Answer:
I attached a photo of balanced equations but thats as much as I can help.
Explanation:
We use Charles's Law: V1/T1=V2/T2
Standard Temperature: 0 degree Celsius= 273K
333.0 degrees Celsius= 606K
Set up: (1.00L)/ (273K)= V2/ (606.0K)
⇒ V2= (1.00L)/ (273K)* (606.0K)= 2.22L
Hope this would help :))
Answer:
157.64 L
Explanation:
We'll begin by converting 30 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
T(°C) = 30 °C
T(K) = 30 °C + 273
T (K) = 303 K
Next, we shall convert 600 mmHg to atm. This can be obtained as follow:
760 mmHg = 1 atm
Therefore,
600 mmHg = 600 mmHg × 1 atm / 760 mmHg
600 mmHg = 0.789 atm
Finally, we shall determine the volume of the gas. This can be obtained as follow:
Number of mole (n) = 5 moles
Temperature (T) = 303 K
Pressure (P) = 0.789 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Volume (V) =?
PV = nRT
0.789 × V = 5 × 0.0821 × 303
0.789 × V = 124.3815
Divide both side by 0.789
V = 124.3815 / 0.789
V = 157.64 L
Therefore, the volume of the gas is 157.64 L
Answer:
Here is my answer I got it correct
Explanation:
