The incomplete combustion of pentane is shown in the balanced equation below. Gi
ID: 989622 • Letter: T
Question
The incomplete combustion of pentane is shown in the balanced equation below. Given H_inc, combust. = -1829.8kJ/mol C_5H_12, add the correct energy term to the appropriate side of the equation 2C_5H_12(I) + 11 O_2 rightarrow10 CO_(g) + 12 H_2O_(g) Use a potential energy diagram to show this reaction For the following equilibrium reaction, predict the effect of each of the changes listed below reaction (shift left, shift right, or no shift). N_2(g) + 3H_2(a) doubleheadarrow 2NH_3(g) + 92 KJ add H_2(g) remove NH_3(g) increase temperature decrease pressure add a catalystExplanation / Answer
6.) Question is not visible. That is the question is partially visible hence cant not be solved with given information.
7.)
For reaction,
N2 (g) + 3H2 (g) ------------> 2NH3 (g)
We will use Le-chatliers princliples to answer the problems
a.) add H2
If more reactant is added, the equation will shift to the right in order to make more product (which will increase the products) . So ,the reaction will shift right.
b.) remove NH3
If more product is added, the equation will shift to the left in order to make less product (which will increase the reactants) . So ,the reaction will shift left.
c.) increase temperature.
N2 + 3 H2 2 NH3, H = -92kJ
This is an exothermic reaction when producing ammonia. If we were to increase the temperature, the equilibrium would shift in such a way as to absorb heat. Since this reaction is endothermic to the left, it would favour the production of more reactant. This reaction is used in the Haber process, which is a good example of the way chemists utilise Le Châtelier's principle. Hence, reaction will shift towards left.
d.) decrease pressure
If we decrease total pressure on the system, now by Le Châtelier's principle the equilibrium would move to increase the pressure. Noting that 4 moles of gas occupy more volume than 2 moles of gas, we can deduce that the reaction will move towards the reactants if we were to decrease the pressure. Hence, reaction will shift towards left.
e.) add a catalyst.
Since, catalyst are added to fasten the reaction and increase the product, so more product will be formed. Hence, the reaction will shift towards right.
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