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emmasim [6.3K]
3 years ago
9

What type of star has an absolute brightness of 5 and a surface temperature around 3,000 °C?

Chemistry
2 answers:
NikAS [45]3 years ago
7 0

Answer : The correct answer is option A : Supergiants

Explanation :

In the above graph absolute brightness is marked on y-axis and surface temperature is marked on x-axis.

To find out what type of star has an absolute brightness of 5 and a surface temperature around 3,000 °C, we will draw a straight line from x axis which represents a temperature of 3,000 °C and another straight line from y-axis which represents absolute brightness of 5.

From the attached graph we can see that these 2 lines meet in the region shown by Supergiants

Therefore we can say that, Supergiants has an absolute brightness of 5 and a surface temperature around 3,000 °C

pav-90 [236]3 years ago
3 0
From the graph. the answer is
A. supergiants
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Which shows the formula for an Organic acid
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Answer:
            The formula of Organic acid is as follow,

                                                 R-COOH

Explanation:
                   The class of organic acids is called Carboxylic Acids. In above general structure, R is alkyl group and can vary. While -COOH is the functional group. 
                    Carboxylic Acids has the tendency to loose protons and their pKa value depends upon the alkyl group. For example the pKa value of Acetic acid (R = -CH₃) is 4.7. The driving force for this acidity is the stability of carboxylate (conjugate base) due resonance. i.e

                               RCOOH     ⇄    RCOO⁻  +  H⁺
Where;
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3 0
3 years ago
0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, C2O42-, and they react according to the equation: Fe3+(aq) + 3 C2O42-(
Studentka2010 [4]

Answer : The concentration of Fe^{3+} at equilibrium is 0 M.

Solution :  Given,

Concentration of Fe^{3+} = 0.0200 M

Concentration of C_2O_4^{2-} = 1.00 M

The given equilibrium reaction is,

                            Fe^{3+}(aq)+3C_2O_4^{2-}(aq)\rightleftharpoons [Fe(C_2O_4)_3]^{3-}(aq)

Initially conc.       0.02         1.00                   0

At eqm.             (0.02-x)    (1.00-3x)                x

The expression of K_c will be,

K_c=\frac{[[Fe(C_2O_4)_3]^{3-}]}{[C_2O_4^{2-}]^3[Fe^{3+}]}

1.67\times 10^{20}=\frac{(x)^2}{(1.00-3x)^3\times (0.02-x)}

By solving the term, we get:

x=0.02M

Concentration of Fe^{3+} at equilibrium = 0.02 - x = 0.02 - 0.02 = 0 M

Therefore, the concentration of Fe^{3+} at equilibrium is 0 M.

4 0
3 years ago
Manganese forms several oxides when combined with oxygen. One of the oxides (Oxide 1) contains 63.2% of Mn and another oxide (Ox
Nina [5.8K]

Explanation:

Defining law of definite proportions, it states that when two elements form more than one compound, the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.

A. One of the oxides (Oxide 1) contains 63.2% of Mn.

Mass of the oxide = 100g

Mass of Mn = 63.2 g

Mass of O = 100 - 63.2

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Ratio of Mn to O = 63.2/36.8

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Another oxide (Oxide 2) contains 77.5% Mn.

Mass of oxide = 100 g

Mass of Mn = 77.5 g

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Therefore, the ratio of the masses of Mn and O in Oxide 1 and Oxide 2 is in the ratio 1.72 : 3.44, which is also 1 : 2. So the law of multiple proportions is obeyed.

B.

Oxide 1

Mass of Mn per 1 g of O = mass of Mn/mass of O

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Oxide 2

Mass of Mn per 1 g of O = mass of Mn/mass of O

= 77.5/22.5

= 3.44 g/g of Oxygen.

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3 years ago
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Which formula equation represents the burning of sulfur to produce sulfur dioxide?
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Answer:

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Upper S (s) plus upper O subscript 2 (g) right arrow with delta above upper S upper O subscript 2 (g).

Explanation:

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S(s) + O2(g) --> SO2(g)

The crrect option is option A. Upper S (s) plus upper O subscript 2 (g) right arrow with delta above upper S upper O subscript 2 (g).

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3 years ago
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