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spayn [35]
2 years ago
15

What should each experiment only have one of?

Chemistry
1 answer:
Ket [755]2 years ago
3 0

Answer: varriable

Explanation:meaning one element, feature or factor able to change

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What is the molarity of a 2.0 L sodium hydroxide solution containing 10.0 grams of solute?
SSSSS [86.1K]
Molar mass NaOH ( sodium hydroxide) = 40.0 g/mol

Number of moles:

n = mass / molar mass

n = 10.0 / 40.0

n = 0.25 moles

Volume = 2.0 L

Molarity = number of moles / volume in liters

M  = 0.25 / 2.0

M = 0.125  M

answer D

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If the statement is true, select True. If it is false, select False.
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Industrial ethanol (CH3CH2OH) is produced by a catalytic reaction of ethylene (CH2═CH2) with water at high pressures and tempera
Natasha2012 [34]

Answer:

using bond energies = - 37 kJ

using enthalpies of formation = - 45.7 kJ

Explanation:

From the reaction;

CH2═CH2(g) + H2O(g) -------> CH3CH2OH(g)

From the above reaction; there are 4 (C-H) bonds , 1 ( C=C) and 2 (H-O) of ethene which forms 5(C-H) bonds, 1 (C-C) and 1 (C-O) and 1(H-O) bonds.

Using Bond Energies; the heat of the reaction can be written as:

\delta H^0_ {rxn}= ∑ energy of old bond breaking + ∑ energies of the new bond formation.

\delta H^0_ {rxn}= ∑ [(4 * BE_{C-H})  + BE_{C-C}) +  + BE_{O-H})]+ ∑ [(5 * BE_{C-H}) + BE_{C-C}) + BE_{O-H}+ BE_{C-O})]

\delta H^0_ {rxn}= ∑[4*413 kJ)+(614kJ)+(2*647kJ]+ ∑ (5*-413kJ)+(-347kJ)+(-467kJ)+(-358kJ)]

\delta H^0_ {rxn}=  -37 kJ

To calculate the heats of reaction by using enthalpies of formation; we have:

\delta H^0_ {rxn}= ∑ \delta H^0_ {products} -  ∑ \delta H^0_ {reactants}

\delta H^0_ {rxn}= ∑ \delta H^0_ {CH_3CH_2OH} - ∑ \delta H^0_ {CH_2=CH_2+H_2O}

\delta H^0_ {rxn}=  (-235.1 kJ) - [(+52.47 kJ) + (-241.826 kJ)]

\delta H^0_ {rxn}=  -45.7 kJ

6 0
3 years ago
PLEASE HELP QUICKLY
Nikolay [14]
If is an endothermic reaction.. heat is absorbed from the surrounding.. so it is Positive(+ve).. l hope it helped???
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