Answer: 8.45 L
Explanation:
Given that,
Initial volume (V1) = 3.5L
Initial pressure (P1) = 2.5 atm
[Since final pressure is given in torr, convert 2.5 atm to torr
If 1 atm = 760 torr
2.5 atm = 2.5 x 760 = 1900 torr
Final volume (V2) = ?
Final pressure (P2) = 787 torr
Since pressure and volume are given while temperature remains the same, apply the formula for Boyle's law
P1V1 = P2V2
3.5L x 1900 torr = 787 torr x V2
6650L•torr = 787 torr•V2
Divide both sides by 787 torr
6650L•torr/787 torr = 787 torr•V2/787 torr
8.45 L = V2
Thus, the volume of the gas at 787 torr and at the same temperature is 8.45 Liters
Answer:
Burning is a chemical process by which two atoms or molecules will combine with each other. In burning, the two atoms or molecules will combine and release energy.When the molecules combine and release energy, it is released in the form of heat and often light.Different compounds react with oxygen differently – some contain lots of heat energy while others produce a smaller amount.The bigger the fuel load, the more intense the fire will be in terms of heat energy output. Moisture content: If the fuel isn't dry enough, it won't burn.Flames consist primarily of carbon dioxide, water vapor, oxygen and nitrogen. If hot enough, the gases may become ionized to produce plasma. Depending on the substances alight, and any impurities outside, the color of the flame and the fire's intensity will be different.
<u>Answer:</u> The empirical formula for the given compound is 
<u>Explanation:</u>
We are given:
Percentage of H = 5.80 %
Percentage of O = 23.02 %
Percentage of N = 20.16 %
Percentage of Cl = 51.02 %
Let the mass of compound be 100 g. So, percentages given are taken as mass.
Mass of H = 5.80 g
Mass of O = 23.02 g
Mass of N = 20.16 g
Mass of Cl = 51.02 g
To formulate the empirical formula, we need to follow some steps:
- <u>Step 1:</u> Converting the given masses into moles.
Moles of Hydrogen = 
Moles of Oxygen = 
Moles of Nitrogen = 
Moles of Chlorine = 
- <u>Step 2:</u> Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 1.44 moles.
For Hydrogen = 
For Oxygen = 
For Nitrogen =
For Chlorine =
- <u>Step 3:</u> Taking the mole ratio as their subscripts.
The ratio of H : O : N : Cl = 4 : 1 : 1 : 1
Hence, the empirical formula for the given compound is
Answer:
stochiometry works with measuring quantitative relationships and used to determine the amount of products and reactants that are produced or needed in a reaction
