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grigory [225]
3 years ago
12

A large pot (10 kg) of beef stew is left out on the kitchen counter to cool. The rate of cooling, in kJ/min, equals 1.955 (T-25)

, where T is the temperature of the stew in degrees Celsius. The heat capacity of the stew is 4 kJ/kg-C. If the stew initially is at 90 C, how long does it take to cool to 40 C? Round off your answer to the nearest minute.
Chemistry
1 answer:
olga_2 [115]3 years ago
5 0

Answer:

16 minutes

Explanation:

First, we need to calculate the amount of heat needed to cool the beef stew:

Q = mcΔT

Where <em>m</em> is the mass, <em>c</em> is the heat capacity and <em>ΔT</em> is the variation of the temperature.

Q = 10x4x(40 - 90)

Q = -2000 kJ

So, the beef stew needs to lost 2000 kJ to cool.

With the initial temperature at 90ºC, the rate of cooling(r) will be:

r = 1.955x(90 - 25)

r = 127.075 kJ/min

So, to lose 2000 kJ, will be necessary:

t = Q/r

t = 2000/127.075

t = 16 minutes

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A mixture of methane and carbon dioxide gases contains methane at a partial pressure of 431 mm Hg and carbon dioxide at a
KatRina [158]

Answer:

XCH₄ = 0.461

XCO₂ = 0.539

Explanation:

Step 1: Given data

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  • Partial pressure of carbon dioxide (pCO₂): 504 mmHg

Step 2: Calculate the total pressure in the container

We will sum both partial pressures.

P = pCH₄ + pCO₂

P = 431 mmHg + 504 mmHg = 935 mmHg

Step 3: Calculate the mole fraction of each gas

We will use the following expression.

Xi = pi / P

XCH₄ = pCH₄/P = 431 mmHg/935 mmHg = 0.461

XCO₂ = pCO₂/P = 504 mmHg/935 mmHg = 0.539

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Answer:

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A hydrocarbon is burnt completely to give 3.447g of
goblinko [34]

<u>Answer:</u> The empirical formula for the given compound is CH_2

<u>Explanation:</u>

The chemical equation for the combustion of compound having carbon, hydrogen, iron and oxygen follows:

C_xH_y+O_2\rightarrow CO_2+H_2O

where, 'x' and 'y'  are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of CO_2=3.447g

Mass of H_2O=1.647g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

<u>For calculating the mass of carbon:</u>

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 3.447 g of carbon dioxide, \frac{12}{44}\times 3.447=0.940g of carbon will be contained.

<u>For calculating the mass of hydrogen:</u>

In 18g of water, 2 g of hydrogen is contained.

So, in 1.647 g of water, \frac{2}{18}\times 1.647=0.183g of hydrogen will be contained.

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Moles of Carbon =\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{0.940g}{12g/mole}=0.0783moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.183g}{1g/mole}=0.183moles

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0783 moles.

For Carbon = \frac{0.0783}{0.0783}=1

For Hydrogen = \frac{0.183}{0.0783}=2.34\approx 2

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H = 1 : 2

Hence, the empirical formula for the given compound is CH_2

8 0
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4. When the following equation is balanced, what is the coefficient for HCI?
kozerog [31]

Hey there!

Mg + HCl → MgCl₂ + H₂

Balance Cl.

1 on the left, 2 on the right. Add a coefficient of 2 in front of HCl.

Mg + 2HCl → MgCl₂ + H₂

Balance H.

2 on the left, 2 on the right. Already balanced.

Balance Mg.

1 on the left, 1 on the right. Already balanced.

Our final balanced equation: Mg + 2HCl → MgCl₂ + H₂

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