Answer:
The energy released will be -94.56 kJ or -94.6 kJ.
Explanation:
The molar mass of methane is 16g/mol
The given reaction is:
![CH_{4}(g) + 2O_{2} (g) --> CO_{2} (g)+ 2H_{2}O(l)](https://tex.z-dn.net/?f=CH_%7B4%7D%28g%29%20%2B%202O_%7B2%7D%20%28g%29%20--%3E%20CO_%7B2%7D%20%28g%29%2B%202H_%7B2%7DO%28l%29)
the enthalpy of reaction is given as ΔH = -890.0 kJ
This means that when one mole of methane undergoes combustion it gives this much of energy.
Now as given that the amount of methane combusted = 1.70g
The energy released will be:
![=\frac{energy released by one moleXgiven mass}{molarmass} =\frac{-890X1.7}{16}= -94.56 kJ](https://tex.z-dn.net/?f=%3D%5Cfrac%7Benergy%20released%20by%20one%20moleXgiven%20mass%7D%7Bmolarmass%7D%20%3D%5Cfrac%7B-890X1.7%7D%7B16%7D%3D%20-94.56%20kJ)
Answer:
it woul be 263
Explanation:
becaue it adds up like that
Answer:
d. Heat is released from the reaction
Explanation:
A negative enthalpy change indicates that it is an exothermic reaction. Exothermic reactions release heat.
Answer:
Q4. 2H₂ + O₂ ⟶ 2H₂O; 5; 2
Q5. 24; 30; H₂; 0; 5
Explanation:
Q4.
The equation for the reaction is
2H₂ + O₂ ⟶ 2H₂O
One O₂ molecule reacts with 2H₂ molecules.
![\text{No. of O$_{2}$ molecules} = \text{10 H$_{2}$ molecules } \times \dfrac{\text{1 O$_{2}$ molecule }}{\text{2 H$_{2}$ molecules}} = \textbf{5 O$_{\textbf{2}}$ molecules}\\\\\text{Ten hydrogen molecules react with $\textbf{five}$ oxygen molecules.}](https://tex.z-dn.net/?f=%5Ctext%7BNo.%20of%20O%24_%7B2%7D%24%20molecules%7D%20%3D%20%5Ctext%7B10%20H%24_%7B2%7D%24%20molecules%20%7D%20%5Ctimes%20%5Cdfrac%7B%5Ctext%7B1%20O%24_%7B2%7D%24%20molecule%20%7D%7D%7B%5Ctext%7B2%20H%24_%7B2%7D%24%20molecules%7D%7D%20%3D%20%5Ctextbf%7B5%20O%24_%7B%5Ctextbf%7B2%7D%7D%24%20molecules%7D%5C%5C%5C%5C%5Ctext%7BTen%20hydrogen%20molecules%20react%20with%20%24%5Ctextbf%7Bfive%7D%24%20oxygen%20molecules.%7D)
We started with seven oxygen molecules. Five of them reacted, so
Two O₂ molecules did not react.
Q5.
Two water molecules form from two hydrogen molecules.
Two water molecules form from one oxygen molecule
Hydrogen forms fewer water molecules of water, so
Hydrogen is the limiting reactant.
The 24 hydrogen molecules will be completely used up.
The number of hydrogen molecules remaining at the end of the reaction is zero.
They have reacted with 12 O₂ molecules.
The number of O₂ molecules remaining is 17 - 12 = 5