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o-na [289]
3 years ago
10

Demand decreases and competition increases are factors that cause a shift in the quantity supplied (true or false)

Chemistry
1 answer:
Pavlova-9 [17]3 years ago
4 0

Answer is: true.

Demand decreases and competition increases decrease the quantity supplied.

Quantity supplied is the quantity of a commodity that producers are willing to sell at a particular price at a particular point of time.

Quantity demanded is the quantity of a commodity that people are willing to buy at a particular price at a particular point of time.

Quantity demanded can change at the same price depending upon factors like recession, changes in the taste of the consumer.

Competition is rivalry between two or more economic groups.

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(b) Data has been collected to show that at a given wavelength in a 1 cm pathlength cell, Beer's Law for the absorbance of Co2+
OlgaM077 [116]

Answer : The concentration of a solution with an absorbance of 0.460 is, 0.177 M

Explanation :

Using Beer-Lambert's law :

A=\epsilon \times C\times l

where,

A = absorbance of solution

C = concentration of solution

l = path length

\epsilon = molar absorptivity coefficient

From this we conclude that absorbance of solution is directly proportional to the concentration of solution at constant path length.

Thus, the relation between absorbance and concentration of solution will be:

\frac{A_1}{A_2}=\frac{C_1}{C_2}

Given:

A_1 = 0.350

A_2 = 0.460

C_1 = 0.135 M

C_2 = ?

Now put all the given values in the above formula, we get:

\frac{0.350}{0.460}=\frac{0.135}{C_2}

C_1=0.177M

Therefore, the concentration of a solution with an absorbance of 0.460 is, 0.177 M

3 0
3 years ago
WILL GIVE BRAINLIEST
dedylja [7]

Answer:

In order to be able to solve this problem, you will need to know the value of water's specific heat, which is listed as

c=4.18Jg∘C

Now, let's assume that you don't know the equation that allows you to plug in your values and find how much heat would be needed to heat that much water by that many degrees Celsius.

Take a look at the specific heat of water. As you know, a substance's specific heat tells you how much heat is needed in order to increase the temperature of 1 g of that substance by 1∘C.

In water's case, you need to provide 4.18 J of heat per gram of water to increase its temperature by 1∘C.

What if you wanted to increase the temperature of 1 g of water by 2∘C ?

This will account for increasing the temperature of the first gram of the sample by n∘C, of the the second gramby n∘C, of the third gram by n∘C, and so on until you reach m grams of water.

And there you have it. The equation that describes all this will thus be

q=m⋅c⋅ΔT , where

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m - the mass of the sample

c - the specific heat of the substance

ΔT - the change in temperature, defined as final temperature minus initial temperature

In your case, you will have

q=100.0g⋅4.18Jg∘C⋅(50.0−25.0)∘C

q=10,450 J

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3 years ago
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