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4 years ago

. Waves with shorter wavelengths have what frequencies a. Lower b. Higher

Chemistry

2 answers:

Setler79 [48]4 years ago

6 0

Answer:

Option b. Higher

Explanation:

The relationship between wavelength and frequency can be determined by the formula:

Velocity = wavelength x frequency

Frequency = Velocity /wavelength

From the above illustration,

Frequency is inversely proportional to the wavelength. That is, as the frequency increase, the wavelength will decrease and also as the frequency decreases, the wavelength will increase.

From the question,

Shorter wavelength will have high frequency

prisoha [69]4 years ago

3 0

Answer:

B. Higher

Explanation:

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timurjin [86]

Explanation:

a) Cr is acid K is base

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3 years ago

I need help with this :/

GREYUIT [131]

Answer:

Blank 1: 1

Blank 2: 2

Blank 3: 1

Blank 4: 1

Explanation:

Assuming this is to balance the equation, write out the amount of each element you have on the reactants side and on the products side

Reactants Products

Ca 1 Ca 1

C 2 C 2

H 2 H 4

O 1 O 2

Comparing the two, we can see that hydrogen and oxygen have different amounts between reactants and products. Therefore, we need to multiply by some number to get the two equal. If we multiply the reactants by 2 we will get the correct amount in the products. So we put a 2 in front of the H₂O to signify this.

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CaC₂ + 2 H₂O --> C₂H₂ + Ca(OH)₂

8 0

3 years ago

the osmotic pressure ofa solution containing 5.87 mg of an unknown protein per 10ml of solution is 2.45 torr at 25 degree celsiu

Neko [114]

Answer: The molar mass of the unknown protein is $4.45\times 10^9g/mol$

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 = 2.45 torr

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

Mass of solute (protein) = 5.87 mg = 5870 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 10 mL

R = Gas constant = $62.364\text{ L.torr }mol^{-1}K^{-1}$

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

Putting values in above equation, we get:

$2.45torr=1\times \frac{5870\times 1000}{\text{Molar mass of protein}\times 10}\times 62.364\text{ L.torr}mol^{-1}K^{-1}\times 298K\\\\\text{molar mass of protein}=4.45\times 10^9g/mol$