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zalisa [80]
2 years ago
11

How much energy is required to convert 100.0 g of water completely to steam?

Chemistry
1 answer:
Brrunno [24]2 years ago
3 0

Answer:

<u>225.6 kJ</u>, <em>assuming the water is already at 100 °C</em>

Explanation:

The correct answer to this question will depend on the initial temperature of the water to which heat is added to produce steam.  Energy is required to raise the water temperature to 100°C.  At that point, an energy of vaporization is needed to convert liquid water at 100 °C to water vapor at 100°C.  The heat of vaporization for water is 2256.4 kJ/kg.  The energy required to bring 100g of water from a lower temperature to 100°C is calculated at 4.186 J/g°C.  We don't know the starting temperature, so this step cannot be calculated.

<em><u>Assuming</u></em> that we are already at 100 °C, we can calculate the heat required for vaporization:

(100.0g)(1000.0g/1 kg)(2256.4 kJ/kg) = 225.6 kJ for 100 grams water.

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If 125g of KClO3 is heated, what is the total mass of the products?​
Andrej [43]

Given parameters:

Mass of KClO₃  = 125g

Unknown:

Total mass of the products = ?

When  KClO₃ is heated, it thermally decomposes to KCl and O₂ according to the chemical equation below;

               2KClO₃  →  2KCl + 3O₂

All chemical equations obeys the law of conservation of matter and with this regard, we know that the amount of reactants used is the same as that of the product.

The total mass of the products must give us 125g according to this law of conservation of matter.

Now to find the masses of each product,

  1. Find the number of moles of the given reactant:

     Number of moles  = \frac{mass}{molar mass}

  molar mass of  KClO₃  = 39 + 35.5 + 3(16)  = 122.5g/mol

    So number of moles of KClO₃ = \frac{125}{122.5}  = 1.02moles

    2. Now, using this number of moles, find the number of moles of the products using this value;

   2 moles of KClO₃ produced 2 moles of KCl

  1.02 moles of KClO₃ will also produce 1.02moles of KCl

   2 moles of KClO₃ produced 3 moles of O₂

   1.02 moles of KClO₃ will produce   \frac{1.02 x 3} {2} mole = 1.53 moles of O₂

   3. Now find the masses of each product;

Mass  = number of moles x molar mass

  molar mass of KCl  = 39 + 35.5 = 74.5g/mol

  molar mass of O₂  = 16 x 2  = 32g/mol

  Mass of KCl  = 74.5 x 1.02  = 75.99g

  Mass of O₂  = 32 x 1.53 = 48.96g

Total mass of products = mass of KCl + Mass of O₂ = 75.99g + 48.96g

                                        = 124.95g

This value is approximately the same as that of mass of  KClO₃

 

7 0
3 years ago
What is that the theoretical yield of aluminum oxide I if 3.20 mol of aluminum metal is exposed to 2.70 mole of oxygen
photoshop1234 [79]

Answer:

163.2g

Explanation:

First let us generate a balanced equation for the reaction. This is shown below:

4Al + 3O2 —> 2Al2O3

From the question given, were were told that 3.2moles of aluminium was exposed to 2.7moles of oxygen. Judging by this, oxygen is excess.

From the equation,

4moles of Al produced 2moles of Al2O3.

Therefore, 3.2moles of Al will produce = (3.2x2)/4 = 1.6mol of Al2O3.

Now, let us covert 1.6mol of Al2O3 to obtain the theoretical yield. This is illustrated below:

Mole of Al2O3 = 1.6mole

Molar Mass of Al2O3 = (27x2) + (16x3) = 54 + 48 =102g/mol

Mass of Al2O3 =?

Number of mole = Mass /Molar Mass

Mass = number of mole x molar Mass

Mass of Al2O3 = 1.6 x 102 = 163.2g

Therefore the theoretical of Al2O3 is 163.2g

8 0
3 years ago
Equal but opposite forces acting on an object results in what?
forsale [732]

Answer:

Action given and reaction taken

Also known as

Newton's third law of motion

Explanation:

An action will be done such as bouncing a ball on the wall

- You throw the ball (Action)

- The ball bounces back (Reaction)

Hope this Helps

3 0
2 years ago
How much would a 50-kg object weigh on Mercury (gravity on Mercury is 3.59 m/s2)?
Andreyy89
Gravitational<span> Acceleration or W=Mg so... Q1: W(earth)=</span>50, W(X)=500 ---> g(X)=10<span>*g(earth)=10*9.8=98 --> C is correct. Q2: </span>M<span>=W/g --> </span>M=735/9.8=75 ---> B is correct. Q3: W=Mg=50*3.59<span>=179.5 N ---> B is correct</span>
4 0
3 years ago
Four preparations involving table sugar (sucrose) are described below. Analyze the sugar preparation processes and the end produ
MAXImum [283]

Answer:

the answer is c

Explanation:

because i got it right

4 0
3 years ago
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