Why do elements in the same group have similar properties

IgorLugansk [536]

Gold Ore is a mixture.

4 0

3 years ago

A silver block, initially at 58.4∘C, is submerged into 100.0 g of water at 25.0∘C in an insulated container. The final temperatu

Vlada [557]

Answer:

The mass of the silver block is 95.52 grams.

Explanation:

Heat lost by silver will be equal to heat gained by the water

$-Q_1=Q_2$

Mass of silver= $m_1$

Specific heat capacity of silver = $c_1=0.235 J/g^oC$

Initial temperature of the silver = $T_1=58.4^oC$

Final temperature of a silver = $T_2=T=26.7^oC$ =

$Q_1=m_1c_1\times (T-T_1)$

Mass of water= $m_1=100.0 g$

Specific heat capacity of water= $c_2=4.186 J/g^oC$

Initial temperature of the water = $T_3=25^oC$

Final temperature of water = $T_3=T=26.7^oC$

$Q_2=m_2c_2\times (T-T_3)$

$-Q_1=Q_2$

$-(m_1c_1\times (T-T_1))=m_2c_2\times (T-T_3)$

$-(m_1\times 0.235 J/g^oC\times (26.7^oC-58.4^oC))=100.0 g\times 4.186 J/g^oC\times (26.7^oC-25.0^oC)$

On substituting all values:

we get, $m_1 = 95.52 g$

The mass of the silver block is 95.52 grams.

3 0

4 years ago

What is the volume of 84 g of bromine gas (Br2) at STP?

Alla [95]

Answer : The correct option is, 11.77 L

Solution : Given,

Mass of bromine gas = 84 g

Molar mass of bromine gas = 159.8 g/mole

First we have to calculate the moles of bromine gas.

$\text{Moles of }Br_2=\frac{\text{ given mass of }Br_2}{\text{ molar mass of }Br_2}=\frac{84g}{159.8g/mole}=0.5256moles$

Now we have to calculate the volume of bromine gas at STP.

As we know that at STP,

1 mole of bromine gas contains 22.4 L volume of bromine gas

So, 0.5256 mole of bromine gas contains $22.4\times 0.5256=11.77L$ volume of bromine gas

Therefore, the volume of bromine gas at STP is, 11.77 L

3 0

4 years ago

Read 2 more answers

How many grams of chlorine gas are present in a 150. liter cylinder of chlorine held at a pressure of 1.00 atm and 0. °C? Group

OlgaM077 [116]

Answer:

474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P*V = n*R*T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

In this case:

P= 1.00 atm
V= 150 L
n= ?
R= 0.082 $\frac{atm*L}{mol*K}$
T= 0 C= 273 K

Replacing:

1.00 atm* 150 L= n*0.08206 $\frac{atm*L}{mol*K}$ *273 K

Solving:

$n=\frac{1.00 atm* 150 L}{0.08206 \frac{atm*L}{mol*K}*273 K}$

n= 6.69 moles

Being Cl= 35.45 g/mole, the molar mass of chlorine gas is:

Cl₂=2*35.45 g/mole= 70.9 g/mole

So if 1 mole has 70.9 grams, 6.69 moles of the gas, how much mass does it have?

$mass=\frac{6.69 moles*70.9 grams}{1 mole}$

mass= 474.321 grams ≅ 474 grams

<u><em>474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C</em></u>

4 0

3 years ago

You plan to use the water displacement method to

N76 [4]

Answer: A stopwatch

Explanation:

You don’t needed

4 0

3 years ago