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Alona [7]
3 years ago
8

A more reactive metal displaces a less reactive metal from salt solution. Such reactions are called:

Chemistry
2 answers:
faust18 [17]3 years ago
8 0

Answer:

displacement reaction

motikmotik3 years ago
6 0

Answer:

Displacement Reaction.

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3 years ago
Which of the following samples of water will contain the most heat?
VMariaS [17]

Answer:

The answer is D- make sure you give good rate

6 0
2 years ago
BRAINLIEST
Kamila [148]
The density increases.

Explanation:
As you go deeper in depth, pressure increases. Density = mass/volume. The layers beneath us due to pressure get packed to the point of being very dense.
6 0
3 years ago
Read 2 more answers
0. 102 g of an unknown compound dissolved in 100. Ml of water has an osmotic pressure of 28. 1 mmhg at 20°c. Calculate the molar
Daniel [21]

The molar mass of the compound is 68 g/mol.

<h3>What is the molar mass?</h3>

The Osmotic pressure can be obtained from the relationship;

π= iCRT

π= osmotic pressure = 28.1 mmHg or 0.037 atm

i = Vant Hoff factor = 1

C = concentration = ?

R = gas constant = 0.082 atmLK-1Mol

T = temperature = 20°c + 273 = 293 K

C = π/iRT

C =  0.037/1 * 0.082  * 293

C = 0.0015 M

Now;

Number of moles = C/V = 0.0015/100 * 10^-3

= 0.015 moles

Number of moles = mass/molar mass

Molar mass =  mass/Number of moles = 0. 102 g/ 0.015 moles = 68 g/mol

Learn more about molar mass:brainly.com/question/22997914

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3 0
2 years ago
A reaction at −8.0°C evolves 854.mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected.
Bas_tet [7]

Answer:  The volume of boron trifluoride gas that is collected is 18.6 L

Explanation:

According to the ideal gas equation:

PV=nRT

P = Pressure of the gas = 1 atm

V= Volume of the gas= ?

T= Temperature of the gas in kelvin =-8.0^0C=273+(-8.0)=265K

R= Gas constant = 0.0821Latm/Kmol

n=  moles of gas=  854 mmol = 0.854 mol   (1mmol=0.001mol)

1atm\times V=0.854\times 0.0821\times 265

V=18.6L

Thus volume of boron trifluoride gas that is collected is 18.6 L

5 0
2 years ago
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