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3 years ago

Convert 0.36 atm to kPa

Chemistry

2 answers:

Marrrta [24]3 years ago

8 0

Answer:

36.36

Explanation:

Multiply pressure value by 101 for every problem like this.

Galina-37 [17]3 years ago

4 0

Answer:

36.477

Explanation:

1 atm = 101.325

multiple 0.36 with 101.325

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SO2 reacts with O2 to produce SO3. If 86.0 g of SO2 is placed in a reaction vessel along with excess oxygen gas, how many moles

Salsk061 [2.6K]

Answer:

0,72 moles of SO₂ remain

Explanation:

The reaction is:

2SO₂ + O₂ → 2SO₃

Where molecular mass of SO₂ is 64,066g/mol and of SO₃ is 80,066g/mol.

86,0g of SO₂ are:

86,0g × (1mol / 64,066g) = 1,34 moles of SO₂.

50,0g of SO₃ are:

50,0g × (1mol / 80,066g) = 0,62 moles of SO₃.

Now, as 2 moles of SO₂ produce 2 moles of SO₃, the moles of SO₂ that remain after the reaction are the initial moles of SO₂ - moles of SO₃:

1,34 moles - 0,62 moles =

0,72 moles of SO₂ remain

I hope it helps!

7 0

3 years ago

By whom is chemistry used in the real world

Alexxx [7]

People who make medicine.

8 0

4 years ago

An example of an extensive property of matter is? temp pressure mass hardness

Gelneren [198K]

I believe the answer is mass :)

7 0

3 years ago

How many grams of NH4Cl (ammonium chloride) should dissolve in 50mL of water at 20 degrees Celsius?

Anna71 [15]

Answer:

about 19 or 20 g

Explanation:

To do this, is neccesary to watch a solubility curve of this compound. This is the only way that you can know how many grams are neccesary to dissolve this compound in 50 mL of water to a given temperature.

Now, if you watched the attached graph, you can see the solubility curve of many compounds in 100 g of water (or 100 mL of water). So, to know how many do you need in 50 mL, it's just the half.

So watching the curve, you can see that at 20 °C, we simply need between 35 g and 40 g. Let's just say we need 38 grams of NH4Cl to be dissolved in 100 mL of water.

So, in 50 mL, it's just the half. So, we only need 19 g or 20 g of NH4Cl at 20 °C, to dissolve this compound in water.

3 0

3 years ago

The molar mass of carbon dioxide (CO2) is 44.01 g/mol. The molar mass of water (H2O) is 18.01 g/mol. A reaction uses 528 g of CO

Nataly [62]

The reaction that results from this is:

H2O + CO2 --> H2CO3

Stoichiometric ratio between water and CO2 is 1:1. So we can say that for every Mole of CO2, we need 1 Mole of water to produce 1 Mole of H2CO3. Thus as n=m/M we can find n = 528/44.01 = 11.997 ~ 12Mol.

therefore, we need 12 moles of water.

5 0

4 years ago

Read 2 more answers