Answer:
So there is83.6g CO2 produced
Explanation:
Burning carbon with air has the following equation
C + O2 → CO2
For 1 mol Carbon, we have 1 mol O2 and 1 mol CO2
Step 2: Calculating moles
mole C = 22.8g / 12g/mole
Mole C = 1.9 mole
1.9 mole C will completely react
Since for each mole C there is 1 mole O2 and 1 mole CO2
This means there will also react 1.9 mole of 02, to be formed 1.9 mole of CO2
mole CO2 = mass CO2 / Molar mass CO2
mass CO2 = 1.9 mole CO2 * 44g/mole =<u>83.6g CO2</u>
In this reaction 18.2 g of O2 remained unreacted
we can control this: 79g - 18.2 g = 60.8g
1.9 mole * 32g/mol = 60.8g
So there is83.6g CO2 produced
I think the answer is <span>supersaturated</span>
1.) when components are needed to be used in different ways
2.) sublimation, filtration, evaporation, and distillation
Answer:
43.13Kg of melamine
Explanation:
The problem gives you the mass of urea and two balanced equations:
First we need to calculate the number of moles of urea that are used in the reaction, so:
molar mass of urea =
The problem says that you have 161.2Kg of urea, so you take that mass of urea and find the moles of urea:
161.2Kg of urea2684 moles of urea
Now from the stoichiometry you have:
2684 moles of urea = 447 moles of melamine
The molar mass of the melamine is so we have:
= 5637.64 g of melamine
Converting that mass of melamine to Kg:
5637.64 g of melamine * = 56.38 Kg of melamine, that is the theoretical yield of melamine.
Finally we need to calculate the mass of melamine with a yield of 76.5%, so we have:
%yield = 100*(Actual yield of melamine / Theoretical yield of melamine)
Actual yield of melamine = = 43.13Kg of melamine
Answer: sorry for a late answer but it would be JJ Thompson
Explanation: