How many grams are KBr are needed to make a saturated solution in 100g of water at 30c
1 answer:
Explanation:
To calculate that you need to know the value of the Kps (constant of solubility) at 30°C of KBr in water.
<u>When the product of the concentrations of both ions (Br- and K+) equals the Kps, the solution is saturated. </u>
Given the disociation of the salt in water:
The concentration of both ions are equal (1:1 ratio) and the same as the concentration of KBr added.
The Kps:
[KBr] are <u>moles of the salt per litre of water</u>
Assuming a density of water of 1 g/cm3, 100 g are 0.1 litre
To calculate the mass:
where M is the molecular weight of the salt.
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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>
Explanation:
the answer and explanation is in the picture
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The ideal gas law may be written as
where
p = pressure
ρ =density
T = temperature
M = molar mass
R = 8.314 J/(mol-K)
For the given problem,
ρ = 0.09 g/L = 0.09 kg/m³
T = 26°C = 26+273 K = 299 K
M = 1.008 g/mol = 1.008 x 10⁻³ kg/mol
Therefore
Note that 1 atm = 101325 Pa
Therefore
p = 2.2195 x 10⁵ Pa
= 221.95 kPa
= (2.295 x 10⁵)/101325 atm
= 2.19 atm
Answer:
2.2195 x 10⁵ Pa (or 221.95 kPa or 2.19 atm)
where
p = pressure
ρ =density
T = temperature
M = molar mass
R = 8.314 J/(mol-K)
For the given problem,
ρ = 0.09 g/L = 0.09 kg/m³
T = 26°C = 26+273 K = 299 K
M = 1.008 g/mol = 1.008 x 10⁻³ kg/mol
Therefore
Note that 1 atm = 101325 Pa
Therefore
p = 2.2195 x 10⁵ Pa
= 221.95 kPa
= (2.295 x 10⁵)/101325 atm
= 2.19 atm
Answer:
2.2195 x 10⁵ Pa (or 221.95 kPa or 2.19 atm)