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Oksi-84 [34.3K]
3 years ago
12

Which experimental setup would let a student investigate the connection between kinetic energy and temperature? (1 point) placin

g one drop of food coloring in a cup with 60 ml of water at 10",placing one drop of od coloring in a second oup with 60 mL of water at 40°C placing one drop of food coloring in a cup with 50 ml of water at 10" placing one drop of food coloring in a second cup with 100 ml of water al 10" placing one drop of food coloring in a cup with some of water al 10 placing two drops of food coloring in a second cup with 100 ml of water an 100 placing one drop of food coloring in a cup with some of water at 100 placing two drops of food coloring in a second cup with 50 ml of water at To ONO type here to search​
Chemistry
1 answer:
Maslowich3 years ago
5 0

Answer:

The correct option is;

Placing one drop of food coloring in a cup with 60 ml of water at 10°, placing one drop of food coloring in a second cup with 60 ml of water at 40°C

Explanation:

The experimental setup that would allow the student investigate the connection between kinetic energy and temperature should be made up of the following characteristics

1) The constant terms for the experiment should be defined, which in this case are

a) The volume of the water which is 60 ml in both subjects of the experiment

2) The definition of the variable that produces the effect that is being monitored, which is the use of the different temperatures in the two experimental subjects

3)The environmental limits of the experiment, which is the water and the food coloring used

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Calculate the standard enthalpy of formation of NOCl(g) at 25 ºC, knowing that the standard enthalpy of formation of NO(g) at th
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Answer:

The standard enthalpy of formation of NOCl(g) at 25 ºC is 105 kJ/mol

Explanation:

The ∆H (heat of reaction) of the combustion reaction is the heat that accompanies the entire reaction. For its calculation you must make the total sum of all the heats of the products and of the reagents affected by their stoichiometric coefficient (number of molecules of each compound that participates in the reaction) and finally subtract them:

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In this case, you have:  2 NOCl(g) → 2 NO(g) + Cl₂(g)

So, ΔH=2*H_{NO} +H_{Cl_{2} }-2*H_{NOCl}

Knowing:

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Replacing:

75.5 kJ/mol=2* 90.25 kJ/mol + 0 - H_{NOCl}

Solving

-H_{NOCl}=75.5 kJ/mol - 2*90.25 kJ/mol

-H_{NOCl}=-105 kJ/mol

H_{NOCl}=105 kJ/mol

<u><em>The standard enthalpy of formation of NOCl(g) at 25 ºC is 105 kJ/mol</em></u>

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