Answer:
the stronger light 5.5 m apart from the total illumination
Explanation:
From the problem's statement , the following equation can be deducted:
I= k/r²
where I = intensity of illumination , r= distance between the point and the light source , k = constant of proportionality
denoting 1 as the stronger light and 2 as the weaker light
I₁= k/r₁²
I₂= k/r₂²
dividing both equations
I₂/I₁ = r₁²/r₂²=(r₁/r₂)²
solving for r₁
r₁ = r₂ * √(I₂/I₁)
since we are on the line between the two light sources , the distance from the light source to the weaker light is he distance from the light source to the stronger light + distance between the lights . Thus
r₂ = r₁ + d
then
r₁ = (r₁ + d)* √(I₂/I₁)
r₁ = r₁*√(I₂/I₁) + d*√(I₂/I₁)
r₁*(1-√(I₂/I₁)) = d*√(I₂/I₁)
r₁ = d*√(I₂/I₁)/(1-√(I₂/I₁)) =
r₁ = d/[√(I₁/I₂)-1)]
since the stronger light is 9 times more intense than the weaker
I₁= 9*I₂ → I₁/I₂ = 9 →√(I₁/I₂)= 3
then since d=11 m
r₁ = d/[√(I₁/I₂)-1)] = 11 m / (3-1) = 5.5 m
r₁ = 5.5 m
therefore the stronger light 5.5 m apart from the total illumination
Answer:
b because I know this
Explanation:
trust me I am I. 6th grade straight a's
Answer:
In materials science, an intrinsic property is independent of how much of a material is present and is independent of the form of the material, e.g., one large piece or a collection of small particles. Intrinsic properties are dependent mainly on the fundamental chemical composition and structure of the material.
Explanation:
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Aldehyde is a group of organic compounds with the general form of RCHO. Oxidation of aldehyde can lead to the formation of the carboxylic acids, with the general form of RCO₂H.
With this oxidation, the typical reagents promoting the oxidation are chromic acids, chromate salts, permanganate, etc.
The balanced equation for the above reaction is as follows;
2H₂ + O₂ --> 2H₂O
stoichiometry of O₂ to H₂O is 1:2
number of O₂ moles reacted - 40.3 g / 32 g/mol = 1.26 mol
according to molar ratio
number of water moles produced = 2 x number of O₂ moles reacted
number of water moles formed - 1.26 x 2 = 2.52 mol
mass of water produced = 2.52 mol x 18 g/mol = 45.4 g
45.4 g of water produced
