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zavuch27 [327]
3 years ago
5

Which statement best describes the reaction pathway graph for endothermic reactions? mainly downhill always linear always parabo

lic mainly uphill
Chemistry
2 answers:
Nat2105 [25]3 years ago
6 0
Endothermic reaction is a type of reaction that absorbs energy during the process. the gauge for this reaction is the change in enthalpy which should be positive. This means the energy of the products should be greater than the energy of the reactants. The graph illustrates an uphill form. 
butalik [34]3 years ago
5 0
I think the correct answer would be always parabolic. The reaction pathway graph for an endothermic reaction would always be parabolic where the products have higher energy than the reactants. Hope this answers the question.
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Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a different temperature with initial conc
Anni [7]

Answer:

Ka = 4.76108

Explanation:

  • CO(g) + 2H2(g) ↔ CH3OH(g)

∴ Keq = [CH3OH(g)] / [H2(g)]²[CO(g)]

                      [ ]initial         change         [ ]eq

CO(g)              0.27 M       0.27 - x        0.27 - x

H2(g)              0.49 M       0.49 - x        0.49 - x

CH3OH(g)          0                0 + x               x = 0.11 M

replacing in Ka:

⇒ Ka = ( x ) / (0.49 - x)²(0.27 - x)

⇒ Ka = (0.11) / (0.49 - 0.11)² (0.27 - 0.11)

⇒ Ka = (0.11) / (0.38)²(0.16)

⇒ Ka = 4.76108

7 0
3 years ago
Ammonia can be produced in the laboratory by heating ammonium chloride
AnnyKZ [126]

Answer:

Mass = 2.89 g

Explanation:

Given data:

Mass of NH₄Cl = 8.939 g

Mass of Ca(OH)₂ = 7.48 g

Mass of ammonia produced = ?

Solution:

2NH₄Cl   +  Ca(OH)₂     →    CaCl₂ + 2NH₃ + 2H₂O

Number of moles of NH₄Cl:

Number of moles = mass/molar mass

Number of moles = 8.939 g / 53.5 g/mol

Number of moles = 0.17 mol

Number of moles of Ca(OH)₂ :

Number of moles = mass/molar mass

Number of moles = 7.48 g / 74.1 g/mol

Number of moles = 0.10 mol

Now we will compare the moles of ammonia with both reactant.

                      NH₄Cl          :          NH₃

                          2              :           2

                         0.17          :          0.17

                   Ca(OH)₂         :          NH₃

                        1                :           2

                    0.10              :          2/1×0.10 = 0.2 mol

Less number of moles of ammonia are produced by ammonium chloride it will act as limiting reactant.

Mass of ammonia:

Mass = number of moles × molar mass

Mass = 0.17 mol × 17 g/mol

Mass = 2.89 g

6 0
2 years ago
Write the balanced equation for the equilibrium reaction for the dissociation ofsilver chloride in water, and write the K expres
Marizza181 [45]

Answer:

See explanation

Explanation:

Hello there!

In this case, since the the concentrations are not given, and not even the Ksp, we can solve this problem by setting up the chemical equation, the equilibrium constant expression and the ICE table only:

AgCl(s)\rightleftharpoons Ag^+(aq)+Cl^-(aq)

Next, the equilibrium expression according to the produced aqueous species as the solid silver chloride is not involved in there:

Ksp=[Ag^+][Cl^-]

And therefore, the ICE table, in which x stands for the molar solubility of the silver chloride:

       \ \ \ \ \ \ \ \ \ \ \ \ \ \ AgCl(s)\rightleftharpoons Ag^+(aq)+Cl^-(aq)

I          -                   0             0

C        -                   +x           +x

E        -                    x             x

Which leads to the following modified equilibrium expression:

Ksp=x^2

Unfortunately, values were not given, and they cannot be arbitrarily assigned or assumed.

Regards!

6 0
2 years ago
`You have to be careful about pouring drano down your pipes since it is mainly hydrochloric acid--you can't do it if they are ma
Zanzabum

Answer:

6.67 moles

Explanation:

Given that:-

Moles of hydrogen gas produced = 10.0 moles

According the reaction shown below:-

2Al + 6HCl\rightarrow 2AlCl_3 +3H_2

3 moles of hydrogen gas are produced when 2 moles of aluminium undergoes reaction.

Also,

1 mole of hydrogen gas are produced when \frac{2}{3} moles of aluminium undergoes reaction.

So,

10.0 moles of hydrogen gas are produced when \frac{2}{3}\times 10.0 moles of aluminium undergoes reaction.

<u>Moles of Al needed  = \frac{2}{3}\times 10.0 moles = 6.67 moles</u>

6 0
3 years ago
Are the relationships in group 7a consistent with the periodic trend that you have been studying
morpeh [17]

what is interfacial tension in liqui liquid extraction?


4 0
3 years ago
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