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Aleks [24]
3 years ago
5

You have a 28.2-g sample of a metal heated to 95.2°c. you drop it in a calorimeter with 100. g of water at 25.1°c. the final tem

perature of the water is 31.0°c. assuming no heat loss to the surroundings nor the calorimeter, calculate the heat capacity of the metal.
Chemistry
1 answer:
Vlad [161]3 years ago
4 0

The heat lost by the metal should be equal to the heat gained by the water. We know that the heat capacity of water is simply 4.186 J / g °C. Therefore:

100 g * 4.186 J / g °C * (31°C – 25.1°C) = 28.2 g * Cp * (95.2°C - 31°C)

<span>Cp = 1.36 J / g °C</span>

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Mazyrski [523]

Step 1

The reaction is written and balanced:

4 Rb + O2 =>2 Rb2O

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Step 2

Define % yield of product (Rb2O) = (Actual yield/Theoretical yield) x 100

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Step 3

Determine the limiting reactant. The molar masses are needed to solve this:

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Procedure:

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4 x 85.4 g Rb ----- 32 g O2

82.4 g Rb ----- X = 7.72 g O2 are needed

For 82.4 g Rb, 7.72 g O2 is needed, but there is 11.6 g O2. Therefore, O2 is the excess agent. Rb is the limiting reactant.

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Step 4

Determine the theoretical yield from the limiting reactant:

The molar mass Rb2O) 187 g/mol

Procedure:

4 x 85.4 g Rb ------ 2 x 187 g Rb2O

82.4 g Rb ------ X = 90.2 g Rb2O = Theoretical yield

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Step 5

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Answer: % yield = 44 %

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