Answer:
3. 2.00 L of air at 100°C has twice the pressure of the same 2.00 L of air at 50°C
Explanation:
1) doubling the pressure of a gas doubles its volume
This is incorrect because by increasing the pressure volume is going to be decreased.
2) 2.00 L of air at 227°C has twice the pressure of the same 2.00 L of air at 23°C
This is also incorrect because 2 L air at 227 °C will have the pressure more than twice time as compared to the 2L air at 23°C.
3. 2.00 L of air at 100°C has twice the pressure of the same 2.00 L of air at 50°C
This is correct;
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
thus, by increasing the temperature pressure is also goes to increase in the same ratio.
4. halving the pressure of a gas halves its volume
This is incorrect because halving the pressure of gas increasing its volume.
% yield = 74.35
<h3>Further explanation</h3>
Given
12 dm³ ethene = 12 L
18.4 g ethanol(actual)
Required
The percentage yield
Solution
Reaction
C₂H₄(g) + H₂O(g) ⇒ C₂H₅OH(g)
Assume at STP, 1 mol gas = 22.4 L
mol ethene :
= 12 L : 22.4 L
= 0.538
From equation, mol ratio C₂H₅OH : C₂H₄ = 1 : 1, so mol C₂H₅OH = 0.538
Mass Ethanol (MW=46 g/mol) ⇒ theoretical
= 0.538 x 46
= 24.748 g
% yield = (actual/theoretical) x 100%
% yield = (18.4/24.748) x 100%
% yield = 74.35
Answer:
The particles gain more kinetic energy and they move around faster
Answer:
Law of Conservation of Mass
Explanation:
Law states that matter cannot be created or destroyed. So when you balance an equation, you are making sure you have the same number of atoms for each element on each side of the equation.
ans D) the process is endothermic
C(s, diamond + O2 (g)-->CO2(g),∆H= -395.5kJ