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enot [183]
3 years ago
12

How does an increase in temperature at which a reaction takes place cause an increase in reaction rate

Chemistry
1 answer:
Allisa [31]3 years ago
6 0
The collision theory explains why reactions occur between atoms, ions, and/or molecules. ... With an increase in temperature there is an increase in the number of collisions. Increasing the concentration of a reactant increases the frequency of collisions between reactants and will, therefore, increase the reaction rate
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In a redox reaction, reduction is defined by the:
jonny [76]

Answer:

C. Gain in electron(s) resulting in a decrease of oxidation number.

Explanation:

Redox reactions are reactions involving transfer of of electron between two species (reduction specie) and (oxidation species) and change resulting in change in oxidation number.

Reduction in terms of redox reaction is the specie that accepts electron(s) and gets "reduced" since its oxidation state has been reduced.

For example

Cl + e- → Cl⁻

The above reaction is an example of reduction reaction taking place in a redox reaction. We can see that Chlorine oxidation state was changed from (0) to (-1) state.

5 0
3 years ago
A mixture of C3H8 and C2H2 has a mass of 2.8 g. It is burned in excess O2 to form a mixture of water and carbon dioxide that con
astraxan [27]

Answer:

The mass of C2H2 in the mixture is 0.56gram using the ratio of carbon in the products contributed by the C2H2.

Explanation:

The balanced equation for the reaction is: C3H8 + 2C2H2 + 10O2 >> 7CO2 + 6H2O.

From the reaction, we know that the oxygen was in excess, this will make the Carbon sources the limiting agents in the reaction. The details of the reaction showed that the ratio of water to the carbon dioxide is 1.6:1. This also means that the expected mole of carbon dioxide will be 7/1.6, which is 3.75moles.

The individual balanced equation of reaction is:

C3H3 +5O2 >> 3CO2 + 4H2O

and 2C2H2 + 5O2 >>4CO2 + 2H2O. From this one can quickly tell that the propane is in sufficient supply as it produces 3 moles of CO2 out of the expected 3.75 moles obtained above. Leaving 0.75moles of CO2 to the ethyne.

The mass of ethyne in the mixture will therefore be: 0.75/3.75 X 2.8 = 0.56g.

4 0
3 years ago
Nitric monoxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO₂), a dark brown gas. If 5.895 mol of NO is mixed with 2
Schach [20]

Answer:

Limiting reactant: O2

grams NO2 produced = 230.276 g NO2

grams of NO unused = 26.67 gNO

Explanation:

2NO + O2 --> 2NO2

Step 1: Determine the molar ratio NO:O2

molar ratio NO:O2 = 5.895: 2.503 = 2.35

stoichiometric molar ratio NO:O2 = 2:1

So, O2 is the limiting reactant.

Step2: Determine the grams of NO2:

?g NO2 = moles O2 x (2moles NO2/1 mol O2) x (MM NO2/ 1 mol NO2) = 2.503 x 2 x 46 = 230.276 g NO2

Step 3: Determine the amount of excess reagent unreacted

moles excess NO reacted = moles O2 x (2 moles NO/1 mol O2) = 2.503 x 2 = 5.006 moles NO reacted

moles NO unreacted = total moles NO - moles NO reacted = 5.895-5.006 =0.889 moles NO unreacted

mass NO unreacted = moles NO unreacted x MM NO = 0.889 x 30 =26.67 g NO unreacted

8 0
3 years ago
A block of lead displaces 50.5ml of water. The block weighs 698 g. From this
Natasha2012 [34]

Answer:

<h2>13.82 g/mL</h2>

Explanation:

The density of a substance can be found by using the formula

density =  \frac{mass}{volume}  \\

From the question we have

density =  \frac{698}{50.5}  \\  = 13.8217...

We have the final answer as

<h3>13.82 g/mL</h3>

Hope this helps you

4 0
3 years ago
6. A solution of CuSO4 is electrolyzed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the
vladimir2022 [97]

The mass of Copper deposited at the cathode : 0.296 g

<h3>Further explanation</h3>

Given

time = t = 10 min=600 s

current = i = 1.5 A

F = 96500 C

charge Cu=+2

Required

The mass of Copper

Solution

Faraday's Law

\tt W=\dfrac{e.i.t}{96500}

e = Ar/valence(valence Cu=2, Ar=63.5 g/mol)

Input the value :

\tt W=\dfrac{63.5/2\times 1.5\times 600}{96500}\\\\W=0.296~g

5 0
3 years ago
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