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s344n2d4d5 [400]
3 years ago
15

A chemical that causes a sudden almost instantaneous release of pressure has and heat when subjected to sudden shock pressure or

high temperatures best describes which type of DOT hazardous materials classification
Chemistry
1 answer:
KIM [24]3 years ago
3 0

A hazardous chemical instantly discharging gas, pressure, and heat when subjected to pressure, heat, or high temperature is categorized under hazard class I explosives by the Department of Transportation.  

These are the explosives that possess the tendency to briskly detonate or conflagrate as an outcome of the chemical reaction. The explosives possess the tendency of generating pressures, temperatures, and speeds as leading to catastrophic destruction via force and/or of generating otherwise hazardous concentrations of light, heat, gas, sound, or smoke, all this resulting due to chemical reactions.  


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what is the correct conversion factor by to which to multiply to convert moles of hyrdogen peroxide (H2O2) to moles of oxygen (O
raketka [301]

Answer:

I looked it up I think I got it but idk

5 0
3 years ago
Which of the following contains a nonpolar covalent bond?
svet-max [94.6K]
I think the answer is C. 02
3 0
3 years ago
I need help with this ASAP PLEASE
Artemon [7]

439.3 g CO2

Explanation:

First find the # of moles of CO2 that results from the combustion of 3.327 mol C3H6:

3.227 mol C3H6 × (6 mol CO2/2 mol C3H6)

= 9.981 mol CO2

Use the molar mass of CO2 to determine the # of grams of CO2:

9.981 mol CO2 x (44.01 g CO2/1 mol CO2)

= 439.3 g CO2

5 0
3 years ago
A student isolated 25 g of a compound following a procedure that would theoratically yield 81 g. Wht was his percentt yield?
Sati [7]

<u>Answer:</u> The percent yield of the compound is 30.86 %.

<u>Explanation:</u>

To calculate the percentage yield of a compound, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of compound = 25 g

Theoretical yield of compound = 81 g

Putting values in above equation, we get:

\%\text{ yield of compound}=\frac{25g}{81g}\times 100\\\\\% \text{yield of compound}=30.86\%

Hence, the percent yield of the compound is 30.86 %.

3 0
4 years ago
___1___Zn + __2___HCl → ___1___H2 + ____1__ZnCl2
strojnjashka [21]

Answer:

Mass = 2.8 g

Explanation:

Given data:

Mass of HCl = 102 g

Mass of Zn = 128 g

Mass of H₂ = ?

Solution:

Chemical equation:

2HCl + Zn      →     H₂ + ZnCl₂

Number of moles of Zn:

Number of moles = mass/molar mass

Number of moles = 128 g/ 65.38 g/mol

Number of moles = 2 mol

Number of moles of HCl:

Number of moles = mass/molar mass

Number of moles = 102 g/ 36.5 g/mol

Number of moles = 2.8  mol

Now we will compare the moles of hydrogen gas with HCl and Zn.

                   HCl          :        H₂

                     2            :        1

                     2.8         :       1/2×2.8 = 1.4 mol

                   Zn          :        H₂

                     1            :        1

                     2           :         2

Number of moles of hydrogen formed by HCl are less thus it will limiting reactant.

Mass of Hydrogen:

Mass = number of moles × molar mass

Mass = 1.4 mol ×  2 g/mol

Mass = 2.8 g

7 0
3 years ago
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