Which of the following is a mixture? a. Orange soda, b. Alcohol, c. Mercury, d. Water

A mixture of He, Ne, and N2 gases are a pressure of 1.348. If the pressures of He and Ne are 0.124 atm, what is the partial pres

Aleks04 [339]

The Best Answer: 1 - (.47+.23) = 0.30

If Ne has a mole fraction of 0.47 (or 47/100) and Ar is 0.23, then H2(or He) has a mole fraction of 0.30

This means the gas mixture is 30/100 H2(or He).

7.85 x 0.30 = 2.355 atm

5 0

2 years ago

Read 2 more answers

2NaHCO3-->Na2CO3+H2O+CO2

algol [13]

I’m not sure what kind of answer you’re looking for, but if you’re supposed to translate it into a sentence it would be two moles of sodium bicarbonate(baking soda) decompose unto one mole of sodium carbonate(soda ash) plus one mole of water and one mole of carbon monoxide gas

8 0

2 years ago

Be sure to answer all parts. Dimercaprol (HSCH2CHSHCH2OH) was developed during World War I as an antidote to arsenic-based poiso

Sauron [17]

Answer:

For A: The number of arsenic atoms are $3.4\times 10^{21}$

For B: The percent composition of mercury, thallium and chromium in their complexes are 61.76 %, 62.2 % and 29.51 % respectively.

Explanation:

For A:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of dimercaprol = 696 mg = 0.696 g (Conversion factor: 1 g = 1000 mg)

Molar mass of dimercaprol = 124.21 g/mol

Putting values in above equation, we get:

$\text{Moles of dimercaprol}=\frac{0.696g}{124.21g/mol}=0.0056mol$

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of molecules.

So, 0.0056 moles of dimercaprol will contain $0.0056\times 6.022\times 10^{23}=3.4\times 10^{21}$ number of molecules.

As, 1 molecule of dimercaprol binds with 1 atom of Arsenic

So, $3.4\times 10^{21}$ number of dimercaprol molecules will bind with = $1\times 3.4\times 10^{21}=3.4\times 10^{21}$ number of arsenic atoms

Hence, the number of arsenic atoms are $3.4\times 10^{21}$

For B:

We know that:

Molar mass of dimercaprol = 124.21 g/mol

Molar mass of mercury = 200.59 g/mol

Molar mass of thallium = 204.38 g/mol

Molar mass of chromium = 51.99 g/mol

Also, 1 molecule of dimercaprol binds with 1 metal atom.

To calculate the percentage composition of metal in a complex, we use the equation:

$\%\text{ composition of metal}=\frac{\text{Mass of metal}}{\text{Mass of complex}}\times 100$ ......(1)

For mercury:

Mass of Hg-complex = (200.59 + 124.21) = 324.8 g

Mass of mercury = 200.59 g

Putting values in equation 1, we get:

$\%\text{ composition of mercury}=\frac{200.59g}{324.8g}\times 100=61.76\%$

For thallium:

Mass of Tl-complex = (204.38 + 124.21) = 328.59 g

Mass of thallium = 204.38 g

Putting values in equation 1, we get:

$\%\text{ composition of thallium}=\frac{204.38g}{328.59g}\times 100=62.2\%$

For chromium:

Mass of Cr-complex = (51.99 + 124.21) = 176.2 g

Mass of chromium = 51.99 g

Putting values in equation 1, we get:

$\%\text{ composition of chromium}=\frac{51.99g}{176.2g}\times 100=29.51\%$

Hence, the percent composition of mercury, thallium and chromium in their complexes are 61.76 %, 62.2 % and 29.51 % respectively.

8 0

3 years ago

How much heat is required to raise the temperature of 250.0g of mercury 52.0°c if the specific heat of mercury is 0.140 j/(g x °

sasho [114]

Q = m c T

c= 0.140 j/(g x °c)

m= 250.0g

T =52

hope you can solve it now

8 0

2 years ago

what is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g

LekaFEV [45]

Answer:

K8S4O16 or K8(SO4)4 depending on if the SO4 is supposed to represent sulfate or not

Explanation:

Find the molar mass of K2SO4 first:

2K + S + 4O ≈ 174 g/mol

Divide the goal molar mass of 696 by the molar mass of the empirical formula:

696 / 174 = 4

This means you need to multiply everything in the empirical formula by 4:

K2SO4 --> K8S4O16 or K8(SO4)4 depending on if the SO4 is for sulfate or not

4 0

2 years ago