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
OlgaM077 [116]
2 years ago
7

A force is applied but nothing happens

Chemistry
1 answer:
Lana71 [14]2 years ago
7 0
If a force is applied but nothing happens, then it means that the forces are balanced. Being at such state, <span>equal forces are acting on an object in opposite directions. Hope this answers the question. Have a nice day. Feel free to ask more questions.</span>
You might be interested in
How many moles are in 16.94g of water?
alexira [117]

16.94/18=.9411111

sig figs: 0.9411 mole of water

7 0
3 years ago
If you dissolve 50.0 grams of potassium bromide in 100.0g of water what is the mass percent of the resultant solution?
tatiyna
Mass percent= grams solute/ grams of solution x 100

Mass Percent= (50/ 150)x100= 33.3%
7 0
2 years ago
Quinine, an antimalarial drug, is 8.63% nitrogen. There are two nitrogen atoms per molecule. What is the molecular weight of qui
Furkat [3]

Answer:

324.18 g/mol

Explanation:

Let the molecular mass of the antimalarial drug, Quinine is x g/mol

According to question,

Nitrogen present in the drug is 8.63% of x

So, mass of nitrogen = \frac {8.63}{100}\times x

Also, according to the question,

2 atoms are present in 1 molecule of the drug.

Mass of nitrogen = 14.01 amu = 14.01 g/mol (grams for 1 mole)

So, mass of nitrogen = 14.01×2 = 28.02

These 2 must be equal so,

\frac {8.63}{100}\times x=28.02

solving for x, we get:

<u>x = 324.18 g/mol</u>

6 0
3 years ago
Why does the hull of an ocean -going ship rust quickly?
stepan [7]
Metal rusts when it oxidized around moisture.
4 0
2 years ago
Calculate the percent yield when 500 grams of carbon dioxide react with an excess of water to produce 640 grams of carbonic acid
Elena-2011 [213]

Answer:

Percent yield =  90.5%

Explanation:

Given data:

Mass of carbon dioxide = 500 g

Mass of water = excess

Actual yield of carbonic acid = 640 g

Percent yield = ?

Solution:

Balanced chemical equation:

CO₂ + H₂O  → H₂CO₃

Number of moles of carbon dioxide

Number of moles  = Mass / molar mass

Number of moles = 500 g/ 44 g/mol

Number of moles = 11.4 mol

Now we will compare the moles of H₂CO₃ with CO₂.

                              CO₂          :              H₂CO₃

                                 1             :                  1

                               11.4           :                11.4

Mass of carbonic acid:

Mass = number of moles × molar mass

Mass = 11.4 mol × 62.03 g/mol

Mass = 707.14 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield =  640 g/ 707.14 g × 100

Percent yield =  90.5%

7 0
3 years ago
Other questions:
  • What product of Al makes it suiyable to be used in electric cables
    13·1 answer
  • In an experiment, Lydia added 50 grams of sugar to 200 milliliters of water. She stirred the mixture, and the sugar eventually d
    6·1 answer
  • Using Carbon cycle what carbon trapped in fossil fuels is converted to carbon dioxide
    10·1 answer
  • Determine the empirical formula of a compound containing 48.38 grams of carbon, 8.12 grams of hydrogen, and 53.5 grams of oxygen
    6·1 answer
  • How would you prepare a 0.1M solution of HCl starting with a 1.0M solution? Assume you want to prepare 100 ml of solution.
    6·1 answer
  • Plants do not adapt to their environment because they do not compete for resources.
    7·1 answer
  • Which best describes a radioactive isotope?
    7·1 answer
  • How can the Swartz process be modified to work for bacteria? Explain.​
    14·1 answer
  • All three types of rock form in which earth layer?
    12·1 answer
  • 750.0g of water that was just boiled (heated to 100.0/c loses 78.45KJ of heat as it cools.What is the final temperature of water
    15·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!