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2 years ago

PLEASE HELP!!!

Chemistry

1 answer:

Elena L [17]2 years ago

3 0

Answer:

no it should not that place is historical and so they should make where u can visit but protect it as a historical landmark

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Help me, it’s pretty easy science moon stuff !

trasher [3.6K]

Hello :)
Based on the information I received reading the picture, the answer should be “B”

Explanation: if I am wrong I’m very sorry. But that should be the answer

8 0

2 years ago

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mixture of N 2 And H2 Gases weighs 13.22 g and occupies a volume of 24.62 L at 300 K and 1.00 atm.Calculate the mass percent of

anygoal [31]

Answer: The mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

Explanation:

To calculate the number of moles, we use the equation given by ideal gas equation:

PV = nRT

where,

P = Pressure of the gaseous mixture = 1.00 atm

V = Volume of the gaseous mixture = 24.62 L

n = number of moles of the gaseous mixture = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = Temperature of the gaseous mixture = 300 K

Putting values in above equation, we get:

$1.00atm\times 24.62L=n_{mix}\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 300K\\\\n_{mix}=\frac{1.00\times 24.62}{0.0821\times 300}=0.9996mol$

We are given:

Total mass of the mixture = 13.22 grams

Let the mass of nitrogen gas be 'x' grams and that of hydrogen gas be '(13.22 - x)' grams

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

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

For nitrogen gas:

Molar mass of nitrogen gas = 28 g/mol

$\text{Moles of nitrogen gas}=\frac{x}{28}mol$

For hydrogen gas:

Molar mass of hydrogen gas = 2 g/mol

$\text{Moles of hydrogen gas}=\frac{(13.22-x)}{2}mol$

Equating the moles of the individual gases to the moles of mixture:

$0.9996=\frac{x}{28}+\frac{(13.22-x)}{2}\\\\x=12.084g$

To calculate the mass percentage of substance in mixture we use the equation:

$\text{Mass percent of substance}=\frac{\text{Mass of substance}}{\text{Mass of mixture}}\times 100$

Mass of the mixture = 13.22 g

For nitrogen gas:

Mass of nitrogen gas = x = 12.084 g

Putting values in above equation, we get:

$\text{Mass percent of nitrogen gas}=\frac{12.084g}{13.22g}\times 100=91.41\%$

For hydrogen gas:

Mass of hydrogen gas = (13.22 - x) = (13.22 - 12.084) g = 1.136 g

Putting values in above equation, we get:

$\text{Mass percent of hydrogen gas}=\frac{1.136g}{13.22g}\times 100=8.59\%$

Hence, the mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

5 0

2 years ago

Q Q 3. (08.02 MC)

AnnyKZ [126]

Answer: A volume of 455 mL from 0.550 M KBr solution can be made from 100.0 mL of 2.50 M KBr.

Explanation:

Given: $V_{1}$ = ?, $M_{1}$ = 0.55 M

$V_{2}$ = 100.0 mL, $M_{2}$ = 2.50 M

Formula used to calculate the volume of KBr is as follows.

$M_{1}V_{1} = M_{2}V_{2}$

Substitute the values into above formula as follows.

$M_{1}V_{1} = M_{2}V_{2}\\0.55 M \times V_{1} = 2.50 M \times 100.0 mL\\V_{1} = 455 mL$

Thus, we can conclude that a volume of 455 mL from 0.550 M KBr solution can be made from 100.0 mL of 2.50 M KBr.

7 0

2 years ago

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The energy of motion is called

timama [110]

Answer:I think it’s mechanical energy

Explanation:

3 0

3 years ago

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when 5.60g of an iron oxide is heated with carbon, 3.92g of iron is produced. calculate the empirical formula of the iron oxide

svetlana [45]

Answer: Fe2O3

Explanation:

5.60 g Iron Oxide

- 3.92 g Iron

===========

= 1.68 g Oxygen

Convert Fe and O to moles:

3.92 g Iron/55.85 = 0.0702 moles Fe

1.68 g Oxygen/16 = 0.105 moles O

The ratio of O to Fe is 1.50. There are 3/2 O for each Fe. Multiply by 2 to get whole numbers: 2Fe for every 3O: Fe2O3

5 0

2 years ago