1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Bogdan [553]
3 years ago
5

Brass is an example of

Chemistry
1 answer:
topjm [15]3 years ago
6 0
Brass is an example of homogeneous mixture.
You might be interested in
How many grams of NaOH are contained in 500 mL of a 0.80 M sodium hydroxide solution?
4vir4ik [10]

This is molarity: moles of solute/liters of solution. (Not molality)

1. Plug in what we know:

500 mL = 0.5 L

0.80 = moles/0.5

0.80*0.5 = moles

moles = 0.4

2. NaOH is given as 40 g/mole, so calculate the grams:

0.4 * 40 = 16 grams

answer: 16 grams

7 0
2 years ago
What information does a balanced equation provide?
MakcuM [25]

Answer:

It has to have a problem base and a realistic explanation.

Explanation:

It needs to have enough information for you to be able to come up with an answer and realistic explanation.

Hope I helped :)

6 0
3 years ago
Read 2 more answers
If 1.0 gram of hydrogen reacts with 19.0 grams of fluorine, then what is the percent by mass of fluorine in the compound that is
astraxan [27]
The reaction between hydrogen (H2) and fluorine (F2) is given below,
                                   H2 + F2 ---> 2HF
One mole of both hydrogen and fluorine yields to 2 moles of hydrogen fluoride. This can also be expressed as, 2 grams of hydrogen and 38 grams of fluorine will form 40 grams of hydrogen fluoride. From the given, only 20 grams of HF is formed with 19 g of it being fluorine. Thus, the percentage fluorine of the compound formed is 95%. 
8 0
3 years ago
Read 2 more answers
Consider 2H2 + O2 → 2H2O. To produce 1.2 g water, how many grams of H2 are required? Report to the correct number of significant
Elden [556K]

Answer:

0.133 mol (corrected to 3 sig.fig)

Explanation:

Take the atomic mass of H=1.0, and O=16.0,

no. of moles = mass / molar mass

so no. of moles of H2O produced = 1.2 / (1.0x2+16.0)

= 0.0666666 mol

From the equation, the mole ratio of H2:H2O = 2:2 = 1:1,

meaning every 1 mole of H2 reacted gives out 1 mole of water.

So, the no, of moles of H2 required should equal to the no, of moles of H2O produced, which is also  0.0666666 moles.

mass = no. of moles x molar mass

hence,

mass of H2 required = 0.066666666 x (1.0x2)

= 0.133 mol (corrected to 3 sig.fig)

3 0
3 years ago
Is an alpha a product or reactant when released from an isotope
trasher [3.6K]

Answer:

Alpha decay

Explanation:

That's the definition of alpha decay

6 0
3 years ago
Other questions:
  • Given that the rate constant is 4.0×10−4 m−1 s−1 at 25.0 ∘c and that the rate constant is 2.6×10−3 m−1 s−1 at 42.4 ∘c, what is t
    11·1 answer
  • Given the reaction: mg(s) 2 agno3(aq)--> mg(no3)2(aq) 2 ag(s) which type of reaction is represented? (1) single replacement (
    8·1 answer
  • A certain element exists as two different isotopes. 76.00% of its atoms have a mass of 35.00 amu and 24.00% of its atoms have a
    11·1 answer
  • An object with a mass of 7.1 g raises the level of water in a graduated cylinder from 25.1 mL to 32.4 mL. What is the density of
    9·1 answer
  • What is the electrical power generated from a voltage of 12.3 V if the current is 9.42 amps
    14·1 answer
  • Why dil. sulphuric acid cannot be used instead of dil.hcl in lab preparation of carbon dioxide gas?​
    8·1 answer
  • A home is heated by a system that uses sunlight to warm water in pipes. Which statement best describes this system?
    5·2 answers
  • I have to make this question longer so im just typing thisgjfgjfjvndfi nufnvfjnvfjnjn vnfj
    14·2 answers
  • What is the maximum amount of energy that could be produced from the reaction of 85.0 grams of Aluminum with 95.0 grams of oxyge
    8·1 answer
  • Please help<br><br> Give an example of a physical and a chemical reaction.
    6·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!