All categories

3 years ago

Plz help me with this question

Chemistry

1 answer:

miskamm [114]3 years ago

5 0

Answer:

<h2>Here is your answer. I hope it will help you . </h2>

You might be interested in

Please help me solve this question

brilliants [131]

The radioactive decay follows first order kinetics

The integrated rate law expression for first order rate is

ln(A / At) = kt

Where A= initial concentration

At=concentration at time "t"

t = time

K= rate constant

ln(50 / 0.0488) = k X 38

Therefore

K = 0.1824 day-1

The relation between rate constant and half life is

So half life = 0.693 / 0.1824 = 3.8 days

So isotope must be Radon-222

7 0

3 years ago

Please tell me the answer I will mark you brainliest

Shkiper50 [21]

Answer:

Explanation:

third answer might be right

8 0

3 years ago

Read 2 more answers

What variables are considered when forecasting weather

saveliy_v [14]

There are lots of variables.
1. relative humidity
2. dew point temperature
3. air temperature
4. wind speeds
5. vapor pressure
6. latitude and longitude
7. orrographic lift (surface type)

there are probably more, but hope this helped! :)

4 0

3 years ago

Consider the dissolution of calcium hydroxide:

Crazy boy [7]

Answer:

1. $K_eq = [Ca^{2+][OH^-]^2 = K_{sp}$

2. a. No effect;

b. Products;

c. Products;

d. Reactants

Explanation:

1. Equilibrium constant might be written using standard guidelines:

only aqueous species and gases are included in the equilibrium constant excluding solids and liquids;
the constant involves two parts: in the numerator of a fraction we include the product of the concentrations of products;
the denominator includes the product of the concentrations of reactants;
the concentrations are raised to the power of the coefficients in the balanced chemical equation.

Based on the guidelines, we have two ions on the product side, a solid on the left side. Thus, the equilibrium constant has the following expression:

$K_eq = [Ca^{2+][OH^-]^2 = K_{sp}$

2. a. In the following problems, we'll be considering the common ion effect. According to the principle of Le Chatelier, an increase in concentration of any of the ions would shift the equilibrium towards the formation of our precipitate.

In this problem, we're adding calcium carbonate. It is insoluble, so it wouldn't have any effect on the equilibrium.

b. Sodium carbonate is completely soluble, it would release carbonate ions. The carbonate ions would combine with calcium cations and more precipitate would dissolve. This would shift the equilibrium towards formation of the products to reproduce the amount of calcium cations.

c. HCl would neutralize calcium hydroxide to produce calcium chloride and water, so the amount of calcium ions would increase, therefore, the products are favored.

d. NaOH contains hydroxide anions, so we'd have a common ion. An increase in hydroxide would produce more precipitate, so our reactants are favored.

3 0

3 years ago

State the observation made when hydrogen chloride gas is passed over ammonia gas

Zarrin [17]

Answer:

dry

Explanation:

it will dry the hydrogen chloride to the ammonia

6 0

3 years ago