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d1i1m1o1n [39]
3 years ago
11

HELP!!!!!!!!!!! *What are some of the safety concerns for Barium sulfate & Barium Sulfide? Explain

Chemistry
1 answer:
Alex3 years ago
3 0

BaSO₄ is relatively harmless, but BaS is highly toxic.

BaSO₄ is quite insoluble (240 µg/100 mL). It is a <em>mild irritant</em> in cases of skin contact and inhalation. However, it is <em>safe enough</em> that health professionals ask patients to drink a suspension of BaSO₄. The Ba is opaque to X-rays, so it makes the stomach and intestines more visible to radiographers.

BaS is soluble (7.7 g/100 mL). It reacts slowly with water and more rapidly in the acid conditions of the stomach to <em>release H₂S</em>.

BaS + 2HCl ⟶ BaCl₂ + H₂S

An H₂S concentration of 60 mg/100 mL can be <em>fatal within 30 min</em>.

<em>Don’t eat barium sulfide!</em>

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Write the chemical equation for this reaction. Use the picture I provide!
Lesechka [4]

Answer:

H2O

H2O

Explanation:

because the are only two hydrogen that can react to Oxygen

3 0
2 years ago
How many grams of nan3 are required to produce 19.0 ft3 of nitrogen gas, about the size of an automotive air bag, if the gas has
Papessa [141]

The  balanced chemical reaction is given as:

2NaN_{3}(s)\rightarrow 2Na(s)+3N_{2}(g)

Now, convert 19.0 ft^{3} into litres.

1 ft^{3}  = 28.3168

So, 19.0 ft^{3} = 19\times 28.3168 = 538.0192 L

Density is equal to the ratio of mass to the volume.

D=\frac{M}{V}

where, M = mass and V= volume (538.0192 L)

Substitute the value of density and volume in formula to get the value of mass.

1.25 g/L=\frac{M}{538.0192 L}

1.25 g/L\times 538.0192 L= M

Mass = 672.524 g

Now, number of moles of N_{2} gas=\frac{672.524 g}{28.02 g/mol}

= 24.00 moles

According to the reaction, 2 moles of sodium azide gives 3 moles of nitrogen gas.

Now, in 24.00 moles of nitrogen gas produced from= \frac{2 moles of sodium azide}{3 moles of nitrogen gas}\times 24.00 moles of nitrogen gas, moles of sodium azide.

number of moles of sodium azide  = 16 moles

Mass of sodium azide in g  =  number of moles\times molar mass of sodium azide.

= 16 moles\times 65.00 g/mol

= 1040 g

Thus, mass of sodium azide which is required to produce 19.0 ft^{3} of nitrogen gas  = 1040 g





3 0
3 years ago
Which of the following would be expected to have the highest viscosity? CH3CH2OH, HOCH2OH, CH3CH2CH3
zaharov [31]

Answer: Out of the given options HOCH_{2}OH is expected to have the highest viscosity.

Explanation:

The resistance occurred in the flow of a liquid substance is called viscosity.

More stronger is the intermolecular forces present in a substance more will be its resistance in its flow. Hence, more will be its viscosity.

For example,  HOCH_{2}OH has strong intermolecular hydrogen bonding than the one's present in CH_{3}CH_{2}OH and CH_{3}CH_{2}CH_{3}. This is because two-OH groups are present over here.

Thus, we can conclude that out of the given options HOCH_{2}OH is expected to have the highest viscosity.

5 0
2 years ago
the Temperature of a sample of an ideal gas in a sealed 5.0 l container is raised from 27 oC to 77oC. If the initial pressure of
matrenka [14]
Answer:
              The pressure increases to 3.5 atm.

Solution:
                According to Gay-Lussac's Law, " At constant volume and mass the pressure of gas is directly proportional to the applied temperature".

For initial and final states of a gas the equation is,

                                           P₁ / T₁  =  P₂ / T₂
Solving for P₂,
                                           P₂  =  P₁ T₂ / T₁    ----- (1)

Data Given;
                   P₁  =  3 atm

                   T₁  =  27 °C + 273  =  300 K
 
                   T₂  =  77 °C + 273  =  350 K

Putting values in eq. 1,

                                           P₂  =  (3 atm × 350 K) ÷ 300 K

                                           P₂  =  3.5 atm
7 0
3 years ago
A container has a mixture of NO2 gas and N2O4 gas in equilibrium. The chemical reaction between the two gases is described by th
kondaur [170]

Answer: The most likely partial pressures are 98.7MPa for NO₂ and 101.3MPa for N₂O₄

Explanation: To determine the partial pressures of each gas after the increase of pressure, it can be used the equilibrium constant Kp.

For the reaction 2NO₂ ⇄ N₂O₄, the equilibrium constant is:

Kp = \frac{P(N_{2}O_{4} )}{P(NO_{2} ^{2}) }

where:

P(N₂O₄) and P(NO₂) are the partial pressure of each gas.

Calculating constant:

Kp = \frac{38.8}{61.2^{2} }

Kp = 0.0104

After the weights, the total pressure increase to 200 MPa. However, at equilibrium, the constant is the same.

P(N₂O₄) + P(NO₂) = 200

P(N₂O₄) = 200 - P(NO₂)

Kp = \frac{P(N_{2}O_{4} )}{P(NO_{2} ^{2}) }

0.0104 = \frac{200 - P(NO_{2})  }{[P(NO_{2} )]^{2}}

0.0104[P(NO_{2} )]^{2} + P(NO_{2} ) - 200 = 0

Resolving the second degree equation:

P(NO_{2} ) = \frac{-1+\sqrt{9.32} }{0.0208}

P(NO_{2} ) = 98.7

Find partial pressure of N₂O₄:

P(N₂O₄) = 200 - P(NO₂)

P(N₂O₄) = 200 - 98.7

P(N₂O₄) = 101.3

The partial pressures are P(NO_{2} ) = 98.7 MPa and P(N₂O₄) = 101.3 MPa

3 0
3 years ago
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