An incandescent bulb becomes hotter than a fluorescent bulb when turned on because in a regular incandescent bulb, there is tungsten wire where electricity is converts into heat. A regular incandescent light bulb requires 4 times more energy than a fluorescent bulb in order to produce the same amount of light. The conversion is such that for a 75-watt bulb, temperature get raised to approximately 2000 K. For such a high temperature, the radiating energy from the wire have some visible light. In such bulbs, 90% of the electricity get consumed in producing heat and only 10% produces light thus, they are not much efficient source of light.
On the other hand, fluorescent bulbs produce light with less amount of heat. In them, 40% of electricity is consumed in producing light and 60% in heat which is very less as compared to heat produced by a incandescent bulb. This is because when it get turned on, mercury atoms inside the bulb collides with electrons and produce UV light which is then converted into visible light using thin layer of phosphor power present inside the bulb. This produces low amount of heat thus, the bulb stays cooler, the bigger size of bulb also helps in dispersing heat.
Therefore, a fluorescent light bulb is not as hot as an incandescent light bulb.
Answer:
0.767 g.
Explanation:
Molarity (M) is defined as the no. of moles of solute dissolved in a 1.0 L of the solution.
M = (no. of moles of K⁺)/(Volume of the solution (L).
<em>∵ no. of moles of K⁺ = (mass/molar mass) of K⁺.</em>
<em>∴ M = (mass/molar mass) of K⁺/(Volume of the solution (L).</em>
<em></em>
M = 0.0044 M.
Volume of the solution = 4459.0 mL = 4.459 L.
mass of K⁺ = ??? g.
molar mass of K⁺ = 39.01 g/mol.
∴ mass of K⁺ = (M)((molar mass of K⁺)(volume of the solution (L)) = (0.0044 M)(39.10 g/mol)(4.459 L) = 0.767 g.
Structural formula: Attached image
The type of organic reaction is <u>esterification</u>
Answer:
so with every stoichiometry problem with a mass it will make it so you can do the conversion factor with reactants or products.
if you dont understand unit conversions try to study how to set it up. anyways
a.) C12H22O11 has a mass of 342.01 Grams per mole
divide 1.202 G by 342.01 G to get 0.004 miles
b.) you're just taking the AMU of each element in the chemical multiply it by how many there is of it in the chemical, then divide it by the mass of a mole of the chemical.
c.) you take your answers of part b and multiply them by Avogadro's number
