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tangare [24]
1 year ago
12

How fast is an electron travelling If it has a wavelength of 8.20 km?

Chemistry
1 answer:
Lemur [1.5K]1 year ago
5 0

The electron is travelling with a velocity of 1.123 × 10⁷m/s if it has a wavelength of 8.20 km.

<h3>How to calculate velocity of an electron?</h3>

The velocity at which an electron travels can be calculated using the following formula:

λ = h/mv

Where;

  • H = Planck's constant
  • m = mass of electron
  • v = velocity of electron
  • λ = wavelength

  • Planck's constant (h) = 6.626 × 10−³⁴ J⋅s.
  • mass of electron (m) = 9.109 × 10−³¹ kg
  • wavelength = 8200m

8200 = 6.626×10−³⁴ / 9.109 × 10−³¹V

8200 = 7.3 × 10-⁴V

V = 8200 ÷ 7.3 × 10-⁴

V = 1.123 × 10⁷m/s

Therefore, the electron is travelling with a velocity of 1.123 × 10⁷m/s if it has a wavelength of 8.20 km.

Learn more about velocity at: brainly.com/question/13171879

#SPJ1

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Explanation:

The reaction is given as;

Br2(g) + Cl2(g) ----> 2BrCl(g)

From the equation;

1 mol of Br2 reacts with 1 mol of Cl2

Converting the masses given to moles, using the formular;

Number of moles = Mass / Molar mass

Br2;

Number of moles = 33.7 g / 159.808 g/mol = 0.21088 mol

Cl2;

Number of moles = 13.0 g / 70.906 g/mol = 0.18334 mol

From the values;

0.18334 mol of Cl2 would react with 0.18334 mol of Br2 with an excess of 0.02754 mol of Br2

<em>What is the maximum amount of bromine monochloride that can be formed? __________grams</em>

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1 mol of Cl2 produces 2 mol of Bromine Monochloride

0.18334 mol of Cl2 would produce x

Solving for x;

x = 0.18334 * 2 = 0.36668 mol

Converting to mass;

Mass = Number of moles * Molar mass = 0.36668 mol * 115.357 g/mol

Mass = 42.299 g

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<em>What is the FORMULA for the limiting reagent?</em>

<em />

The limiting reagent is Cl2 as it determines the amount of product formed. The moment the reaction uses up Cl2, the reaction stops.

<em>What amount of the excess reagent remains after the reaction is complete? __________grams</em>

The excess reagent is Br2

The number of moles left is;

0.02754 mol of Br2

Converting to mass;

Mass = Number of moles * Molar mass = 0.02754 mol  * 159.808 g/mol

Mass = 4.401 g

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Answer:

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Determine the heat of reaction for the process TiO2(s) + 4HCl(g) TiCl4(l) + 2H2(g) + O2(g) using the information given below: Ti
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Answer : The heat of reaction for the process is, 1374.7 kJ

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The main chemical reaction is,

TiO_2(s)+4HCl(g)\rightarrow TiCl_4(l)+2H_2(g)+O_2(g)    \Delta H_{rxn}=?

The intermediate balanced chemical reaction will be,

(1) Ti(s)+O_2(g)\rightarrow TiO_2(s)     \Delta H_1=-939.7kJ

(2) 2HCl(g)\rightarrow H_2(g)+Cl_2(g)    \Delta H_2=-184.6kJ

(3) Ti(s)+2Cl_2(g)\rightarrow TiCl_4(l)    \Delta H_3=-804.2kJ

We reversing reaction 1, 3 and multiplying reaction 2 by 2 and then adding all the equations, we get :

(1) TiO_2(s)\rightarrow Ti(s)+O_2(g)     \Delta H_1=939.7kJ

(2) 4HCl(g)\rightarrow 2H_2(g)+2Cl_2(g)    \Delta H_2=2\times (-184.6kJ)=-369.2kJ

(3) TiCl_4(l)\rightarrow Ti(s)+2Cl_2(g)    \Delta H_3=804.2kJ

The expression for heat of reaction for the process is:

\Delta H_{rxn}=\Delta H_1+\Delta H_2+\Delta H_3

\Delta H_{rxn}=(939.7kJ)+(-369.2kJ)+(804.2kJ)

\Delta H_{rxn}=1374.7kJ

Therefore, the heat of reaction for the process is, 1374.7 kJ

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