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
Evgen [1.6K]
3 years ago
9

Of the​ rock's original​ uranium-235 remains. how old is the​ rock

Chemistry
1 answer:
Gemiola [76]3 years ago
5 0
2.1 billion years
2,139,000,000 to be exact
You might be interested in
16. Which is an example of a transverse wave? (1 point)
GarryVolchara [31]

Answer:

<h2>Transverse wave,</h2>

Explanation:

<h3>motion in which all points on a wave oscillate along paths at right angles to the direction of the wave's advance. Surface ripples on water, seismic S (secondary) waves, and electromagnetic (e.g., radio and light) waves are examples of transverse waves.</h3>
7 0
2 years ago
Read 2 more answers
The sodium atom loses an electron to form a sodium Ion (Na+). Which statement is correct with respect to its atomic radius?
SCORPION-xisa [38]

Answer:

sodium ion has smaller radius than a atom.

Explanation:

6 0
2 years ago
How do you find the molar mass for ba(NO3)2
Korvikt [17]
To find the molar mass<span> of </span>Ba(NO3)2<span>, determine the </span>molar masses of all the atoms that form it. The Molar mass for Barium nitrate is <span>261.337 g/mol.</span>
8 0
3 years ago
To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.6-L bulb, then filled
aleksandrvk [35]

Answer:

The gas was N₂

Explanation:

V = 3.6L

P = 2.0 atm

T = 24.0°C = 297K

R = 0.0821 L.atm/K.mol

m = 8.3g

M = molar mass = ?

Using ideal gas equation;

PV = nRT

n = no. Of moles = mass / molar mass

n = m/M

PV = m/M * RT

M = mRT / PV

M = (8.3*0.0821*297) / (2.0*3.6)

M = 28.10

Since X is a diatomic molecule

M = 28.10 / 2 = 14.05 g/mol

M = Nitrogen

X = N₂

5 0
2 years ago
At 298 K, the osmotic pressure of a glucose solution (C6H12O6 (aq)) is 12.1 atm. Calculate the freezing point of the solution. T
Anarel [89]

<u>Answer:</u> The freezing point of solution is -0.974°C

<u>Explanation:</u>

  • To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

where,

\pi = osmotic pressure of the solution = 12.1 atm

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature of the solution = 298 K

Putting values in above equation, we get:

12.1atm=1\times M\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K\\\\M=\frac{12.1}{1\times 0.0821\times 298}=0.495M

This means that 0.495 moles of glucose is present in 1 L or 1000 mL of solution

  • To calculate the mass of solution, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Density of solution = 1.034 g/mL

Volume of solution = 1000 mL

Putting values in above equation, we get:

1.034g/mL=\frac{\text{Mass of solution}}{1000mL}\\\\\text{Mass of solution}=(1.034g/mL\times 1000mL)=1034g

  • To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of glucose = 0.495 moles

Molar mass of glucose = 180.16 g/mol

Putting values in above equation, we get:

0.495mol=\frac{\text{Mass of glucose}}{180.16g/mol}\\\\\text{Mass of glucose}=(0.495mol\times 180.16g/mol)=89.18g

Depression in freezing point is defined as the difference in the freezing point of pure solution and freezing point of solution.

  • The equation used to calculate depression in freezing point follows:

\Delta T_f=\text{Freezing point of pure solution}-\text{Freezing point of solution}

To calculate the depression in freezing point, we use the equation:

\Delta T_f=iK_fm

Or,

\text{Freezing point of pure solution}-\text{Freezing point of solution}=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}

where,

Freezing point of pure solution = 0°C

i = Vant hoff factor = 1 (For non-electrolytes)

K_f = molal freezing point elevation constant = 1.86°C/m

m_{solute} = Given mass of solute (glucose) = 89.18 g

M_{solute} = Molar mass of solute (glucose) = 180.16  g/mol

W_{solvent} = Mass of solvent (water) = [1034 - 89.18] g = 944.82 g

Putting values in above equation, we get:

0-\text{Freezing point of solution}=1\times 1.86^oC/m\times \frac{89.18\times 1000}{180.16g/mol\times 944.82}\\\\\text{Freezing point of solution}=-0.974^oC

Hence, the freezing point of solution is -0.974°C

8 0
3 years ago
Other questions:
  • 8. (16 pts.) Using sentences, compare a dipeptide to a fatty acids specifically in terms of water
    10·1 answer
  • If sea water has a density of 1.025 kg/L and 3.5% of the mass in sea water is salt, determine the mass of salt dissolved in 500
    7·1 answer
  • How many milliliters of 0.111 m hclo4 solution are needed to neutralize 50.00 ml of 0.0789 m naoh?
    8·1 answer
  • How do you classify a substance with a pH of 3?
    11·1 answer
  • Which of the following is best described by the term macroscopic?
    10·1 answer
  • PLS PLS PLS PLS HELP IM STRUGGLING
    15·1 answer
  • What amount of ice must be added to 250 g of water at 15°c to cool the water to 0°c and have no ice left
    5·1 answer
  • Compare the properties of elements in groups 17 and group 18. Make sure to cover the following points:
    7·2 answers
  • Importancia de la química orgánica en el desarrollo de los seres vivos.
    12·1 answer
  • Please follow me thanku​
    12·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!