Ask question

Ask question

All categories

3 years ago

14

help me balance & find how many grams of water would be produced if 20.0 liters of O2 gas were burned at a temperature of -1

0.O*c & a pressure of 1.3 atm

1 answer:

vova2212 [387]3 years ago

6 0

I have finished the balanced equation part. Give me a little more time for part B.

Edit: Found a way so here it is as well.

You might be interested in

Given: N2 + 3Cl2 → 2NCl3, ΔH = 464 kJ/mol Use the given bond energies and the periodic table to calculate the energy change in t

guapka [62]

The given chemical reaction is:

$N_{2}+3Cl_{2}-->2NCl_{3}$

Δ $H^{0}_{reaction}=$ ∑BE(reactants)-∑BE(products)

= {(941 kJ/mol) + (3 * 242 kJ/mol)} -[{2*(3*200 kJ/mol)}]

= 467 kJ/mol

Calculating the change in heat when 85.3 g chlorine reacts in the above reaction:

Moles of chlorine = $85.3 g Cl_{2}* \frac{1 mol Cl_{2}} {70.91 g Cl_{2} }$

= 1.20 mol $Cl_{2}$

Heat change when 1.20 mol chlorine reacts

= $1.20 mol * \frac{467kJ}{mol} =560.4 kJ$

6 0

3 years ago

Why do elements undergo chemical reactions?

DaniilM [7]

Answer:

They have to

Explanation:

It occurs when 2 or more molecules interact and their bonds change

6 0

4 years ago

What is the chemical composition of our<br> air? Name the chemical properties.

RoseWind [281]

Answer:

oxygen(O2), Nitrogen(N2) ,water (H2O),Carbon dioxide (CO2)

4 0

3 years ago

Will give brainliest <br><br> Process name of water vapor to ice

Elenna [48]

Answer:

<u>Deposition</u>

this is the process of a substance changing its state from gas to solid. Solid to gas is known as sublimation

8 0

3 years ago

Read 2 more answers

What is the theoretical yield of aspirin ( C 9 H 8 O 4 ), which has a molar mass of 180.15 g/mol, possible when reacting 3.03 g

pantera1 [17]

Answer:

The theoretical yield of aspirin is 3.95 grams

Explanation:

Step 1: Data given

Mass of salicylic acid = 3.03 grams

Volume of acetic anhydride = 3.61 mL

Density of acetic anhydride = 1.08 g/cm³

Step 2: The balanced equation

C4H6O3+C7H6O3→C9H8O4+C2H4O2

Step 3: Calculate moles salicylic acid

Moles salicylic acid = mass salicylic acid / molar mass salicylic acid

Moles salicylic acid = 3.03 grams /138.121 g/mol

Moles salicylic acid = 0.0219 moles

Step 4: Calculate mass acetic anhydride

Mass acetic anhydride = volume * density

Mass acetic anhydride = 3.61 mL * 1.08 g/mL

Mass acetic anhydride = 3.90 grams

Step 5: Calculate moles acetic anhydride

Moles acetic anhydride = 3.90 grams / 102.09 g/mol

Moles acetic anhydride = 0.0382 moles

Step 6: Calculate limiting reactant

For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirin

Salicylic acid is the limiting reactant. It will completely be consumed. (0.0219 moles). Acetic anhydride is in excess. There will react 0.0219 moles. There remain 0.0382 - 0.0219 =0.0163 moles

Step 7: Calculate moles aspirin

For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirin

For 0.0219 moles salicylic acid we'll have 0.0219 moles aspirin

Step 8: Calculate theoretical yield of aspirin

Mass of aspirin = moles aspirin *molar mass aspirin

Mass of aspirin = 0.0219 moles *180.15 g/mol

Mass of aspirin = 3.95 grams

The theoretical yield of aspirin is 3.95 grams

7 0

4 years ago