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Dmitrij [34]
3 years ago
8

Can someone tell me how to solve this step by step? I got the answer but I want to know how to solve it I have a test !!!!

Chemistry
1 answer:
UNO [17]3 years ago
6 0
C becuase that is the one that you would have to do becuase that is the only option
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PLZ HELP For the reaction: 2NO2(g) → N2O4(l),
Furkat [3]

Answer: \Delta H_{rxn}=-20kJ/mol-(+66kJ/mol)

Explanation:

Heat of reaction or enthalpy change is the energy released or absorbed during the course of the reaction.

It is calculated by subtracting the enthalpy of reactants from the enthalpy of products.

\Delta H=H_{products}-H_{reactants}

\Delta H = enthalpy change = ?

H_{products} = enthalpy of products

H_{reactants} = enthalpy of reactants

For the given reaction :

2NO_2(g)\rightarrow N_2O_4(l)

\Delta H=H_{N_2O_4}-2\times H_{NO_2}

\Delta H=-20kJ/mol-(+66kJ/mol)

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Which event most likely occurs at point V?<br><br> cooling<br> erosion<br> heating<br> melting
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Answer: cooling

Explanation:

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A scientist discovers that an atom with a mass number of 14 contains eight electrons.
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3 years ago
Pick 1 answer, please help!
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If a 58 g sample of metal at 100 c is placed into calorimeter containing 60g of water at 18 c , the temperature of the water inc
tatiyna

Answer:

The water will absorb 1004.16 Joule of heat

Explanation:

Step 1: Data given

Mass of the metal = 58.00 grams

Temperature of the metal = 100.00 °C

Mass of water = 60.00 grams

Temperature of water = 18.00 °C

Final temperature = 22.00 °C

Specific heat of water = 4.184 J/g°C

Step 2: Calculate the amount of heat absorbed by the water in joules

Q = mass *specific heat *ΔT

 ⇒ with Q = the heat absorbed by water

⇒ with mass of water = 60.00 grams

⇒ with specific heat of water = 4.184 J/g°C

⇒ with ΔT = The change in temperature of water = T2 - T1 = 22 - 18 = 4.0 °C

Q = 60.00 * 4.184 J/g°C * 4.0 °C

Q = 1004.16 J

The water will absorb 1004.16 Joule of heat

6 0
3 years ago
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