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3 years ago

Nuclear reactions in a reactor produce a lot of thermal

Chemistry

2 answers:

Anna11 [10]3 years ago

6 0

Answer:

Explanation:

Leokris [45]3 years ago

4 0

Answer:

Heat flows from the reactor to the water

Explanation:

The thermal energy mentioned in the description is another way to say heat. The energy that is produced by the nuclear reactions leaves the reactor and enters the water, warming it.

The passage does not say that heat flows in the form of electricity, but rather that the turbines turned by the steam produce electricity.

The passage does not say that the steam produces the heat, but rather that the boiling of the water (caused by the heat) produces steam.

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What is the concentration (M) of CH3OH in a solution prepared by dissolving 12.5 g of CH3OH in sufficient water to give exactly

timurjin [86]

Answer:

1.7 M

Explanation:

Concentration is the number of moles of solute dissolved in 1 L of solution

Concentration = number of moles of solute / volume of solution

Number of moles of solute needs to be calculated first

Mass of methanol - 12.5 g

Molar mass of methanol - 32 g/mol

Number of methanol moles - 12.5 g / 32 g/mol = 0.39 mol

Therefore concentration is = 0.39 mol / 0.230 L = 1.7 mol/L

Concentration is 1.7 M

6 0

3 years ago

When a chemist collects hydrogen gas over water, she ends up with a mixture of hydrogen and water vapor in her collecting bottle

elixir [45]

Answer: The partial pressure of hydrogen is 93.9 kPa.

Explanation:

To calculate the partial pressure of hydrogen, we will follow Dalton's Law.

This law states that the total pressure of a mixture of gases is equal to the sum of the individual pressures exerted by the constituent gases.

Mathematically,

$p_{total}=p_A+p_B$

According to the question,

$p_{total}=p_{H_2O}+p_{H_2}$

We are given:

$p_{total}=97.1 kPa$

$p_{H_2O}=3.2kPa$

$p_{H_2}= ?kPa$

Putting values in above equation, we get:

$97.1kPa=3.2kPa+p_{H_2}$

$p_{H_2}= 93.9kPa$

Hence, the partial pressure of hydrogen is 93.9 kPa.

5 0

2 years ago

Read 2 more answers

Using the mmoles of (35)-2,2,-dibromo-3,4-dimethylpentane calculated earlier and the molecular weight of the product (962 g/mol)

Sedbober [7]

Answer:

The yield of the product in gram is $\mathsf{{w_P}=0.26 \ gram}$

Explanation:

Given that:

the molecular mass weight of the product = 96.2 g/mol

the molecular mass of the reagent (3S)-2,2,-dibromo-3,4-dimethylpentane is 257.997 g

given that the millimoles of the reagent = 2,7 millimoles = $2.7 \times 10^{-3} \ moles$

We know that:

Number of moles = mass/molar mass

Then:

$2.7 \times 10^{-3} = \dfrac{ mass}{257.997}$

$mass = 2.7 \times 10^{-3} \times 257.997$

mass = 0.697

Theoretical yield = (number of moles of the product/ number of moles of reactant) × 100

i.e

Theoretical yield = $\dfrac{n_P}{n_R}\times 100\%$

where;

$n_P = \dfrac{w_P}{m_P}$ and $n_R = \dfrac{w_R}{m_R}$

Theoretical yield = $\dfrac{(\dfrac{w_P}{m_P})}{(\dfrac{w_R}{m_R})} \times 100\%$

Given that the theoretical yield = 100%

Then:

$100\% =\dfrac{(\dfrac{w_P}{m_P})}{(\dfrac{w_R}{m_R})} \times 100\%$

$\dfrac{w_P}{m_P}=\dfrac{w_R}{m_R}$

${w_P}=\dfrac{w_R \times m_P}{m_R}$

where,

$w_P$ = derived weight of the product

$m_P =$ the molecular mass of the derived product

$m_R =$ the molecular mass of the reagent

$w_R$ = weight in a gram of the reagent

${w_P}=\dfrac{w_R \times m_P}{m_R}$

${w_P}=\dfrac{0.697 \times 96.2}{257.997}$

$\mathsf{{w_P}=0.26 \ gram}$

8 0

3 years ago

Help, 8th grade Science

valentinak56 [21]

Answer:

Control container

Explanation:

5 0

3 years ago

Read 2 more answers

How do you figure out the final temperature or the initial temperature in calorimetry.

Zolol [24]

Add the change in temperature to your substance's original temperature to find its final heat. For example, if your water was initially at 24 degrees Celsius, its final temperature would be: 24 + 6, or 30 degrees Celsius.

4 0

2 years ago