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Chapter 5: Q28E (page 227)

The reaction of 50ml of acid and 50ml of base described in example 5.5 increased the temperature of the solution by 6.9 degrees. How much would the temperature have increased if 100ml of acid and 100ml base had been used in the same calorimeter starting at the same temperature of 22˚C? Explain your answer.

Short Answer

Expert verified

The temperature increases by 3.45˚C if 100 ml of the acid and 100 ml of the base are taken in the same calorimeter mentioned in example 5.5.

Step by step solution

01

Given data

To visualize what is going on, imagine that you combined the two solutions so quickly that no reaction takes place when they are combined, then after mixing, the reaction takes place.

The moment the two solutions are mixed, you have 100 ml of the acid at 22˚C and 100 ml of the base at 22˚C. HCl and NaOH then react until the solution’s temperature reaches 28.9˚C. In this example, through proper calculations, we find the value of the heat of the reaction to beqreaction = -qsolution= -2.89kJ.

02

Heat of the reaction

Since the solution is aqueous, we can proceed in terms of the water’s specific heat and mass. The density of the water is 1.0 g/ml, so 200.0 ml has a mass of about 200 g.

The specific heat of the water is approximately 4.18 J/g˚C, and from example 5.5, the heat of the reaction is -2.89 kJ.

03

Calculation of temperature

Substitute the values into the equation below.

qsolution= (c × m × ΔT)solution

-2.89×103J =(4.18J/g˚C)(200g)(25.2˚C-24.1˚C)(∆T)

∆T = 3.45˚C

Therefore, the temperature increases by 3.45˚C.

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Most popular questions from this chapter

Aluminum chloride can be formed from its elements:

(i)\({\bf{2Al(s) + 3C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ = ?}}\)

Use the reactions here to determine the ΔH° for reaction(i):

\(\begin{array}{*{20}{l}}{\left( {{\bf{ii}}} \right){\rm{ }}{\bf{HCl(g)}} \to {\bf{HCl(aq) \Delta H^\circ (ii) = - 74}}{\bf{.8 kJ}}}\\{\left( {{\bf{iii}}} \right){\rm{ }}{{\bf{H}}_{\bf{2}}}{\bf{(g) + C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2HCl(g) \Delta H^\circ (iii) = - 185 kJ}}}\\{\left( {{\bf{iv}}} \right){\rm{ }}{\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq)}} \to {\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ (iv) = + 323 kJ}}}\\{\left( {\bf{v}} \right){\rm{ }}{\bf{2Al(s) + 6HCl(aq)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g) \Delta H^\circ (v) = - 1049 kJ}}}\end{array}\)

If a reaction produces 1.506 kJ of heat, which is trapped in 30.0 g of water initially at 26.5 °C in a calorimeter like that in Figure 5.12, what is the resulting temperature of the water?

When 0.963 g of glucose, C6H6, is burned in a bomb calorimeter, the temperature of the calorimeter increases by 8.39°C. The bomb has a heat capacity of 784 J/°C and is submerged in 925 mL of water. How much heat was produced by the combustion of the glucose sample?

Calculate the heat of combustion of 1 mole of ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\)(l), when \({{\bf{H}}_{\bf{2}}}{\bf{O}}\)(l) and \({\bf{C}}{{\bf{O}}_{\bf{2}}}\)(g) are formed.

Use the following enthalpies of formation: \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\)(l), −278 kJ/mol; \({{\bf{H}}_{\bf{2}}}{\bf{O}}\)(l), −286 kJ/mol; and \({\bf{C}}{{\bf{O}}_{\bf{2}}}\)(g), −394 kJ/mol.

Both propane and butane are used as gaseous fuels. Which compound produces more heat per gram when burned?
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