Answer:
C8H18(g) + 12.5O2(g) -> __8__CO2(g) + 9H2O(g) + heat
CH4(g) + _2___O2(g) -> ____CO2(g) + _2___H2O(g) + heat
C3H8(g) + _5___O2(g) -> _3___CO2(g) + __4__H2O(g) + heat
2C6H6(g) + __15__O2(g) -> __12__CO2(g) + __6__H2O(g) + heat
Explanation:
I hope it helps!
<u>Given:</u><u> </u>
Mass of Nitrogen (N₂) gas = 75 grams
<u>Finding the number of moles of N₂:</u><u> </u>
We know that the molar mass of N₂ is 28 grams/mole
Number of moles = Given mass / Molar mass
Number of moles = 75 / 28
Number of moles = 2.68 moles
Hence, there are 2.68 moles in 75 grams of Nitrogen Gas
Answer:
-100.125
Explanation:
We are given
CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) △H = -890.0 kJ/mol
The given information is for complete reaction
we have 1.8grams of Methane
Molar mass of CH4 = 16
No of moles of Methane = 1.8/ 16
= 0.1125
So the amount of the heat will be released from the amount of the methane
Q = No of moles*( -890.0 kJ/mol)
= 0.1125*(-890)
= -100.125kJ/mole
Therefore the amount of Energy released from 1.8 grams of methane is equal to -100.125
