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patriot [66]
3 years ago
7

If an automobile air bag has a volume of 11.5 l , what mass of nan3 (in

Chemistry
2 answers:
True [87]3 years ago
8 0
Moles of NaN3 at STP  = volume of gas / 22.4 = 11.5/22.4 = 0.5mole. Massof NaN3 = moles of NaN3 x molecular weight = 0.5 x 65 = 32.5 grams.
anastassius [24]3 years ago
5 0

<u>Answer:</u> The mass of sodium nitride required is 35.4 grams.

<u>Explanation:</u>

We are given:

Volume of gas = 11.5 L

At STP:

22.4 L of volume is occupied by 1 mole of gas

So, 11.5 L of volume will be occupied by = \frac{1}{22.4}\times 11.5=0.513mol of sodium nitride

To calculate the mass for given number of moles, we use the equation:

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

Molar mass of sodium nitride = 69 g/mol

Moles of sodium nitride = 0.513 moles

Putting values in above equation, we get:

0.513mol=\frac{\text{Mass of sodium nitride}}{69g/mol}\\\\\text{Mass of sodium nitride}=(0.513mol\times 69g/mol)=35.4g

Hence, the mass of sodium nitride required is 35.4 grams.

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madam [21]

Answer:

Matter

Explanation:

All matter is made up of substances called elements

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3 years ago
Which branch of chemistry would study how pollution effects marine life?
mart [117]

Answer: (D) environmental chemistry

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8 0
3 years ago
An enclosed vessel contains 2.5g of 9b nitrogen and 13.3g of chlorine at s.T.P. Of What will be the partial pressure of the Il n
kow [346]

Answer:

0.535 atm

Explanation:

Since the volume of the tank is constant, we use Gay- Lussac's law to find the pressure at 180°C.

So, P₁/T₁ = P₂/T₂ where P₁ = pressure at S.T.P = 1 atm, T₁ = temperature at S.T.P = 273.15 K, P₂ = pressure of gas at 180 °C and T₂ = 180 °C = 273.15 + 180 K = 453.15 K

So, P₁/T₁ = P₂/T₂

P₂ = P₁T₂/T₁

Substituting the values of the variables into the equation, we have

P₂ = P₁T₂/T₁

P₂ = 1 atm × 453.15 K/273.15 K

P₂ = 1 atm × 1.66

P₂ = 1.66 atm

We now need to find the total number of moles of each gas present

number of moles of nitrogen = mass of nitrogen, m/molar mass of nitrogen molecule M

n = m/M

m = 2.5 g and M = 2 × atomic mass of nitrogen (since it is diatomic) = 2 × 14 g/mol = 28 g/mol

So, n = 2.5 g/28 g/mol

n = 0.089 mol

number of moles of chlorine, n' = mass of chlorine, m'/molar mass of chlorine molecule M'

n' = m'/M'

m' = 13.3 g and M = 2 × atomic mass of chlorine (since it is diatomic) = 2 × 35.5 g/mol = 71 g/mol

So, n' = 13.3 g/71 g/mol

n' = 0.187 mol

So, the total number of moles of gas present is n" = n + n' = 0.089 mol + 0.187 mol = 0.276 mol

So, the partial pressure due to nitrogen gas, P = mole fraction of nitrogen × pressure of gas at 180 °C

P = n/n" × P₂

P = 0.089 mol/0.276 mol × 1.66 atm

P = 0.322 × 1.66 atm

P = 0.535 atm

8 0
3 years ago
atch the following aqueous solutions with the appropriate letter from the column on the right. fill in the blank 1 A 1. 0.20 m N
Firdavs [7]

Answer:

Highest boiling point - 0.43 m Urea

Second highest boiling point - 0.20 m NiSO4

Third highest boiling point - 0.19 m NH4I

Lowest boiling point - 0.17 m NH4NO3

Explanation:

We know that;

ΔT = kb m i

Where;

ΔT = boiling point elevation

kb = boiling point constant

m = molality of the solution

i = Van't Hoff factor

For NiSO4 , NH4I  and NH4NO3 , the Van't Hoff factor, i = 2

But for Urea, the Van't Hoff factor, i = 1

We also have to consider both the values of the molality and Van't Hoff factor , knowing that a higher molality and a higher Van't Hoff factor leads to a higher ΔT and consequently a higher boiling point.

This facts above account for the arrangement of substances shown in the answer.

6 0
3 years ago
An unknown substance with a mass of 100 grams absorbs 1000 J while undergoing a temperature increase of 15 C. what is the specif
Alika [10]
B is the correct answer to the question
4 0
3 years ago
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