Answer:
cis-hex-2-ene as produced as major product.
Explanation:
- In presence of (Lindlar catalyst) and , alkynes are reduced to alkene.
- molecules first adsorbed onto metal surface through chemisorption.
- When alkyne molecule comes in close proximity to the metal surface, H atoms add onto triple bond to reduce it to alkene.
- Two H atoms add onto alkyne from same face of metal. So, (Z) or cis-isomer of alkene is produced as a major product.
- Reaction mechanism has been shown below.
Answer:
FC of C = -1
General Formulas and Concepts:
- Lewis Dot Structures
- Resonance Structures
- Formal Charge: FC = # of valence e⁻ - # of lone e⁻ - # of bonds
Explanation:
<u>Step 1: Define</u>
Carbon (C)
- 4 valence e⁻
- 2 lone e⁻
- 3 bonds
Oxygen (O)
- 6 valence e⁻
- 2 lone e⁻
- 3 bonds
<u>Step 2: FC of C</u>
- Substitute: FC = 4e⁻ - 2e⁻ - 3
- Subtract: FC = -1
The number of sulfate ions that are in 100 ml of a solution of 0.0020 M Fe2(SO4)3 is 6 x10 ^-4 moles
calculation
find the moles of Fe2(SO4)3 that dissociated
moles = molarity x volume in liters
volume in liters = 100/1000 = 0.1 liters
molarity =0.002 M
moles = 0.002 x0.1 =2 x10 ^-4 moles
write the equation for dissociation
Fe2(SO4)3 = 2fe^3+ + 3 SO4^2-
by use of mole ratio between Fe2(SO4)3 to SO4^2- which is 1:3 therefore the moles of SO4^2- is
= 0.0002 x3 = 6 x10 ^-4 moles
Answer:
49.5J/°C
Explanation:
The hot water lost some energy that is gained for cold water and the calorimeter.
The equation is:
Q(Hot water) = Q(Cold water) + Q(Calorimeter)
<em>Where:</em>
Q(Hot water) = S*m*ΔT = 4.184J/g°C*54.56g*(80.4°C-59.4°C) = 4794J
Q(Cold water) = S*m*ΔT = 4.184J/g°C*47.24g*(59.4°C-40°C) = 3834J
That means the heat gained by the calorimeter is
Q(Calorimeter) = 4794J - 3834J = 960J
The calorimeter constant is the heat gained per °C. The change in temperature of the calorimeter is:
59.4°C-40°C = 19.4°C
And calorimeter constant is:
960J/19.4°C =
<h3>49.5J/°C</h3>
<em />
Answer:
To help evenly distribute heat throughout the solution
Explanation:
The purpose of stirring a solution while being heated would be<u> to evenly distribute heat throughout the solution.</u>
<em>When a vessel containing a solution is heated, the molecules at the lower portion of the vessel get heated first before heat graduate radiates around the entire solution. Stirring the solution will ensure that the process of heat distribution around the entire solution is quickened.</em>
Stirring a solution while heating does not slow down the reactions that might occur in the solution, does not encourage sudden boiling of the solution, and neither does it prevent solute from dissolving into the solution.