Question

$\huge \fbox \red{❥ Question}$

◍Wʀɪᴛᴇ Aʙᴏᴜᴛ Hᴇɴʀʏ
ᴡɪᴛʜ ғᴜʟʟ ᴇxᴘʟᴀɴᴀᴛɪᴏɴ..

◍ɴᴏ sᴘᴀᴍ ɪғ ʏᴏᴜ sᴘᴀᴍ ɪs ʀᴇᴘᴏʀᴛ ᴛʜᴇʀᴇ 10 ᴀɴsᴡᴇʀs..

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Answer 1

Answer:

Henry, pseudonym of William Sydney Porter, original name William Sidney Porter, (born September 11, 1862, Greensboro, North Carolina, U.S.—died June 5, 1910, New York, New York), American short-story writer whose tales romanticized the commonplace—in particular the life of ordinary people in New York City. His stories expressed the effect of coincidence on character through humour, grim or ironic, and often had surprise endings, a device that became identified with his name and cost him critical favour when its vogue had passed.

Answer 2

Henry's law is one of the gas laws, formulated by the British chemist, William Henry, in 1803. It states that:

At a constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.

[edit]Formula and Henry constant

A formula for Henry's law is:

e^p = e^{k_{\rm H}}\;c

where:

e\, is approximately 2.7182818, the base of the natural logarithm (also called Euler's number)

p\, is the partial pressure of the solute above the solution

c\, is the concentration of the solute in the solution (in one of its many units)

k_{\rm H}\, is the Henry's law constant, which has units such as L·atm/mol, atm/mole fraction or Pa·m3/mol.

Taking the natural logarithm of the formula, gives us the more commonly used formula:[1][2][3][4]

p = k_{\rm H}\;c

Some values for k_{\rm H}\, include:

oxygen (O2) : 769.2 L·atm/mol

carbon dioxide (CO2) : 29.4 L·atm/mol

hydrogen (H2) : 1282.1 L·atm/mol

when these gases are dissolved in water at 298 kelvins.

As shown in Table 1 below, there are other forms of Henry's law each of which defines the constant k_{\rm H}\, differently and requires different dimensional units.[5] The form of the equation presented above is consistent with the example numerical values presented for oxygen, carbon dioxide and hydrogen and with their corresponding dimensional units.

Note that for the above values, the unit of concentration, c, was chosen to be molarity (i.e., mol/L). Hence the dimensional units: L is liters of solution, atm is the partial pressure of the gaseous solute above the solution (in atmospheres of absolute pressure), and mol is the moles of the gaseous solute in the solution. Also note that the Henry's law constant, kH, varies with the solvent and the temperature.