 gr of Na to produce 2 gr of H2, and you will need = 53.2*23/2 = 611.8 gr of Na to yield 53.2 gr of H2

4. 611.8 * 0.97 = 593.45 ml of Na
Thats an incorrect method of solving you need to first find the number of moles or the amount that reacted to produce 53.2 moles of hydrogen not just from the atomic weight and then comparing ratios.

Answer 32

oh oops

Answer 33

\(\color{blue}{\text{Originally Posted by}}\) @superhelp101
1. 2Na + 2H2O → 2NaOH + H2
in mol grams
2. You need 46 gr of Na to produce 2 gr of H2, and you will need = 23 g of Na to produce 1 g of H2

Answer 34

What you need to do is to solve to obtain the number of moles of hydrogen, use mole ratio from the balanced chemical equation. Use Number of moles=Mass(g)/Molar Mass(g/mol)
to find out the mass of sodium consumed to produce 53.2 grams of hydrogen and use Density=mass/volume. Density is provided and mass too solve to get volume

Answer 35

@Abmon98 i see i will have to do that. @Abhisar do you agree?

Answer 36

yeah obvsly !
:) check the steps i told u above..same thing !

Answer 37

ah. ok. thank you both!!!!!!!!!!!!! i wish i can best response you both :'(

Answer 38

aah..it's ok :)

Answer 39

Your welcome :D