Answer:
A. 8.8 g.
B. 5.3 g.
C. 449 g.
Explanation:
A. Determination of the mass of CO2.
Mole of CO2 = 0.2 mole
Molar mass of CO2 = 12 + (2×16)
= 12 + 32
= 44 g/mol
Mass of CO2 =?
Mole = mass /Molar mass
0.2 = mass of CO2 /44
Cross multiply
Mass of CO2 = 0.2 × 44
Mass of CO2 = 8.8 g
B. Determination of the mass of Na2CO3.
Mole of Na2CO3 = 0.05 mole
Molar mass of Na2CO3 = (2×23) + 12 + (3×16)
= 46 + 12 + 48
= 106 g/mol
Mass of Na2CO3 =?
Mole = mass /Molar mass
0.05 = mass of Na2CO3 /106
Cross multiply
Mass of Na2CO3 = 0.05 × 106
Mass of Na2CO3 = 5.3 g
C. Determination of the mass of Fe(OH)2.
Mole of Fe(OH)2 = 5 moles
Molar mass of Fe(OH)2 = 55.8 + 2(16 + 1)
= 55.8 + 2(17)
= 55.8 + 34
= 89.8 g/mol
Mass of Fe(OH)2 =?
Mole = mass /Molar mass
5 = mass of Fe(OH)2/89.8
Cross multiply
Mass of Fe(OH)2 = 5 × 89.9
Mass of Fe(OH)2 = 449 g.
<span>Electromagnetic radiation will be emitted when any
object has a temperature above zero. The
reason behind this is that atoms within any object at a temperature above
absolute zero have energy, and thus is moving.</span>
<span>Atoms are at least partly composed of charged
particles, changed particles must be moving too.</span>
It is the first one because haven't you ever noticed when you hold a mirror a certain way the light can reflect a light up another surface? so, therefore, the answer that makes the most sense would be the first. :)
Answer:
a) Equilibrium will shift to the left i.e. reactants
b) K will increase with increase in temperature
Explanation:
The given reaction is:
C6H12O6 + 6 O2 ↔ 6 CO2 + 6 H2O ΔH = -2816 kJ/mol
a) As per Le Chatelier's principle, for a reaction at equilibrium any changes in temperature, pressure or concentration will shift the equilibrium in a direction so as to undo the effect of the induced change.
The given reaction is exothermic (since ΔH is negative) i.e. it accompanied by the release of heat and hence an increase in temperature. Therefore, if the temperature is increased the equilibrium will shift in the opposite direction i.e. towards the left or towards the reactants.
b) The equilibrium constant (K) and temperature T are related via the Van't Hoff equation:
![[ln\frac{K2}{K1}=\frac{-\Delta H}{R}[\frac{1}{T2}-\frac{1}{T1}]](https://tex.z-dn.net/?f=%5Bln%5Cfrac%7BK2%7D%7BK1%7D%3D%5Cfrac%7B-%5CDelta%20H%7D%7BR%7D%5B%5Cfrac%7B1%7D%7BT2%7D-%5Cfrac%7B1%7D%7BT1%7D%5D)
In the given reaction, ΔH is negative and the condition is T2>T1
Therefore, K2 > K1
The value of equilibrium constant will increase with increase in temperature
