What is the maximum number of electrons that can go into the D orbitals

Fill in the blanks to correctly describe each separation process.

Dimas [21]

Answer:

C, B ,A(in the order of the blanks)

Explanation:

A centrifuge uses centrifugal force to seperate 2 substances with different densities, the lighter one at the top. This cannot be done with homogeneous mixtures

4 0

3 years ago

rate of a certain reaction is given by the following rate law: rate Use this information to answer the questions below. What is

Sunny_sXe [5.5K]

Complete Question

The rate of a certain reaction is given by the following rate law:

$rate = k [H_2][I_2]$

rate Use this information to answer the questions below.

What is the reaction order in $H_2$ ?

What is the reaction order in $I_2$ ?

What is overall reaction order?

At a certain concentration of H2 and I2, the initial rate of reaction is 2.0 x 104 M / s. What would the initial rate of the reaction be if the concentration of H2 were doubled? Round your answer to significant digits. The rate of the reaction is measured to be 52.0 M / s when [H2] = 1.8 M and [I2] = 0.82 M. Calculate the value of the rate constant. Round your answer to significant digits.

Answer:

The reaction order in $H_2$ is n = 1

The reaction order in $I_2$ is m = 1

The overall reaction order z = 2

When the hydrogen is double the the initial rate is $rate_n = 4.0*10^{-4} M/s$

The rate constant is $k = 35.23 \ M^{-1} s^{-1}$

Explanation:

From the question we are told that

The rate law is $rate = k [H_2][I_2]$

The rate of reaction is $rate = 2.0 *10^{4} M /s$

Let the reaction order for $H_2$ be n and for $I_2$ be m

From the given rate law the concentration of $H_2$ is raised to the power of 1 and this is same with $I_2$ so their reaction order is n=m=1

The overall reaction order is

$z = n +m$

$z =1 +1$

$z =2$

At $rate = 2.0 *10^{4} M /s$

$2.0*10^{4} = k [H_2] [I_2] ---(1)$

= > $k = \frac{2.0*10^{4}}{[H_2] [I_2] }$

given that the concentration of hydrogen is doubled we have that

$rate = k [2H_2] [I_2] ----(2)$

=> $k = \frac{rate_n }{ [2H_2] [I_2]}$

So equating the two k

$\frac{2.0*10^{4}}{[H_2] [I_2] } = \frac{rate_n }{ [2H_2] [I_2]}$

=> $rate_n = 4.0*10^{-4} M/s$

So when

$rate_x = 52.0 M/s$

$[H_2] = 1.8 M$

$[I_2] = 0.82 \ M$

We have

$52 .0 = k(1.8)* (0.82)$

$k = \frac{52 .0}{(1.8)* (0.82)}$

$k = 35.23 M^{-2} s^{-1}$

3 0

2 years ago

Select all of the items that are true about a sample of water vapor at 101°C as it cools.

zloy xaker [14]

Answer:

D. Its temperature will remain 100 C until all the vapours condenses

Explanation:

Heat absorbed by a substance to change the state of matter is known as latent heat. This heat is utilized to break the bonds between atoms of the substance so that they can undergo phase change.

So, when water boils at 100 degree Celsius then temperature will remain constant unless and until all the water changes into vapor. As it is the latent heat that breaks the bonds between hydrogen and oxygen atoms of water so that liquid state can change into gaseous state.

Since latent heat is a hidden heat, that is why, it does not get reflected and there is no change in temperature due to it.

Thus, we can conclude that it is true that temperature will remain at 100°C until all the vapor condenses for a sample of water vapor at 101°C as it cools.

5 0

3 years ago

How many milliliters of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?

never [62]

Answer: 97.2223 ml

Explanation:

The rule that we will use to solve this problem is:

M2*V1 = M2*V2 where:

M1 is the initial concentration = 3.5 m

V1 is the initial volume = 0.25 l = 250 ml

M2 is the final concentration = 9 m

V2 is the final volume that we need to find

Substitute with the givens in the above equation to get V2 as follows:

3.5*250 = 9*V2

V2 = <em><u>97.2223 ml</u></em>

3 0

2 years ago

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The vapor pressure of pure water at 110 °C is 1070 torr. A solution of ethylene glycol and water has a vapor pressure of 1.00 at

Kitty [74]

Answer:

idkidkidkidkidkidkidkidkidkidklookitup

7 0

3 years ago

Read 2 more answers