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Chapter 5: Q8E (page 268)

Question: How much would the temperature of 275 g of water increase if 36.5 kJ of heat were added?

Short Answer

Expert verified

The rise in the temperature of water = 31.72\(^0C\)

Step by step solution

01

Specific heat

The heat required to raise the temperature of a substance is given by the formula Q = C × m ×∆ T.

Where “C” is the specific heat of the substance:

“m” is the mass of the substance, and

“∆T” is the change in the temperature of the substance.

02

Increase in temperature

We know from the given details that:

C = 4.184 J/g °C(Table 5.1)

m = 275 g

Q = 36.5kJ = 36500 J

By putting the values above in the equation Q = C × m × ∆ T, we get:

36500 = 4.184\( \times \)275\( \times \)\(\Delta \)T.

\(\Delta \)T = \(\frac{{36500}}{{4.184 \times 275}} = {31.72^0}C\).

Therefore, the rise in the temperature of 275 g of water = 31.72\(^0C\).

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Most popular questions from this chapter

How much heat is produced by the combustion of 125 g of acetylene?

How much heat, in joules, must be added to a 5.00×10 2 g iron skillet to increase its temperature from 25°C to 250 °C? The specific heat of iron is 0.451 J/g °C.

A 248-g piece of copper is dropped into 390 mL of water at 22.6°C. The final temperature of the water was measured as 39.9 °C. Calculate the initial temperature of the piece of copper. Assume that all heat transfer occurs between the copper and the water.

Calculate ∆H for the reaction described by the equation. (Hint: use the value for the approximate amount of heat absorbed by the reaction that you calculated in a previous exercise.)

Ba(OH)2. 8H2O(s) + 2NH4SCN(aq) → Ba(SCN)2(aq) + 2NH3(aq) + 10H2O(l)

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 °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—for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of O2 per liter.)

(c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation,ΔHf °of propane given thatΔHf °of H2O(l) = −285.8 kJ/mol andΔHf °of CO2(g) = −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.
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