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emmasim [6.3K]
3 years ago
5

Complete and balance the following reaction. Zinc loses two electrons to form an ion. What type of reaction does this equation r

epresent? Explain your reasoning Zn + AgNO3 ________ + ________
Chemistry
2 answers:
guajiro [1.7K]3 years ago
8 0

Answer: Redox reaction/displacement reaction

Explanation:

Zn + 2AgNO3----------> Zn(NO3)2+ 2Ag

Let us consider the change in oxidation number from left to right

Oxidation number of zinc changed from 0 to +2

Oxidation number of silver changed from +1 to 0

Zinc was oxidized while silver was reduced. This shows a redox process

Also Zinc displaced silver because silver is below zinc in the a electrochemical series of metals. That is, the electrode potential of zinc is more negative than that of silver hence it can displace silver from its salt.

ICE Princess25 [194]3 years ago
4 0
2AgNO3  +  Zn  -->  Zn(NO3)2  +  2Ag
Its a redox reaction, Zn is oxidised (0 --> 2+), Ag is reduced (1+ --> 0)
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How much heat energy is required to convert 48.3 g of solid ethanol at -114.5 degree C to gasesous ethanol at 135.3 degree C? Th
OLEGan [10]

Answer:

7.21 × 10⁴ J

Explanation:

Ethanol is solid below -114.5°c, liquid between -114.5°C and 78.4°C, and gaseous above 78.4°C.

<em>How much heat energy is required to convert 48.3 g of solid ethanol at -114.5°C to gaseous ethanol at 135.3 °C?</em>

<em />

We need to calculate the heat required in different stages and then add them.

The moles of ethanol are:

48.3g.\frac{1mol}{46.07g} =1.05mol

Solid-liquid transition

Q₁ = ΔHfus . n = (4.60 kJ/mol) . 1.05 mol = 4.83 kJ = 4.83 × 10³ J

where,

ΔHfus: molar heat of fusion

n: moles

Liquid: from -114.5°C to 78.4°C

Q₂ = c(l) . m . ΔT = (2.45 J/g.°C) . 48.3g . [78.4°C-(-114.5°C)] = 2.28 × 10⁴ J

where,

c(l): specific heat capacity of the liquid

ΔT: change in the temperature

Liquid-gas transition

Q₃ = ΔHvap . n = (38.56 kJ/mol) . 1.05 mol = 40.5 kJ = 40.5 × 10³ J

where,

ΔHvap: molar heat of vaporization

Gas: from 78.4°C to 135.3°C

Q₄ = c(g) . m . ΔT = (1.43 J/g.°C) . 48.3g . (135.3°C-78.4°C) = 3.93 × 10³ J

where

c(g): specific heat capacity of the gas

Total heat required

Q₁ + Q₂ + Q₃ + Q₄ = 4.83 × 10³ J + 2.28 × 10⁴ J + 40.5 × 10³ J + 3.93 × 10³ J = 7.21 × 10⁴ J

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3 years ago
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Learn more about dissociation equation: brainly.com/question/1903354

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