½H2(g) + ½I2(g) → HI(g) ΔH = +6.2 kcal/mol
or...
½H2(g) + ½I2(g) + 6,2kcal/mole → HI(g)
________
21.0 kcal/mole + C(s) + 2S(s) → CS2(l)
or...
C(s) + 2S(s) → CS2(l) ΔH = +2,1 kcal/mole
_________
ΔH > 0 ----------->>> ENDOTHERMIC REACTIONS
Answer:
kJ/mol
Explanation:
Given and known facts
Mass of Benzene 
grams
Mass of water 
grams
Standard heat capacity of water 
J/g∙°C
Change in temperature ΔT 
°C
Heat
Heat released by benzine is - 7.82 kJ
Now, we know that
grams of benzene release 
kJ heat
So, 
g benzine releases
kJ/g
mol C6H6
Heat released
kJ/mol
<span>Oil and water don't mix because oil is made up of non-polar molecules while water molecules are polar in nature. Because water molecules are electrically charged, they get attracted to otherwater molecules and exclude the oil molecules. (this is from wiki)</span>
<h3>
Answer:</h3>
1.93 g
<h3>
Explanation:</h3>
<u>We are given;</u>
The chemical equation;
2C₂H₆(g) + 7O₂(g) → 4CO₂(g) + 6H₂O(l) ΔH = -3120 kJ
We are required to calculate the mass of ethane that would produce 100 kJ of heat.
- 2 moles of ethane burns to produce 3120 Kilo joules of heat
Number of moles that will produce 100 kJ will be;
= (2 × 100 kJ) ÷ 3120 kJ)
= 0.0641 moles
- But, molar mass of ethane is 30.07 g/mol
Therefore;
Mass of ethane = 0.0641 moles × 30.07 g/mol
= 1.927 g
= 1.93 g
Thus, the mass of ethane that would produce 100 kJ of heat is 1.93 g
It's A. volume
Pressure =
with const depends on the chosen unit of volume
I think so...
