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3241004551 [841]
3 years ago
8

What does the absolute magnitude of a star depend on?

Chemistry
1 answer:
Serggg [28]3 years ago
8 0
C. Distance from Earth

The observed brightness of a star (the apparent magnitude) to an absolute magnitude, you need to know the distance [d], to the star. Alternatively, if we know the distance and the apparent magnitude [m] of a star, we can calculate its absolute magnitude [d].

*paraphrased from "COSMOS.com"
You might be interested in
What would be the mass, in grams, of 3.50 x 1025 molecules of chlorine?<br><br> Show your work
Maurinko [17]

Answer:

2059.645g Cl

Explanation:

A mole of any element contains 6.022e23 molecules, so we will divide the given amount of molecules by 6.022e23.

3.5e25 / 6.022e23 = 5.81e1

5.81e1 = 58.1 mol Cl

Now that we have found the amount of moles of Chlorine, we will multiply the number of moles by the molar mass of Chlorine, which is 35.45g/mol.

35.45(58.1) = 2059.645g Cl

4 0
2 years ago
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e
Sonbull [250]

Answer:

Option (B) is correct

Explanation:

Oxidation: Zn\rightarrow Zn^{2+}+2e^{-}

Reduction: Sn^{2+}+2e^{-}\rightarrow Sn

---------------------------------------------------------------------------

Overall: Zn+Sn^{2+}\rightarrow Zn^{2+}+Sn

Nernst equation for this cell reaction at 25^{0}\textrm{C}:

E_{cell}=(E_{Sn^{2+}\mid Sn}^{0}-E_{Zn^{2+}\mid Zn}^{0})-\frac{0.059}{n}log\frac{[Zn^{2+}]}{[Sn^{2+}]}

Where, n is number of electron exchanged and species inside third bracket represents concentrations in molarity.

Here, n = 2, E_{cell}=0.660V and [Zn^{2+}]=2.5\times 10^{-3}M

So, plug in all the given values into above equation:

0.660V=(-0.136V+0.76V)-\frac{0.059}{2}log\frac{2.5\times 10^{-3}M}{[Sn^{2+}]}

So, [Sn^{2+}]=4.2\times 10^{-2}M

As the value "0.059" varies from literature to literature and 4.2\times 10^{-2}M is most closest to 3.3\times 10^{-2}M therefore option (B) is correct.

8 0
3 years ago
What volume of 0.0748 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?
Irina18 [472]

Answer:

0.375 L

Explanation:

We know that at neutralization, the number of mol  of acid must equal the number of equivalents of base.

This is a reaction 1:1 acid to base:

HClO₄ + NaOH ⇒ NaClO₄ + H₂O

We re given the  moles  of the base indirectly since we know the volume and molarity. From there we can calculate the volume of HClO₄.

Moles NaOH = 0.115 L x 0.244 M = 0.115 L x 0.244 mol/L =0.028 mol

Thus we require 0.028 mol of HClO₄ in the pechloric acid solution:

Molarity = # moles / V ⇒ V = # moles / M

V = 0.028 mol / 0.0748 mol/L = 0.375 L

Note  that this problem can be solved in just one step since

M(HClO₄) x V(HClO₄) = M(NaOH) x V(NaOH)  ⇒

V(HClO₄) = M(NaOH) x V(NaOH) / M(HClO₄)

5 0
2 years ago
What is the correct reaction for the dissociation (ionization) for a weak acid?
slava [35]

Answer: HA + H2O ⇌ H3O+ + H- (option #4)

Explanation: Since the acid is weak you have to use a ⇌ (equilibrium) sign. Equilibrium is denoted in a chemical equation by the ⇌ symbol. Also, when any acid dissolves into water, it produces hydronium (H3O+ or H+). Therefore, the fourth chemical reaction is your answer.

7 0
3 years ago
What is the molarity of 3.2 moles of magnesium chloride in 1.5 L of water
diamong [38]

Answer:4.8

Explanation:

5 0
3 years ago
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