The moon makes light the same way that the sun does.True or False

It takes 208.4 kJ of energy to remove 1 mole of electrons from the atoms on the surface of rubidium metal. If rubidium metal is

Elanso [62]

Answer:

4.34x10⁻¹⁹ J

Explanation:

The total energy emitted by irradiation is given by

E = hf, where E is the energy, <em>h</em> is the plack constant (6.626x10⁻³⁴ J.s), and <em>f</em> is the frequency. The frequency is also the velocity of the light (c = 2.99x10⁸ m/s) divided by the length of the irradiation (254x10⁻⁹ m). So:

E = (6.626x10⁻³⁴)x(2.99x10⁸)/ (254x10⁻⁹)

E = 7.80x10⁻¹⁹ J

The energy to remove 1 electron is the energy necessary to remove 1 mol divided by the Avogadros number ( 1 mol = 6.02x10²³ electrons):

208400/6.022x10^23 = 3.46x10⁻¹⁹ J

The total energy is the energy necessary to remove one electrons plus the kinectic energy (Ek) of the electrons:

7.80x10⁻¹⁹ = 3.46x10⁻¹⁹ + Ek

Ek = 7.80x10⁻¹⁹ - 3.46x10⁻¹⁹

Ek = 4.34x10⁻¹⁹ J

7 0

3 years ago

How many particles are in 2.50 moles of iron (II) chloride?

liq [111]

Answer:

<h2>1.505 × 10²⁴ particles</h2>

Explanation:

The number of particles in iron (II) chloride can be found by using the formula

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

N = 2.5 × 6.02 × 10²³

We have the final answer as

<h3>1.505 × 10²⁴ particles</h3>

Hope this helps you

8 0

3 years ago

You deposit $2000 in a bank account that pays 3% annual interest. Find the balance after 8 years if the interest is compounded q

Phantasy [73]

Answer:

2480‬$

Explanation:

2000$*(3%=0.03)=60$

multiply by 8 = 480$

then by adding it to 2000 = 2480$

5 0

4 years ago

How many grams of aluminum are required to produce 8.70 moles of aluminum chloride

Serggg [28]

Answer:

1160.058g

Explanation:

8.70*133.34=1160.058g

4 0

3 years ago

Consider a simple reaction in which a reactant AA forms products: A→productsA→products What is the rate law if the reaction is z

levacccp [35]

Answer :

The rate law expression for zero order reaction will be:

$Rate=k[A]^0$

The rate law expression for first order reaction will be:

$Rate=k[A]^1$

The rate law expression for second order reaction will be:

$Rate=k[A]^2$

Zero order reaction : There is no affect on the rate law.

First order reaction : The rate law becomes doubled.

Second order reaction : The rate law becomes quadrupled.

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The given reaction is:

$A\rightarrow Products$

The rate law expression for zero order reaction will be:

$Rate=k[A]^0$

The rate law expression for first order reaction will be:

$Rate=k[A]^1$

The rate law expression for second order reaction will be:

$Rate=k[A]^2$

Now we have to determine that if doubling of the concentration of A then the rate of reaction will be:

As we know that the zero order reaction does not depend on the concentration of reactant. So, there is no affect on the rate law.

As we know that the first order reaction depend on the concentration of reactant. So, the rate law becomes doubled.

As we know that the second order reaction depend on the concentration of reactant. So, the rate law becomes quadrupled.

5 0

4 years ago