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Alexxx [7]
2 years ago
6

A molten sample of 1.00kg of iron with a specific heat of 0.385J/g.K at 1000.K is immersed in a sample of water. If the water ab

sorbs 270 kJ of heat what is the final temperature of the iron?
Chemistry
1 answer:
Schach [20]2 years ago
6 0

Answer:

Final T = 298.7K

Explanation:

In this problem, the heat given for the iron is equal to the heat that water absorbs. Using the equation:

Q = C*m*ΔT

<em>Where Q is heat given = 270000J</em>

<em>C is specific heat of substance = 0.385J/gK</em>

<em>m is mass of iron = 1000g</em>

<em>ΔT is change in temperature = Initial temperature - Final temperature.</em>

<em />

270000J = 0.385J/gK*1000g*(1000K-Final temperature)

701.3J/K = 1000K - Final T

<h3>Final T = 298.7K</h3>
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Answer:

1. C₄H₁₀ + ¹³/₂O₂ → 4CO₂ + 5H₂O

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1. The balanced chemical equation is:

C₄H₁₀ + ¹³/₂O₂ → 4CO₂ + 5H₂O

2. 0,360kg of butane are:

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6,19moles of butane×\frac{4CO_2}{1molButane}= <em>24,8 moles CO₂</em>

Using V=nRT/P

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n are moles (24,8 moles CO₂); R is gas constant (0,082atmL/molK); T is temperature, 20°C (293,15K); and P is pressure (1atm).

Volume (V) is:

<em>V = 596L</em>

I hope it helps!

8 0
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Hence, the correct answer is "D".

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