74.62 g of magnesium oxide is formed from 45.00 g magnesium so 74.62-45.00= 29.62 g of oxygen is consumed or in other words a new compound is formed in the burning of magnesium in oxygen with a heavier mass than the pure magnesium.
There are 158.4 grams of CO2 in 3.6 mol of CO2.
<h3>HOW TO CALCULATE MASS?</h3>
The mass of a substance can be calculated by multiplying the number of moles of the substance by its molar mass. That is;
mass of CO2 = no. of moles × molar mass
According to this question, there are 3.6 moles of CO2.
mass of CO2 = 3.6 moles × 44g/mol
mass of CO2 = 158.4g.
Therefore, there are 158.4 grams of CO2 in 3.6 mol of CO2
Learn more about mass at: brainly.com/question/15959704
Answer: 1.87 atm
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
![\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}](https://tex.z-dn.net/?f=%5Cfrac%7BP_1V_1%7D%7BT_1%7D%3D%5Cfrac%7BP_2V_2%7D%7BT_2%7D)
where,
= initial pressure of gas = 2.50 atm
= final pressure of gas = ?
= initial volume of gas = 26.4 ml
= final volume of gas = 36.2 ml
= initial temperature of gas = ![2.5^oC=273+2.5=275.5K](https://tex.z-dn.net/?f=2.5%5EoC%3D273%2B2.5%3D275.5K)
= final temperature of gas = ![10^oC=273+10=283K](https://tex.z-dn.net/?f=10%5EoC%3D273%2B10%3D283K)
Now put all the given values in the above equation, we get:
![\frac{2.50\times 26.4}{275.5}=\frac{P_2\times 36.2}{283}](https://tex.z-dn.net/?f=%5Cfrac%7B2.50%5Ctimes%2026.4%7D%7B275.5%7D%3D%5Cfrac%7BP_2%5Ctimes%2036.2%7D%7B283%7D)
![P_2=1.87atm](https://tex.z-dn.net/?f=P_2%3D1.87atm)
The new pressure is 1.87 atm by using combined gas law.