How much energy, in Joules, does one microwave with wavelength of 9.0 meters carry?

. What is the acceleration of a 25.05 kg mass being pushed by a 10.0 N force? What is the acceleration of a 24.00 kg mass pushed

Tomtit [17]

a 25.05kg mass being pushed by a 10 N force should be 15.05

24kg pushed by 8N should be 16

4 0

3 years ago

g n the following three compounds(1,2,3) arrange their relative reactivity towards the reagent CH3Cl / AlCl3. Justify your order

Sedbober [7]

Answer:

3 > 2> 1

Explanation:

Aromatic compounds undergo electrophilic substitution reaction which passes through a positively charged intermediate to yield the product.

Substituted benzenes may be more or less reactive towards electrophilic aromatic substitution than benzene molecule depending on the nature of the substituent.

Certain substituents increase the ease of reaction of benzene towards aromatic substitution.

If we look at the compounds closely, we will notice that toluene reacts readily with CH3Cl / AlCl3. This is because, the methyl group is electron donating hence it stabilizes the positively charged intermediate produced in the reaction.

Carbonyl compounds are electron withdrawing substituents hence they decrease the magnitude of the positive charge and hence decrease the rate of electrophilic aromatic substitution.

3 0

3 years ago

WILL GIVE BRAINLIEST!

Oliga [24]

Answer:

A

Explanation:

Increasing the the temperature would favour the endothermic reaction which is the forward direction however increasing the pressure would make the reaction try to counteract this change by favouring the reaction that would create more products so the equilibrium will shift left instead of right.

Hope this helps.

4 0

2 years ago

Gaseous butane, CH3(CH2)2CH, reacts with gaseous oxygen gas, O2, to produce gaseous carbon dioxide, CO2, and gaseous water, H2O.

weeeeeb [17]

Answer:

Percentage yield of carbon dioxide is 49.9%

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2CH3(CH2)2CH3 + 13O2 —> 8CO2 + 10H2O

OR

2C4H10 + 13O2 —> 8CO2 + 10H2O

Next, we shall determine the masses of butane and oxygen that reacted and the mass of carbon dioxide produced from the balanced equation. This is illustrated below:

Molar mass of butane C4H10 = (12×4) + (10×1)

= 48 + 10

= 58 g/mol

Mass of C4H10 from the balanced equation = 2 × 58 = 116 g

Molar mass of O2 = 16 × 2 = 32 g/mol

Mass of O2 from the balanced equation = 13 × 32 = 416 g

Molar mass of CO2 = 12 + (16×2)

= 12 + 32

= 44 g/mol

Mass of CO2 from the balanced equation = 8 × 44 = 352 g

Summary:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen to produce 352 g of carbon dioxide.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen.

Therefore, 34.29 g of butane will react with = (34.29 × 416) / 116 = 122.97 g of oxygen.

From the calculation made above, we can see clearly that only 122.97 g out of 165.7 g of oxygen reacted completely with 34.29 g of butane. Therefore, butane is the limiting reactant and oxygen is the excess reactant.

Next, we shall determine the theoretical yield of carbon dioxide.

In this case, we shall use the limiting reactant because it will give the maximum yield of carbon dioxide as all of it is used up in the reaction.

The limiting reactant is butane and the theoretical yield of carbon dioxide can be obtained as follow:

From the balanced equation above,

116 g of butane reacted to produce 352 g of carbon dioxide.

Therefore, 34.29 g of butane will react to produce = (34.29 × 352) / 116 = 104.05 g of carbon dioxide.

Therefore, the theoretical yield of carbon dioxide is 104.05 g

Finally, we shall determine the percentage yield of carbon dioxide as follow:

Actual yield of carbon dioxide = 51.9 g

Theoretical yield of carbon dioxide = 104.05 g

Percentage yield of carbon dioxide =?

Percentage yield = Actual yield /Theoretical yield × 100

Percentage yield of carbon dioxide = 51.9 / 104.05 × 100

Percentage yield of carbon dioxide = 49.9%

7 0

3 years ago

Plz help with this........

Elodia [21]

<h2>GREETINGS!</h2><h2>_____________________________________</h2><h3>Answer:</h3>

ITS $C_{4}H_{10}$ AND $C_{5}H_{12}$

<h2>_____________________________________</h2><h3><u>GENERAL FORMULA OF ALKANE</u></h3><h3> $C_{n}H_{2n+2}$ </h3>

Where n is the number of CARBONS

A)

By using the General Formula of Alkanes having 4 carbon atoms is

$C_{4}H_{2x4+2}$

$C_{4}H_{10}$

C)

By using the General Formula of Alkanes having 5 carbon atoms is

$C_{5}H_{2x5+2}$

$C_{5}H_{12}$

IF YOU USE THE SAME FORMULA FOR THE OTHER TWO OPTIONS THE OUTCOME WILL NOT BE AS SAME AS GIVEN IN THE QUESTION SO THOSE TWO ARE CAN NOT BE OUR ANSWER

<h2>_____________________________________</h2><h2>HOPE THIS HELPS!</h2>

3 0

3 years ago