Answer:
0.78 atm
Explanation:
Step 1:
Data obtained from the question. This includes:
Mass of CO2 = 5.6g
Volume (V) = 4L
Temperature (T) =300K
Pressure (P) =?
Step 2:
Determination of the number of mole of CO2.
This is illustrated below:
Mass of CO2 = 5.6g
Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol
Number of mole CO2 =?
Number of mole = Mass/Molar Mass
Number of mole of CO2 = 5.6/44
Number of mole of CO2 = 0.127 mole
Step 3:
Determination of the pressure in the container.
The pressure in the container can be obtained by applying the ideal gas equation as follow:
PV = nRT
The gas constant (R) = 0.082atm.L/Kmol
The number of mole (n) = 0.127 mole
P x 4 = 0.127 x 0.082 x 300
Divide both side by 4
P = (0.127 x 0.082 x 300) /4
P = 0.78 atm
Therefore, the pressure in the container is
Answer:
look it up on gogole and if that doesnt work try asking teachers or take notes in class
Explanation:
Answer:
3200
Step-by-step explanation:
Let the number be x:
25 % of x = 800
⇒ 25/100 × x = 800
⇒ 1/4 × x = 800
⇒ x = 800 × 4
∴ x = 3200
Answer:
1
Explanation:
An unknown element, X, is a nonmetal that contains seven valence electrons. Element X most likely forms <u>1 </u>covalent bond.
Nonmetals gain the electron to complete the octet and form anion. Consider the example of halogen.
When it combine with another halogen atom they form covalent bond. There are seven valance electrons in outer most orbital of halogen atom. By combining with other halogen atom they form one covalent bond and complete the octet.
For example:
Cl atom combine with other Cl atom and form Cl₂.