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3 years ago

What is the difference between chemical reactions and nuclear decay rates

1 answer:

4 0

Nuclear decay rates are influenced by /depend on the forces that keep the nucleus together. Chemical reaction rates depend on the concentration, nature of reactants, temperature, pressure, catalysts i.e. external factors

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A reaction contains two reactants, A and B. If A is doubled, there will be a greater number of effective collisions between reac

svlad2 [7]

True true true true true

4 0

3 years ago

Substances dissolved in a solvent are correctly known as what?

KatRina [158]

Answer:

solute

Explanation:

The substance that dissolves is called the solute. The substance that dissolves it is called the solvent.

7 0

3 years ago

Difference between molar mass and molecular mass?

Elden [556K]

Answer:

In chemistry the substance is usually measured using molecular mass and molar mass. They are very important concepts in chemistry. Expression of molar mass is grams per mole.

...

Molar mass:

Difference between Molar mass and Molecular mass

Measurement given to compounds, atoms or molecules Determined only in molecules

Explanation:

hope the answer was helpful

8 0

3 years ago

How many grams of cuno3 will be required to make 1.00 l of 0.420 m solution?

7nadin3 [17]

Answer:

The answer to your question is: 52.92 g of CuNO₃

Explanation:

Data

grams of CuNO₃ = ?

volume = 1 l

concentration = 0.420 M

MW of CuNO₃ = 64 + 14 + 3(16) = 126 g

Formula

Molarity = moles / volume

moles = Molarity x volume

moles = 0.420 x 1

moles = 0.420 moles

1 mol of CuNO₃ ------------------- 126 g of CuNO₃

0.420 moles CuNO₃ ------------- x

x = (0.420 x 126) / 1

x = 52.92 g of CuNO₃

3 0

3 years ago

100. mg of an unknown protein are dissolved in enough solvent to make 5.00mL of solution. The osmotic pressure of this solution

PolarNik [594]

Answer: The molar mass of the unknown protein is 6387.9 g/mol

Explanation:

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

$\pi=iMRT$

or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 0.0766 atm

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

Mass of protein = 100. mg = 0.100 g (Conversion factor: 1 g = 1000 mg)

Molar mass of protein = ?

Volume of solution = 5.00 mL

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

T = temperature of the solution = $25^oC=[25+273]K=298K$

Putting values in above equation, we get:

$0.0766atm=1\times \frac{0.100\times 1000}{\text{Molar mass of protein}\times 5}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 298K\\\\\pi=\frac{1\times 0.100\times 1000\times 0.0821\times 298}{0.0766\times 5}=6387.9g/mol$

Hence, the molar mass of the unknown protein is 6387.9 g/mol

5 0

4 years ago