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Elanso [62]
3 years ago
6

18. Predict the products for this single replacement reaction.

Chemistry
1 answer:
fenix001 [56]3 years ago
3 0

Answer:

3rd response

4th response

Explanation:

i lowkey feel like im doing this whole chem exam for u lol. good luck anyway! u rock!

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Creep since it’s slow over time.
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During combustion, chemical energy stored in fossil fuels is converted into _____ energy.
Mumz [18]
During combustion, chemical energy stored in fossil fuels is converted into KINETIC energy. 
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3 years ago
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What is the rate law for the uncatalyzed reaction?
elena55 [62]

What is the rate law for the uncatalyzed reaction?

Metals often form several cations with different charges. Cerium, for example, forms and ions, and thallium forms and ions. Cerium and thallium ions react as follows:  

2Ce^4+(aq) + Tl^+(aq) ---> 2Ce^3+(aq)+Tl^3+(aq)  

This reaction is very slow and is thought to occur in a single elementary step. The reaction is catalyzed by the addition of Mn^2+ according to the following mechanism:  

Ce^4+(aq)+Mn^2+(aq) ---> Ce^3+(aq)+Mn^3+(aq)  

Ce^4+(aq)+Mn^3+(aq) ---> Ce^3+ (aq) + Mn^4+ (aq)  

Mn^4+(aq) + Tl^+(aq) ---> Mn^2+(aq) + Tl^3+(aq)  

If the uncatalyzed reaction occurs in a single elementary step, why is it a slow reaction?  

1)The probability of an effective three-particle collision is low.  

2) The transition state is low in energy.  

3) The reaction requires the collision of three particles with the correct energy and orientation.  

4) All reactions that occur in one step are slow.  

The catalyzed reaction is first order in [Ce^4+] and first order in [Mn^2+]. Which of the steps in the catalyzed mechanism is rate determining?  

Based on their available oxidation states, rank the following metals on their ability to catalyze this and other oxidation-reduction reactions.  

Rank from best to worst catalyst.  

Vanadium, titanium, manganese

4 0
3 years ago
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A 0.271g sample of an unknown vapor occupies 294ml at 140C and 874mmHg. The emperical formula of the compound is CH2. How many m
Phoenix [80]
Using PV = nRT, we can calculate the moles of the sample.
874 mmHg = 116,524 Pa
n = PV/RT
n = 116,524 x 294 x 10⁻⁶ / 8.314 x (140 + 273)
n = 9.98 x 10⁻³ mol

moles = mass / Mr
Mr = 0.271/9.98 x 10⁻³
Mr = 27.2
Mass of empirical formula = 14
Repeat units = 27.2 / 14 ≈ 2

Formula of substance:
C₂H₄

Combustion equation:
C₂H₄ + 3O₂ → 2CO₂ + 2H₂O

1 mole produces 2 moles of CO₂, so 3 moles will produce 6 moles CO₂
7 0
3 years ago
Given the atomic mass of select elements, calculate the molar mass of each salt.
arlik [135]

Answer:

See explanation

Explanation:

Molar mass is obtained as the sum of relative atomic masses as follow;

For CaBr = 40.08 + 79.90 = 119.98 g/mol

For BeBr =  9.012 + 79.90 = 88.912 g/mol

For CdBr2 = 112.41 + 2(79.90) = 272.21 g/mol

For CuBr2 = 63.55 + 2(79.90) = 223.35 g/mol

3 0
3 years ago
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