Answer:
336.6 grams of CO₂ and 183.6 grams of H₂O are formed from 2.55 moles of propane.
Explanation:
In this case, the balanced reaction is:
C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reactant and product participate in the reaction:
- C₃H₈: 1 mole
- O₂: 5 moles
- CO₂: 3 moles
- H₂O: 4 moles
Being the molar mass of each compound:
- C₃H₈: 44 g/mole
- O₂: 16 g/mole
- CO₂: 44 g/mole
- H₂O: 18 g/mole
Then, by stoichiometry, the following quantities of mass participate in the reaction:
- C₃H₈: 1 mole* 44 g/mole= 44 grams
- O₂: 5 moles* 16 g/mole= 80 grams
- CO₂: 3 moles* 44 g/mole= 132 grams
- H₂O: 4 moles* 18 g/mole= 72 grams
So you can apply the following rules of three:
- If by stoichiometry 1 mole of C₃H₈ forms 132 grams of CO₂, 2.55 moles of C₃H₈ how much mass of CO₂ will it form?
mass of CO₂= 336.6 grams
- If by stoichiometry 1 mole of C₃H₈ forms 72 grams of H₂O, 2.55 moles of C₃H₈ how much mass of H₂O will it form?
mass of H₂O= 183.6 grams
<u><em>336.6 grams of CO₂ and 183.6 grams of H₂O are formed from 2.55 moles of propane.</em></u>
This problem has two parts; the first one asking for the concentration of NaBr given both its mass and volume and the second one asking for its volume given both mass and concentration. The answers turn out to be 0.158 M and 211 mL.
<h3>Molarity</h3>
In chemistry, the use of units of concentration depends on both the substances to analyze and their amounts. In such a way, for molarity, one needs the following relationship between the moles of solute and volume of solution:
Thus, for the first part of the problem we first calculate the moles in 2.60 g of NaBr via its molar mass:
Next, we convert the 160. mL to L by dividing by 1000 in order to obtain 0.160 L to subsequently calculate the molarity:
Next, since the moles remain the same and for the second part we are asked for the volume given the concentration, one can solve for the volume so as to obtain:
That in milliliters turns out to be:
Learn more about molarity: brainly.com/question/10053901
0.24 moles of oxygen must be placed in a 3.00 L container to exert a pressure of 2.00 atm at 25.0°C.
The variables given are Pressure, volume and temperature.
Explanation:
Given:
P = 2 atm
V = 3 litres
T = 25 degrees or 298.15 K by using the formula 25 + 273.17 = K
R = 0.082057 L atm/ mole K
n (number of moles) = ?
The equation used is of Ideal Gas law:
PV = nRT
n = 
Putting the values given for oxygen gas in the Ideal gas equation, we get
n = 
= 0.24
Thus, from the calculation using Ideal Gas law it is found that 0.24 moles of oxygen must be placed in a container.
Ideal gas law equation is used as it tells the relation between temperature, pressure and volume of the gas.
Answer:
Pure Substances are made of the same material throughout and have the same properties throughout. Pure substances cannot be separated into other substances. Some examples are carbon, iron, water, sugar, salt, nitrogen gas, and oxygen gas. ... If so, you have a pure substance.
Hope this helps!!
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Chemical. burning is a chemical change
