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2 years ago

The empirical mass is a whole number multiple of the molar mass true or false?

Chemistry

1 answer:

elena-14-01-66 [18.8K]2 years ago

6 0

Answer:

True

Explanation:

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I really need help with this. Be serious. If you answer something random just for the points I will report you to brainly.

sashaice [31]

Answer:

It get thicker beacause the mid ocean

Explanation:

Because when it gets moved back the heat rises and it builds up to be thicker.

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2 years ago

A 13.5g sample of gold is heated, then placed in a calorimeter containing 60g of water. The temperature of water increases from

sweet-ann [11.9K]

Answer:

$T_i~=163.1$ ºC

Explanation:

We have to start with the variables of the problem:

Mass of water = 60 g

Mass of gold = 13.5 g

Initial temperature of water= 19 ºC

Final temperature of water= 20 ºC

Initial temperature of gold= Unknow

Final temperature of gold= 20 ºC

Specific heat of gold = 0.13J/gºC

Specific heat of water = 4.186 J/g°C

Now if we remember the heat equation:

$Q_H_2_O=m_H_2_O*Cp_H_2_O*deltaT$

$Q_A_u=m_A_u*Cp_A_u*deltaT$

We can relate these equations if we take into account that all heat of gold is transfer to the water, so:

$m_H_2_O*Cp_H_2_O*deltaT=~-~m_A_u*Cp_A_u*deltaT$

Now we can put the values into the equation:

$60~g*4.186~J/g{\circ}C*(20-19)~{\circ}C=-(13.5~g*0.13~J/g{\circ}C*(20-T_i)~{\circ}C)$

Now we can solve for the initial temperature of gold, so:

$T_i~=(\frac{60~g*4.186~J/g{\circ}C*(20-19)~{\circ}C}{13.5~g*0.13~J/g{\circ}C})+20$

$T_i~=163.1$ ºC

I hope it helps!

5 0

2 years ago

What does lithium 6 and lithium 7 look like

Marysya12 [62]

Lithium 6 would have 6 valence electrons in the outer orbital, while lithium 7 would have 7 in the outer orbital.

3 0

3 years ago

V=5, M=10 What is the density?

ch4aika [34]

Answer:

the answer to this question is 2 kilogram/cubic meter

Explanation:

4 0

3 years ago

If 7.25g of chlorine is reacted with excess hydrogen and produces 7.25 g HCl. What is the percent yield?

lozanna [386]

Answer:

94.61 %

Explanation:

percent yield = (actual yield / theoretical yield) X 100%

The balanced equation for the reaction is:

H2 (g ) + Cl2(g) => 2 HCl (l)

So, the theoretical yield =

7.25g of chlorine X (2mol of Cl / 35.453 g of Cl) X (2mol Cl / 2mol of HCl) X 37.469g of Hcl / 2mol of Hcl = 0.409 x 18.735 = 7.663g of Hcl

Using this theoretical yield and the provided value for actual yield, the percent yield = (actual yield / theoretical yield) X 100%

= (7.25 g / 7.663g) X 100

= 94.61 %

3 0

2 years ago

The empirical mass is a whole number multiple of the molar mass true or false?​

The empirical mass is a whole number multiple of the molar mass true or false?