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Chapter 5: Q6E (page 268)

Question: How much heat, in joules and in calories, must be added to a 75.0鈥揼 iron block with a specific heat of 0.449 J/g 掳C to increase its temperature from 25 掳C to its melting temperature of 1535 掳C?

Short Answer

Expert verified

The heat required to raise the temperature in joules = 50,849 J

The heat required to raise the temperature in calories = 12,147 calories

Step by step solution

01

Step 1: Specific heat

The heat required (Q) to raise the temperature of a substance is given by the formula Q = C 脳 m 脳鈭� T,where 鈥淐鈥� is the specific heat of the substance, 鈥渕鈥� is the mass of the substance, and 鈥溾垎T鈥� is the change in the temperature of the substance.

02

Calculation of heat in Joules

We know from the given details that:

C = 0.449 J/g 掳C

m = 75 g

T = change in temperature =Tfinal - Tinitial = 15350C 鈥� 250C = 15100C

By putting the values above in the equation Q = C 脳 m 脳 鈭� T, we get:

Q = 75 脳 0.449 脳 1510 = 50,849 J.

The heat required to raise the temperature of 75 g of iron block = 50,849 J

03

Calculation of heat in calories

Also,

1 calorie = 4.184 J.

The heat required to raise the temperature in calories =\(\frac{{50,849}}{{4.186}} = 12147.39cal\)

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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 螖H掳 for reaction(i):

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

Question 11: A piece of unknown solid substance weighs 437.2 g, and requires 8460 J to increase its temperature from 19.3 掳C to 68.9 掳C.

(a) What is the specific heat of the substance?

(b) If it is one of the substances found in Table 5.1, what is its likely identity?

Ethylene, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\), a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80% of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}{\bf{(g) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(g)}} \to {{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH(l)}}\).Using the data in the table inAppendix G, calculate 螖H掳 for the reaction.

Propane, \({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{8}}}\), is a hydrocarbon that is commonly used as a fuel.

(a) Write a balanced equation for the complete combustion of propane gas.

(b) Calculate the volume of air at 25 掳C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later

chapter on gases鈥攆or now use the information that 1.00 L of air at 25 掳C and 1.00 atm contains 0.275 g of O2 per liter.)

(c) The heat of combustion of propane is 鈭�2,219.2 kJ/mol. Calculate the heat of formation,螖Hf 掳of propane given that螖Hf 掳of H2O(l) = 鈭�285.8 kJ/mol and螖Hf 掳of CO2(g) = 鈭�393.5 kJ/mol.

(d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.

The amount of fat recommended for someone with a daily diet of 2000 Calories is 65g. What percent of the calories in this diet would be supplied by this amount of fat if the average number of calories for fat is 9.1 Calories/g?
See all solutions

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