Fluorine is used to strengthen the enamel of your teeth, it can be used in acid form to etch glass, and chlorine is used in our drinking water and swimming pools. They're all part of the halogen family
Answer:
Cold coffee
Explanation:
The higher the temperature of something, the more kinetic energy it will have. The colder coffee's molecules will have less kinetic energy than the hot coffee's molecules
1. Given the following equation: N2 (g) + 3 H2 (g) ↔ 2NH3 (g) ΔH = -92 kJ/mol
a. this reaction is exothermic as ΔH is -ve
b. the equilibrium will shift 2 the left if nitrogen gas is removed
c. the equilibrium shift 2 the right if the temperature is lowered
d. the equilibrium shift 2 the left if ammonia (NH3) is added
e. principle of thermodynamic potential or Gibbs energy is used to answer B-D
Answer:
5.42g, 71.77%
Explanation:
First, we have to write out the balanced chemical equation. The unbalanced equation can be written as “SO2+O2 -> SO3” and to balance it, we can see that having two mols of SO2 and two mols of SO3 will make each side have the same amount of mols per element on each side. So the balanced chemical equation is “2SO2 + O2 -> 2SO3”
Now, we want to solve for the theoretical yield in grams of SO3. To do this, we have to use dimensional analysis. We convert g SO2 into mols SO2 using the molar mass of the elements. Then we convert mols of SO2 into mols of SO3 using the balanced equation. Once we’ve done that, we can convert mols of SO3 into grams of SO3.
You should know how to look up the molar mass of elements on the periodic table by now. Find the masses and set up the terms so they cancel like so:
Doing the math, we get 5.42g so3 as the theoretical yield. This is the most amount that you could ever get if the world was a perfect place. But alas, it isn’t and mistakes are gonna happen, so the number is going to be less than that. So the best we can do, is to figure out the percent yield that we got.
In a lab scenario, this was calculated to be 3.89 g as stated by the problem. The percent composition formula is
and plugging the numbers into it, we get:
make sure to follow the decimal/significant figure rules of your instructor, but only round at the end. My professor didn't care too much thankfully, but some professors do