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Ksenya-84 [330]
2 years ago
9

CHEMISTRY PLEASE HELP!!!???

Chemistry
1 answer:
Montano1993 [528]2 years ago
5 0

1. Solids

- definite volume & shape

- little energy

-vibrate in place

- very incompressible


2. Liquids

- held together yet can still flow

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Current is applied to a molten mixture of AgF , FeCl2 , and AlBr3 . What is produced at each electrode? STRATEGY Rank the cation
ratelena [41]

Answer:

Cathode: Ag

Anode: Br₂

Explanation:

In the cathode must occur a reduction, so it's more likely to a metal atom be in the cathode. For the metals given the reduction reactions and the potential of reduction are:

Ag⁺ + e⁻ ⇒ Ag⁰ E° = + 0.80 V

Fe⁺² + 2e⁻ ⇒ Fe⁰ E° = - 0.44 V

Al⁺³ + 3e⁻ ⇒ Al⁰ E° = -1.66 V

As the potential for Ag is the higher, the reduction will occur for it first, so in the cathode will produce Ag.

For the anode an oxidation must occurs, so the reactions for the nonmetals are:

F₂ + 2e⁻ ⇒ 2F⁻ E° = +2.87 V

Cl₂ + 2e⁻ ⇒ 2Cl⁻ E° = +1.36 V

Br₂ + 2e⁻ ⇒ 2Br⁻ E° = +1.07 V

For oxidation, the less the E°, the faster the reaction will occur, so Br₂ will be formed in the anode.

5 0
2 years ago
In a spontaneous fusion reaction, the total mass of the products is ________________________ the mass of the original elements.
Mice21 [21]
I believe the correct term that would fit the statement would be greater than. In a spontaneous fusion reaction, the total mass of the products is greater than the mass of the original elements. This nuclear reaction involves at least two nuclei that fuses to form one nuclei having larger mass than that of the reactant.
4 0
3 years ago
What will happen to the chemical equilibrium if MgCl2 is added?
Verizon [17]
The chemical equilibrium will be unaffected 
6 0
3 years ago
what volume of N2 is required to convert 5.0L of hydrogen gas to ammonia? assume that all gases are at the same temperature and
____ [38]

Answer:

Approximately 1.7\; {\rm L}.

Explanation:

Nitrogen {\rm N_{2}}\, (g) reacts with hydrogen {\rm H_{2}}\, (g) at a 1:3 ratio to produce ammonia {\rm NH_3}\, (g):

{\rm N_{2}}\, (g) + 3\; {\rm H_{2}}\, (g) \to 2\; {\rm NH_{3}}\, (g).

The ratio between the coefficient of {\rm N_{2}}\, (g) and the coefficient of {\rm H_{2}}\, (g) is:

\begin{aligned}\frac{n({\rm N_{2}})}{n({\rm H_{2}})} = \frac{1}{3}\end{aligned}.

Under the ideal gas assumptions, the same ratio would apply to the volume of {\rm N_{2}}\, (g) and {\rm H_{2}}\, (g) in this reaction:

\begin{aligned}\frac{V({\rm N_{2}})}{V({\rm H_{2}})} = \frac{n({\rm N_{2}})}{n({\rm H_{2}})} = \frac{1}{3}\end{aligned}.

\begin{aligned}V({\rm N_{2}})= \frac{1}{3}\, V({\rm H_{2}})\end{aligned}.

Given that V({\rm H_{2}}) = 5.0\; {\rm L}:

\begin{aligned}V({\rm N_{2}}) &= \frac{1}{3}\, V({\rm H_{2}}) \\ &= \frac{1}{3}\times 5.0\; {\rm L} \\ &\approx 1.7\; {\rm L}\end{aligned}.

(Rounded to 2 significant figures.)

5 0
2 years ago
What is the concentration of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?
ss7ja [257]

Answer:

0.15 M KCl

Explanation:

(Step 1)

Convert the original volume from mL to L. Calculate the moles of the original solution.

75.0 mL / 1,000 = 0.0750 L

Molarity = moles / volume (L)

0.200 M = moles / 0.0750 L

0.0150 = moles

(Step 2)

Convert the final volume from mL to L. Calculate the final molarity.

100. mL / 1,000 = 0.100 L

Molarity = moles / volume (L)

Molarity = 0.0150 moles / 0.100 L

Molarity = 0.15 M

6 0
2 years ago
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