Calculate the mass of oxygen (in mg) dissolved in a 4.97 l bucket of water exposed to a pressure of 1.08 atm of air. assume the mole fraction of oxygen in air to be 0.21 and the henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 m/atm o2. (enter your value using three significant figures.)

46.9mg of oxygen

Explanation:

From Henry's law,

Concentration of oxygen (C) = Henry's constant (K) × partial pressure of oxygen in air (p)

K = 1.3×10^-3M/atm O2, p = mole fraction of oxygen in air × pressure of air = 0.21×1.08atm = 0.2268atm

C = K×p = 1.3×10^-3 × 0.2268 = 0.00029484M of O2

Concentration (C) = number of moles of oxygen (n)/volume of water (V)

Volume of water (V) = 4.97L

n = CV = 0.00029484 × 4.97 = 0.001465mole

number of moles (n) = mass of O2/MW of O2

mass of O2 = number of moles of O2 × MW of O2 = 0.001465mole × 32g/mole = 0.0469g = 0.0469×1000mg = 46.9mg (to three significant figures)

answer is: nuclear fusion produces elements that are heavier than helium.

nuclei combine to form a heavier nucleus, releasing energy.  

for example, fusion of hydrogen atoms at the sun.  

this fusion nuclear reaction is in the inner core of the sun and hydrogen (atomic number 1) is conveted into helium (atomic number 2).  

the inner core is the central region of the sun and all solar energy is produced in the core by nuclear fusion.