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julia-pushkina [17]
3 years ago
8

Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes compare. List from lowest freez

ing point to highest freezing point.
BeBr2, AlBr3, Mg3(PO4)2, KBr
Chemistry
1 answer:
Elden [556K]3 years ago
8 0

Answer:

The solutions are listed from the lowest freezing point to highest freezing point.

Mg₃(PO₄)₂ -  AlBr₃ - BeBr₂ -  KBr

Explanation:

Colligative property of freezing point, is the freezing point depression.

Formula is:

ΔT = Kf . m . i

Where ΔT = T° freezing pure solvent - T° freezing solution

Kf is the cryoscopic constant

m is molality and i is the Van't Hoff factor (number of ions, dissolved in solution)

In this case, T° freezing pure solvent is 0° because it's water, so the Kf is 1.86 °C/m, and m is 0.1 molal.

The i modifies the T° freezing solution. The four salts, are ionic compounds, so for each case:

BeBr₂  → Be²⁺  +  2Br⁻   i = 3

AlBr₃ →  Al³⁺  + 3Br⁻   i = 4

Mg₃(PO₄)₂  →  3Mg²⁺  +  2PO₄⁻³    i = 5

KBr →  K⁺  +  Br⁻   i = 2

Solution of Mg₃(PO₄)₂ will have the lowest temperature of freezing and the solution of KBr, the highest (always lower, than 0°).

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Acetylene (c2h2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. given δh°f[co2(g)] = –393.5
Brums [2.3K]
Answer is: 13181,7 kJ of energy <span>is released when 10.5 moles of acetylene is burned.
</span>Balanced chemical reaction: C₂H₂ + 5/2O₂ → 2CO₂ + H₂O.
<span>ΔHrxn = sum of ΔHf (products of reaction) - sum of ΔHf (reactants).</span><span>
Or ΔHrxn = ∑ΔHf (products of reaction) - ∑ΔHf (reactants).
ΔHrxn - enthalpy change of chemical reaction.
<span>ΔHf - enthalpy of formation of reactants or products.
</span></span>ΔHrxn = (2·(-393,5) + (-241,8)) - 226,6 · kJ/mol.
ΔHrxn = -1255,4 kJ/mol.
Make proportion: 1 mol (C₂H₂) : -1255,4 kJ = 10,5 mol(C₂H₂) : Q.
Q = 13181,7 kJ.
8 0
3 years ago
Use enthalpies of formation to determine the ΔHreaction for the reaction
Daniel [21]

Answer:

The enthalpy is increased by the increased heat of the reaction.

Explanation:

In this reaction, as the transition from solid to liquid state, enthalpy increases, that is, the heat applied to change its state is greater and this increases, reaching a mayor disorder.

If the reaction increases its heat, and a liquid state passes, the enthalpy increases, therefore the disorder also and the entropy will also be increased.

5 0
3 years ago
2. A chemical analysis of a sample provides the following elemental data:
Vadim26 [7]

Answer:

C3 H6 O2

Explanation:

first divide their mass by their respective molar mass, we get:

30.4 moles of C

61.2 moles of H

20.25 moles of O

now divide everyone by the smallest one of them then we get

C= 1.5

H= 3

O= 1

since our answer of C is not near to any whole number so we will multiply all of them by 2

so,

C3 H6 O2 is our answer

3 0
1 year ago
Bananas Foster is an example of a dessert that is flambéed. A Bananas Foster label states the accepted number of Calories to be
WINSTONCH [101]

Answer:

6.00%

Explanation:

Step 1: Given data

Accepted value for the number of calories in a Bananas Foster: 300 calories

Measured value for the number of calories in a Bananas Foster: 318 calories

Step 2: Calculate the percent error in the measure

We will use the following expression.

%error = |accepted value - experimental value|/ accepted value × 100%

%error = |300 cal - 318 cal|/ 300 cal × 100% = 6.00%

4 0
3 years ago
What is the molar mass of (NH), CO?<br> 138g<br> 788<br> 968<br> 1448
aleksandr82 [10.1K]

Answer:

The molar mass of (NH_{4})_{2}CO_{3} is 96.8 g/mol

Explanation:

The given molecular formula - (NH_{4})_{2}CO_{3}

Individual molar masses of each element in the compound is as follows.

Molar mass of nitrogen - 14.01 g/mol

Molar mass of of hydrogen = 1.008g/mol

Molar mass of carbon = 12.01 g/mol

Molar mass of oxygen =16.00 g/mol

Molar mass of (NH_{4})_{2}CO_{3} is

2\times[1(14.01)+4(1.008)]+1(12.01)+3(16.00)= 96.8g/mol

Therefore,The molar mass of (NH_{4})_{2}CO_{3} is 96.8 g/mol

7 0
3 years ago
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