A 50.0 N force is applied to an object travels with a constant velocity of 20m/s, calculate
1 answer:
You might be interested in
Taking into account the reaction stoichiometry and the definition of STP, 5.4 L of carbon dioxide is produced.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- C₃H₈: 1 mole
- O₂: 5 moles
- CO₂: 3 moles
- H₂O: 4 moles
The following rule of three can be applied: if by reaction stoichiometry 1 mole of C₃H₈ form 3 moles of CO₂, 0.080 moles of C₃H₈ form how many moles of CO₂?
<u><em>amount of moles of CO₂= 0.24 moles</em></u>
<h3>Definition of STP condition</h3>The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.
<h3>Volume of CO₂ produced</h3>You can apply the following rule of three: If by definition of STP 1 mole of CO₂ occupies 22.4 L, 0.24 moles of CO₂ how much volume does it occupy?
<u><em>volume of CO₂= 5.376 L ≅ 5.4 L</em></u>
Finally, 5.4 L of carbon dioxide is produced.
Learn more about
the reaction stoichiometry:
<u>brainly.com/question/24741074</u>
<u>brainly.com/question/24653699</u>
STP conditions:
<u>brainly.com/question/26364483</u>
<u>brainly.com/question/8846039</u>
<u>brainly.com/question/1186356</u>
The mass of water (H₂O) that would be produced is 4.5 g
<h3>Stoichiometry </h3>From the question, we are to determine the mass of water that would be produced.
From the given balanced chemical equation
2C₂H₆ +7O₂ → 4CO₂ +6H₂O
This means
2 moles of C₂H₆ reacts with 7 moles of O₂ to produce 4 moles of CO₂ and 6 moles of H₂O
Now, we will determine the number of moles of each reactant present
- For Ethane (C₂H₆)
Mass = 2.5 g
Molar mass = 30.07 g
Using the formula,
Number of moles of C₂H₆ present =
Number of moles of C₂H₆ present = 0.08314 mole
- For Oxygen (O₂)
Mass = 170g
Molar mass = 31.999 g/mol
Number of moles of O₂ present =
Number of moles of O₂ present = 5.3127 moles
Since
2 moles of C₂H₆ reacts with 7 moles of O₂
Then,
0.08314 mole of C₂H₆ will react with
= 0.58198 mole
Therefore,
0.08314 mole of C₂H₆ reacts with 0.58198 mole of O₂ to produce 3 × 0.08314 moles of H₂O
3 × 0.08314 = 0.24942 mole
Thus, the number of moles of water (H₂O) produced is 0.24942 mole
Now, for the mass of water that would be produced,
Using the formula,
Mass = Number of moles × Molar mass
Molar mass of water = 18.015 g/mol
Then,
Mass of water that would be produced = 0.24942 × 18.015
Mass of water that would be produced = 4.4933 g
Mass of water that would be produced ≅ 4.5 g
Hence, the mass of water (H₂O) that would be produced is 4.5 g
Learn more on Stoichiometry here: brainly.com/question/14271082