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juin [17]
2 years ago
6

Who is good at chemistry?! HMU asap!!!​

Chemistry
1 answer:
____ [38]2 years ago
6 0
Id say i’m good i guess. send links for the brainly problems u need help with!
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You must answer all questions to get credit for this assignment. Use the notes above and/or the textbook to help you find the an
Allisa [31]

Explanation:

(1).  It is known that in a reaction equation, reactants are placed or written on left hand side and products are written on the right hand side.

For example, N_{2} + 3H_{2} \rightarrow 2NH_{3}

Hence, in a reaction equation you start with the reactants and end up with the products.

(2).  The number of atoms in a reaction will remain the same because according to the law of conservation of mass, mass of reactants will be equal to the mass of products.

Therefore, number of atoms on the reactant side will be equal to the number of atoms on product side.

7 0
3 years ago
Qofudowqfowefjwobfwofbwfofnroenennefeoiqefopne FREEE PONITTSS
Thepotemich [5.8K]
Hey lol
explanation:)))
5 0
3 years ago
Read 2 more answers
Which of the following best represents both accuracy and precision
makkiz [27]
Accuracy is when you hit as close as to the target as you can and precision is when you are on point
5 0
3 years ago
Read 2 more answers
Calculate the molarity of a solution prepared by dissolving 5.850g of solid NaCl in enough water to make 200mL of the solution?
Y_Kistochka [10]
See the attachment below. Thanks :)

6 0
3 years ago
The substance water always has a mass ratio of 11% H to 89% O. If 5.00g of a substance containing H and O was decomposed into .2
Gre4nikov [31]

Answer:

                    No the substance is not water.

Explanation:

                   The balance chemical equation for the decomposition of water is as follow;

                                           2 H₂O = 2 H₂ + O₂

Step 1: <u>Calculate moles of H₂O;</u>

               Moles  =  Mass / M.Mass

               Moles  =  5.0 g / 18.01 g/mol

               Moles  =  0.277 moles of H₂O

Step 2: <u>Calculate Moles of O₂ and H₂ produced by 0.277 moles of H₂O:</u>

According to equation,

                        2 moles of H₂O produced  =  1 mole of O₂

So,

                  0.277 moles of H₂O will produce  =  X moles of O₂

Solving for X,

                     X =  0.277 mol × 1 mol / 2 mol

                     X =  0.138 moles of O₂

Also,

According to equation,

                        2 moles of H₂O produced  =  2 mole of H₂

So,

                  0.277 moles of H₂O will produce  =  X moles of H₂

Solving for X,

                     X =  0.277 mol × 2 mol / 2 mol

                     X =  0.227 moles of H₂

Step 3: <u>Calculate Mass of O₂ and H₂ as;</u>

For O₂:

                 Mass  =  Moles × M.Mass

                 Mass  =  0.138 mol × 31.99 g/mol

                 Mass  =  4.44 g of O₂

For H₂:

                 Mass  =  Moles × M.Mass

                 Mass  =  0.227 mol × 2.01 g/mol

                 Mass  =  0.559 g of H₂

Conclusion:

                   From conclusion it is proved that the amount of H₂ produced by decomposition of 5 g of water should be 0.559 g while in statement it is less i.e. 0.290 g.

6 0
3 years ago
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