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crimeas [40]
3 years ago
10

1. Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions, write a balanced equation. Assume

that there will be a reaction even if you didn't see one in the lab. General equation for single-displacement reactions:
A + BX → AX + B

Ion charges: (Zn2+, Cu2+, SO42-, Al3+, Ag1+, NO31-) Answer: • zinc [Zn] + copper sulfate [Cu(SO4)] (2 points) ◦

Balanced equation: … + … → …. + …. • aluminum [Al] + copper sulfate [Cu(SO4)] (2 points) ◦

Balanced equation: … + … → …. + …. • zinc [Zn] + silver nitrate [Ag(NO3)] (2 points)

◦ Balanced equation: … + … → …. + …. • copper [Cu] + silver nitrate [Ag(NO3)] (2 points) ◦ Balanced equation: … + … → …. + ….
Chemistry
1 answer:
natima [27]3 years ago
6 0
Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.

- zinc [Zn] + copper sulfate [Cu(SO4<span>)
</span>Balanced equation:Zn + Cu(SO4) → Zn(SO4<span>) + Cu

- </span>aluminum [Al] + copper sulfate[Cu(SO4)]Balanced equation:2Al + 3Cu(SO4) → Al2(SO4)3<span>+ 3Cu

-  </span>zinc [Zn] + silver nitrate [Ag(NO3)]Balanced equation:Zn + 2Ag(NO3) → 2Ag + Zn(NO3)<span>2

- </span>copper [Cu] + silver nitrate [Ag(NO3)]
Balanced equation:Cu + Ag(NO3) → Cu(NO3<span>) + Ag</span>
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IRINA_888 [86]
Look in a beehive SAFELY
7 0
3 years ago
Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) +
adoni [48]

Answer:

Overall reaction equation;

2NO(g) +Cl2(g) -----> 2NOCl (g)

Explanation:

Given

1) NO(g) + Cl2(g) → NOCl2(g)

2) NOCl2(g) + NO(g) → 2NOCl(g)

Overall reaction equation;

2NO(g) +Cl2(g) -----> 2NOCl (g)

k1= [NOCl2]

k-1= [NO] [Cl2]

k2 = [NOCl2] [NO]

Equilibrium for the first equation (reaction 1)

K= k1/k-1 = [NOCl2]/[NO] [Cl2]

Therefore

[NOCl2] = k1/k-1 [NO] [Cl2]

Rate= k2× k1/k-1 [NO]^2 [Cl2]

Rate = Koverall [NO]^2 [Cl2]

Where Koverall= k1k2/k-1

3 0
3 years ago
For each process, state whether ΔH is less than (more negative), equal to, or greater than ΔE of the system. Explain.
olganol [36]

An ideal gas is cooled at constant pressure, option A. A. ΔH is less than (more negative) Δ E of the system.

∆H is the exchange in enthalpy from reactants to products A  ΔHº charge represents an addition of electricity from the reaction and from the surroundings, resulting in an endothermic response. A horrible cost for ΔHº represents the removal of power from the reaction and into the surroundings and so the reaction is exothermic.

The enthalpy of a system can not be measured right away because of the fact the inner energy consists of additives that are unknown, now not effects available, or aren't of interest in thermodynamics.

Hence, the answer is option A.

Learn more about ideal gas here:-brainly.com/question/20348074

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Disclaimer:- your question is incomplete, please see below for the complete question.

A solid yields a mixture of gases in an exothermic reaction that takes place in a container of variable volume.

A. ΔH is less than (more negative) Δ E of the system.

B. ΔH is greater than ΔE of the system.

C. ΔH is equal to ΔE of the system.

D. can't be determined without more information

7 0
1 year ago
A 44.0 ml volume of 0.25 m hbr is titrated with 0.50 m koh. calculate the ph after addition of 22.0 ml of koh at 25 ∘c.
Helga [31]
The reaction between KOH and HBr is as follows ;
KOH + HBr ---> H₂O + KBr
Stoichiometry of base to acid is 1:1 molar ratio
Both are strong acid and strong base therefore complete ionization takes place
The number of KOH moles added - 0.50 M / 1000 mL/L x 22 mL = 0.011 mol
the number of HBr moles - 0.25 M /1000 mL/L x 44 mL = 0.011 mol
the number of H⁺ ions and OH⁻ ions are equal therefore the whole amount of acid has been completely neutralised by base.
No remaining acid nor base, therefore solution is neutral.
pH = 7 
thats the pH value for a neutral solution

4 0
3 years ago
What is solvent!!?️​
Flura [38]

Answer:

Solvent, substance, ordinarily a liquid, in which other materials dissolve to form a solution.

3 0
2 years ago
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