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Katyanochek1 [597]

3 years ago

10

At constant pressure, the combustion of 5.00 g of c2h6(g) releases 259 kj of heat. what is δh for the reaction given below? 2 c2

h6(g) + 7 o2(g) → 4 co2(g) + 6 h2o(l).

2 answers:

LekaFEV [45]3 years ago

7 0

Answer:

-3108 kJ

Explanation:

Because the combustion is releasing heat, the reaction is exothermic, and because of that, the value of the enthalpy must be negative. When a reaction absorbs heat it is endothermic and the enthalpy is positive.

By the reaction given, there are 2 moles of C₂H₆ reacting. The molar mass of the compound is:

2* 12 g/mol of C + 6* 1 g/mol of H = 30 g/mol

So, 2 moles have 60 g (2mol * 30g/mol).

5.00 g --------------- -259 kJ

60 g --------------- δh

By a simple direct three rule:

5δh = -15540

δh = -3108 kJ

Nonamiya [84]3 years ago

3 0

3120 kJ

<h3>Further explanation</h3>

Given:

At constant pressure, the combustion of 5.00 g of C₂H₅ releases 259 kJ of heat.

Question:

What is ΔH for the reaction given below?

$\boxed{ \ 2C_2H_6_{(g)} + 7O_2_{(g)} \rightarrow 4CO_2_{(g)} + 6H_2O_{(l)} \ }$ .

The Process:

Step-1

Relative atomic mass: C = 12.01 and H = 1.008
Relative molecular mass (Mr) of C₂H₅ = 2(12.01) + 6(1.008) = 30.07 g/mol

Step-2

Let us convert mass to mol of 5 g of C₂H₅.

$\boxed{ \ n = \frac{mass}{Mr} \ } \rightarrow \boxed{ \ n = \frac{5}{30.07} \ } \rightarrow \boxed{ \ n = 0.166 \ moles \ }$

Remember, the combustion of 0.166 moles of C₂H₅ releases 259 kJ of heat.

Step-3

Combustion reactions that release heat into the environment, including the type of exothermic reaction. The exothermic reaction has a negative ΔH because the product enthalpy is lower than the reactant enthalpy of the system.

And now, we will solve the problem of what is ΔH for the reaction given below.

$\boxed{ \ 2C_2H_6_{(g)} + 7O_2_{(g)} \rightarrow 4CO_2_{(g)} + 6H_2O_{(l)} \ }$

Notice that 2 moles of C₂H₅ take part in this reaction.

$\boxed{ \ \Delta H = \frac{2 \ moles}{0.166 \ moles} \times (-259 \ kJ) \ }$

$\boxed{ \ \Delta H = 12.048 \times (-259 \ kJ) \ }$

$\boxed{ \ \Delta H \approx - 3120 \ kJ \ }$

Thus, the combustion of C₂H₅ based on the equation of reaction above releases heat of 3120 kJ.

<h3>Learn more</h3>

How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH) at its boiling point brainly.com/question/4035699
How many moles of O₂ are required for the complete reaction of combustion of C₂H₄ brainly.com/question/3609972
Calculate the enthalpy change per mole of ethylene combusted brainly.com/question/9360310

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