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3 years ago

The chemical equation below shows the combustion of methane (CH4).

Chemistry

2 answers:

Vikki [24]3 years ago

8 0

Answer:

B. 6.15

Explanation:

pishuonlain [190]3 years ago

3 0

According to the chemical equation, the reaction ratio between O2 and CO2 is 2:1, which mean for every 2 moles of O2 reacted there is 1 mole of CO2 formed.

Use the molar mass and mass of O2 to find out the moles of O2: moles of O2 = mass of O2/molar mass of O2 = 8.94g/32.00g/mol = 0.2794 mole. Therefore, the moles of CO2 that formed is 0.2794moles/2 = 0.1397 mole

Use the moles and molar mass CO2 to find out the mass of CO2:
Mass of CO2 = moles of CO2 * molar mass of CO2 = 0.1397 mole * .44.01g/mole = 6.15 g.

So the answer is B 6.15g.

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Butanal, an aldehyde, can be made from 1-bromobutane, but it requires two reactions in sequence. What are the two reagents that

hammer [34]

Answer:

See explanation and image attached

Explanation:

My aim is to convert 1-bromobutane to butanal. The first step is to react the 1-bromobutane substrate with water. This reaction occurs by SN2 mechanism to yield 1-butanol. Hence reagent A is water.

1-butanol is now reacted with an oxidizing agent such as acidified K2Cr2O7 (reagent B) to yield butanal. Note that primary alkanols are oxidized to alkanals.

These sequence of reactions are shown in the image attached.

4 0

3 years ago

The element Oxygen, O, is an example of which of the following?

Anon25 [30]

It is an example of a molecule

5 0

4 years ago

Read 2 more answers

What volume of a 9.00 M NaOH stock solution would you need to make 800. ML of a 0.750 M NaOH solution

joja [24]

Answer: 66.66 ml

Explanation: Using Molarity equation:

$M_1V_1$ (stock solution)= $M_2V_2$ (solution to be prepared)

given: $M_2=0.750M$

$V_2=800ml$

$M_1=9.00M$

$V_1=?$

$9.00M\times V_1$ (stock solution)= $0.750M\times 800ml$ (solution)

$V_1= 66.66ml$

8 0

3 years ago

2 SO2(g) + O2(g) + 2 H2O(ℓ) −→ 2 H2SO4(ℓ)

DIA [1.3K]

Answer:

6116g

Explanation:

2SO2(g) + O2(g) + 2H2O(ℓ) −→ 2H2SO4(ℓ)

We want to find the mass in grams of SO2 that is needed to react with 1527 g of O2. First we must convert the grams of O2 to moles of O2 then to moles of SO2 and then to grams of SO2

So first lets find the molar mass of O2

The mass of oxygen according to a periodic table is 15.999

Using this the mass of O2 would be 15.999(2) = 31.988g

Next we need to identify the mole ratio of O2 to SO2

Looking at the equation for 1 mole of O2 there are two moles of SO2

Next we need to find the molar mass of SO2

Again the mass of oxygen is 15.999g and the mass of Sulfur is 32.066

So the mass of SO2 would be 15.999(2) + 32.066 = 64.064g

Now that we have found all the needed conversions :

1 mol O2 = 31.988g

1 mol O2 = 2 mol SO2

1 mol SO2 = 64.064g

We can now use dimensional analysis to calculate the answer.

Kindly check the attached image to see the table. ( sorry if its a bit blurry )
Explanation : The conversions are used to cancel out the units to get to the final unit which is gSO2.

Once the units are cancelled out except for the gSO2 we mutliply and divide based off of what the table says to do.
Here first we divide 1527 by 31.988. We than multiply by 2. Finally we multiply by 64.064 to get the final answer which is 6116gSO2

7 0

2 years ago

Where does the actual gas exchange happen?

katen-ka-za [31]

Answer:

Option a. is correct.

Explanation:

Gas exchange refers to the the elimination of carbon dioxide from the bloodstream to the lungs and delivery of oxygen from the lungs to the bloodstream. The actual gas exchange happens in the lungs between the alveoli and capillaries (a network of tiny blood vessels). Capillaries are located in the walls of the alveoli.

4 0

4 years ago