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Finger [1]
2 years ago
14

Helpppp pleaseeeeeee

Chemistry
1 answer:
algol132 years ago
4 0

Answer: c

Explanation:

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The objects mass I took physical science
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Which of the following shows a coefficient?
rosijanka [135]

Answer:

my answer is b oti d I am not sure

6 0
2 years ago
How many mL of 2M stock solution would I use to prepare 0.500 L of 0.1 M NaCl?
nordsb [41]

Answer:

25 mL

Explanation:

Step 1: Given data

  • Concentration of the concentrated solution (C₁): 2 M
  • Volume of the concentrated solution (V₁): ?
  • Concentration of the diluted solution (C₂): 0.1 M
  • Volume of the diluted solution (V₂): 0.500 L

Step 2: Calculate the volume of the concentrated NaCl solution

We will use the dilution rule.

C₁ × V₁ = C₂ × V₂

V₁ = C₂ × V₂ / C₁

V₁ = 0.1 M × 0.500 L / 2 M

V₁ = 0.025 L = 25 mL

4 0
3 years ago
A sample of 10.6 g of KNO3 was dissolved in 251.0 g of water at 25 oC in a calorimeter. The final temperature of the solution wa
finlep [7]

Answer:

36.55kJ/mol

Explanation:

The heat of solution is the change in heat when the KNO3 dissolves in water:

KNO3(aq) → K+(aq) + NO3-(aq)

As the temperature decreases, the reaction is endothermic and the molar heat of solution is positive.

To solve the molar heat we need to find the moles of KNO3 dissolved and the change in heat as follows:

<em>Moles KNO3 -Molar mass: 101.1032g/mol-</em>

10.6g * (1mol/101.1032g) = 0.1048 moles KNO3

<em>Change in heat:</em>

q = m*S*ΔT

<em>Where q is heat in J,</em>

<em>m is the mass of the solution: 10.6g + 251.0g = 261.6g</em>

S is specififc heat of solution: 4.184J/g°C -Assuming is the same than pure water-

And ΔT is change in temperature: 25°C - 21.5°C = 3.5°C

q = 261.6g*4.184J/g°C*3.5°C

q = 3830.87J

<em>Molar heat of solution:</em>

3830.87J/0.1048 moles KNO3 =

36554J/mol =

<h3>36.55kJ/mol</h3>

<em />

6 0
2 years ago
HELP!!!! The freezing of methane is an exothermic change. What best describes the temperature conditions that are likely to make
vazorg [7]

<u>Answer:</u> The correct statement is low temperature only, because entropy decreases during freezing.

<u>Explanation:</u>

The relationship between Gibb's free energy, enthalpy, entropy and temperature is given by the equation:

\Delta G=\Delta H-T\Delta S

Where,

\Delta G = change in Gibb's free energy

\Delta H = change in enthalpy

T = temperature

\Delta S = change in entropy

It is given that freezing of methane is taking place, which means that entropy is decreasing and Delta S is becoming negative. It is also given that the reaction is an exothermic reaction, this means that the \Delta H is also negative.

For a reaction to be spontaneous, \Delta G must be negative.

-ve=-ve-[T(-ve)]\\\\-ve=-ve+T

From above equations, it is visible that \Delta G will be negative only when the temperature will be low.

Hence, the correct statement is low temperature only, because entropy decreases during freezing.

8 0
3 years ago
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