Molecular bromine is 24 percent dissociated at 1600 k and 1.00 bar in the equilibrium br2 (
1 answer:
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Answer:
CO = zero
CO2 =1 bar
O2 = 2.02 bar
Explanation:
We are given
initial pressure of CO = 1bar
total pressure = 3.52 bar
so initial pressure of O2 = 3.52 - 1 = 2.52 bar
the reaction is
2CO + O2 → 2CO2
using the unitary method
2 moles of CO2 → 1 mole of O2
1 bar of CO → (required)
but we have more oxygen present , that means CO is the limiting reagent
- Final pressure of CO will be zero as it is the limiting reagent so it will be consumed completely
- 1 bar of CO →
of CO2
- 2.52 bar O2 (initially) - 0.5 bar (reacted) = 2.02bar O2
Answer:
1.17 grams
Explanation:
Let's consider the balanced equation for the combustion of ethylene.
C₂H₄(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(l)
We can establish the following relations:
- 1411 kJ are released (-1411 kJ) when 1 mole of C₂H₄ burns.
- The molar mass of C₂H₄ is 28.05 g/mol.
The grams of C₂H₄ burned to give 59.0 kJ of heat (q = -59.0 kJ) is: