Which type of molecule is shown below?

The temperature of a 95.4 g piece of Cu increases from 25.0 °C to 48.0 °C when the Cu absorbs 849 J of heat. What is the specifc

melisa1 [442]

<h3>Answer:</h3>

0.387 J/g°C

<h3>Explanation:</h3>

To calculate the amount of heat absorbed or released by a substance we need to know its mass, change in temperature and its specific heat capacity.
Then to get quantity of heat absorbed or lost we multiply mass by specific heat capacity and change in temperature.
That is, Q = mcΔT

in our question we are given;

Mass of copper, m as 95.4 g

Initial temperature = 25 °C

Final temperature = 48 °C

Thus, change in temperature, ΔT = 23°C

Quantity of heat absorbed, Q as 849 J

We are required to calculate the specific heat capacity of copper

Rearranging the formula we get

c = Q ÷ mΔT

Therefore,

Specific heat capacity, c = 849 J ÷ (95.4 g × 23°C)

= 0.3869 J/g°C

= 0.387 J/g°C

Therefore, the specific heat capacity of copper is 0.387 J/g°C

3 0

3 years ago

Chloroform, formerly used as an anaesthetic and now believed to be a carcinogen, has a heat of vaporization ΔHvaporization = 31.

djverab [1.8K]

Answer:

Chloroform is expected to boil at 333 K (60 $^{0}\textrm{C}$ ).

Explanation:

For liquid-vapor equilibrium at 1 atm, $\Delta G^{0}$ = 0.

We know, $\Delta G^{0}=\Delta H^{0}-T\Delta S^{0}$ , where T is temperature in kelvin scale.

Here both $\Delta H^{0}$ and $\Delta S^{0}$ are corresponding to vaporization process therefore T represents boiling point of chloroform.

So, $0=(31.4\times 10^{3}\frac{J}{mol})-[T\times (94.2\frac{J}{mol.K})]$

or, T = 333 K

So, at 333 K (60 $^{0}\textrm{C}$ ) , chloroform is expected to boil.

6 0

3 years ago

Read 2 more answers

Cylinders of compressed gas are typically filled to a pressure of 200 bar. For oxygen, what would be the molar volume at this pr

mars1129 [50]

Answer:

a

$V = 0.124 \ Liters$

b

$V = 0.112 \ Liters$

Explanation:

From the question we are told that

The pressure of compressed gas is $P = 200 \ bar = \frac{200}{1.013}= 197.4 \ atm$

The temperature is $T = 25^oC = 25 + 273 = 298 \ K$

Generally the perfect gas equation is mathematically represented as

$PV = nRT$

substituting 0.08206 L-atm/mol-K for R and 1 mole for n

We have that

$V = \frac{1 * 0.08206 * 298 }{ 197.4}$

$V = 0.124 \ Liters$

Generally the van der Waals equation is mathematically represented as

$nRT = [P + \frac{n^2 * a }{V^2 } ][V - nb]$

=> $1 * 0.08206 *298 = [197.4 + \frac{1^2 * 1.364}{V^2 } ][V - 1 * 3.19 * 10^{-2}]$

=> $V = 0.112 \ Liters$

7 0

4 years ago

Which of the following is an example of a covalent bond?

loris [4]

Answer:

C. H2O

yep this one is right

4 0

3 years ago

Balance the following Equation:

pashok25 [27]

Answer:

HCl

Explanation:

Given data:

Mass of Zn = 50 g

Mass of HCl = 50 g

Limiting reactant = ?

Solution:

Chemical equation:

Zn + 2HCl → ZnCl₂ + H₂

Number of moles of Zn:

Number of moles = mass / molar mass

Number of moles = 50 g/ 65.38 g/mol

Number of moles = 0.76 mol

Number of moles of HCl:

Number of moles = mass / molar mass

Number of moles = 50 g/ 36.5 g/mol

Number of moles = 1.4 mol

Now we will compare the moles of Reactant with product.

Zn : ZnCl₂

1 : 1

0.76 : 0.76

Zn : H₂

1 : 1

0.76 : 0.76

HCl : ZnCl₂

2 : 1

1.4 : 1/2×1.4 = 0.7

HCl : H₂

2 : 1

1.4 : 1/2×1.4 = 0.7

Less number of moles of product are formed by HCl it will act limiting reactant.

6 0

3 years ago