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Levart [38]
2 years ago
6

A 35.0 g piece of metal wire is heated, and the temperature changes from 21 degrees Celsius to 52 degrees Celsius. The amount of

heat absorbed is 320 calories. What is the specific heat of the metal?
Chemistry
1 answer:
Elina [12.6K]2 years ago
5 0

Answer:

1.23 j/g. °C

Explanation:

Given data:

Mass of metal = 35.0 g

Initial temperature = 21 °C

Final temperature = 52°C

Amount of heat absorbed = 320 cal  (320 ×4.184 = 1338.88 j)

Specific heat capacity of metal = ?

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = 52°C -  21 °C

ΔT = 31°C

1338.88 j= 35 g ×c× 31°C

1338.88 j= 1085 g.°C ×c

1338.88 j/1085 g.°C = c

1.23 j/g. °C = c

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What is the theoretical yield of aluminum oxide if 1.40 mol of aluminum metal is exposed to 1.35 mol of oxygen?
jasenka [17]

Answer:

71.372 g or 0.7 moles

Explanation:

We are given;

  • Moles of Aluminium is 1.40 mol
  • Moles of Oxygen 1.35 mol

We are required to determine the theoretical yield of Aluminium oxide

The equation for the reaction between Aluminium and Oxygen is given by;

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

From the equation 4 moles Al reacts with 3 moles of oxygen to yield 2 moles of Aluminium oxide.

Therefore;

1.4 moles of Al will require 1.05 moles (1.4 × 3/4) of oxygen

1.35 moles of Oxygen will require 1.8 moles (1.35 × 4/3) of Aluminium

Therefore, Aluminium is the rate limiting reagent in the reaction while Oxygen is the excess reactant.

4 moles of aluminium reacts to generate 2 moles aluminium oxide.

Therefore;

Mole ratio Al : Al₂O₃ is 4 : 2

Thus;

Moles of Al₂O₃ = Moles of Al × 0.5

                         = 1.4 moles × 0.5

                         = 0.7 moles

But; 1 mole of Al₂O₃ = 101.96 g/mol

Thus;

Theoretical mass of Al₂O₃ = 0.7 moles × 101.96 g/mol

                                            = 71.372 g

3 0
3 years ago
One mole of a metallic oxide reacts with one mole of hydrogen to produce two moles of the pure metal
kenny6666 [7]

Answer:

Lithium oxide, Li₂O.  

Explanation:

Hello!  

In this case, according to the given amounts, it is possible to write down the chemical reaction as shown below:

M_2O+H_2\rightarrow 2M+H_2O  

Which means that the metallic oxide has the following formula: M₂O. Next, we can set up the following proportional factors according to the chemical reaction:

5.00gM_2O*\frac{1molM_2O}{(2*X+16)gM_2O}*\frac{2molM}{1molM_2O}*\frac{XgM}{1molM}=2.32gM  

Thus, we perform the operations in order to obtain:

\frac{10X}{(2X+16)}=2.32  

So we solve for x as shown below:

10X=2.32(2X+16)\\\\10X=4.64X+37.12\\\\X=\frac{37.12}{10-4.64}\\\\X= 6.93g/mol  

Whose molar mass corresponds to lithium, and therefore, the metallic oxide is lithium oxide, Li₂O.  

Best regards!

8 0
2 years ago
Need ASAP will give brainlist
Leokris [45]

Answer:

A.

The answer is A :)

7 0
2 years ago
How many moles of hydrogen gas can be produced if 0.78 moles of hydrochloric acid reacts with excess solid zinc according to the
White raven [17]

Answer:

The answer to your question is It will be formed 0.39 moles of H₂

Explanation:

Data

moles of H₂ = ?

moles of HCl = 0.78

moles of Zinc = excess

Balanced chemical reaction

              2 HCl  +  Zn  ⇒  1 H₂  +  ZnCl₂

Process

1.- Use proportions to solve this problem. Consider the coefficients of the balanced reaction.

               2 moles of HCl ---------------------- 1 mol of H₂

               0.78 moles of HCl -----------------  x

               x = (0.78 x 1) / 2

- Simplification

              x = 0.78 / 2

- Result

              x = 0.39 moles of H₂

3 0
3 years ago
The complete orbital notation diagram of an atom is shown.
Yuki888 [10]

Answer:

Explanation:

From the description provided by the statement of the problem, we can easily solve for the values of the angular momentum quantum number.

Let us represent the atom as J:

In atom J, we have five sub-orbitals in which there 9 electrons. From the designation used to represent sublevels, we can write the notation as below:

             J = 10 electrons = 1s² 2s² 2p⁵

The s-sublevel can only contain 2 electrons

p-sublevel can contain 6 electrons but we have just 5 electrons in there.

Now, to find the angular momentum quantum number, we need to understand what this quantum number denotes.

This quantum number is also known as azimuthal or secondary quantum number. It gives the shape of the orbitals in subshells accomodating electrons. This quantum number is designated by (l).

         l (n-1)            name of orbital               shape of orbital

             0                     s                                   spherical

             1                     p                                    dumb-bell

             2                    d                                    double dumb-bell

             3                    f                                      complex

J  = 1s² 2s² 2p⁵

where 1 and 2 coefficients are the principal quantum numbers(n).

            s and p are the shape of the orbitals

For 1s², the l vaue is 0 because the electron is in the s orbital

     2s² the l value is 0, 1 and the electron can be in the s or p orbitals

     2p⁵ the l value is 0, 1 and the electrons can be in the s or p orbitals

The quantum number gives the shape of the orbital.

8 0
3 years ago
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