Answer:
V₂ = 4.34 L
Explanation:
According to general gas equation:
P₁V₁/T₁ = P₂V₂/T₂
Given data:
Initial volume = 3.50 L
Initial pressure = 150 Kpa (150/101.325 = 1.5 atm)
Initial temperature = 330 K
Final temperature = 273 K
Final volume = ?
Final pressure = 1 atm
Formula:
P₁V₁/T₁ = P₂V₂/T₂
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature
P₂ = Final pressure
V₂ = Final volume
T₂ = Final temperature
Solution:
V₂ = P₁V₁ T₂/ T₁ P₂
V₂ = 1.5 atm × 3.50 L × 273 K / 330 K × 1 atm
V₂ = 1433.3 atm .L. K / 330 k.atm
V₂ = 4.34 L
Ethylene- C2H4 = 85.7% Carbon and 14.3% Hydrogen
Find the atomic masses for each element and multiply it by the number of atoms in the compound, then add.
C- 12.0 * 2= 24.0
H- 1.00 * 4= 4.00
-----------------------
28.0
Take the masses for each element and divide it by the total mass. Then change the answer to get the percent.
C 24.0 / 28.0= .857 = 85.7%
H 4.00 / 28.0= .143 = 14.3%
<h3>
Ethylene is 85.7% Carbon and 14.3% Hydrogen </h3>
Answer is: a<span> fruit and oatmeal bar contains 142000 calories.
</span>A nutritional calorie<span>, or kilocalorie, is equal to 1000 calories.
</span>E = 142 kcal · 1000 cal/kcal.
E = 142 000 cal.
Calorie (cal)<span>, or small calorie, is the amount of energy needed to heat one gram of water by one degree Celsius.
</span><span>One small calorie is approximately 4.2 joules.
</span>A calorie is a unit of energy.
Answer:
The value of for this reaction at 1200 K is 4.066.
Explanation:
Partial pressure of water vapor at equilibrium =
Partial pressure of hydrogen gas at equilibrium =
Total pressure of the system at equilibrium P = 36.3 Torr
Applying Dalton's law of partial pressure to determine the partial pressure of hydrogen gas at equilibrium:
The expression of is given by:
The value of for this reaction at 1200 K is 4.066.
Answer:
Pottasium reacts with water vigorously and the reation is exothermic. The heat released causes the hydrogen released to ignite
Explanation: