Protons: 12
Neutrons: 13
<span>Electrons: 12</span>
Answer:
66 g of CO₂
Solution:
The Balance Chemical Reaction is as follow,
C₂H₂ + 5/2 O₂ → 2 CO₂ + H₂O
Or,
2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O ------- (1)
Step 1: Find out the limiting reagent as;
According to Equation 1,
56.1 g (2 mole) C₂H₂ reacts with = 160 g (5 moles) of O₂
So,
125 g of C₂H₂ will react with = X g of O₂
Solving for X,
X = (125 g × 160 g) ÷ 56.1 g
X = 356.5 g of O₂
It means for total combustion of Ethylene we require 356.5 g of O₂, but we are only provided with 60.0 g of O₂. Therefore, O₂ is the limiting reagent and will control the yield.
Step 2: Calculate Amount of CO₂ produced as;
According to Equation 1,
160 g (5 mole) O₂ produces = 176 g (4 moles) of CO₂
So,
60.0 g of O₂ will produce = X g of CO₂
Solving for X,
X = (60.0 g × 176 g) ÷ 160 g
X = 66 g of CO₂
Answer: 750ml
Explanation:
Using charle's law
V1/T1=V2/T2
V1= 500ml
T1= -73⁰C
V2= ?
T2=27⁰C
We can see that the temperature is in Celsius
Now,we will convert to Kelvin
Kelvin= 273+ Celsius
So convert the Celsius value to Kelvin
For T1= 273+(-73)
T1= 273-73
T1= 200K
For T2= 273+27
T2= 300K
V1/T1=V2/T2
500/200=V2/300
Cross multiply
200×V2=500×300
200V2= 150000
V2= 150000/200
V2= 750ml
So,
750ml of gas will occupy at 27⁰C
The correct answer to this question is letter "A. homogeneous mixture." The following characteristics describe the type of mixture, which is a homogeneous mixture. The substance is mixed uniformly throughout and each part of <span>the substance contains the same ratio of materials with the same properties</span>