Explanation:
the base in this equation is KOH (POTASSIUM HYDROXIDE)
BASES MOSTLY HAVE OH AS THEIR FORMULA
Given:
<span> 2.1 moles of chlorine gas (Cl2) at standard temperature and pressure (STP)
Required:
volume of CL2
Solution:
Use the ideal gas law
PV = nRT
V = nRT/P
V = (2.1 moles Cl2) (0.08203 L - atm / mol - K) (273K) / (1 atm)
V = 47 L</span>
Boron tribromide = bBr3
mol = mass/mr
mol=3/10.811+3(79.904)
= 0.018772527032439
Answer:
The new pressure is 1,67atm
Explanation:
In this case, having constant temperature we apply Boyle Mariotte's Law, where the volume varies inversely proportional to the pressure: P1 xV1 = P2xV2. We pass the pressure unit from Torr to atm: 760 Torr = 1atm
P1 xV1 = P2xV2 --> P2=P1 xV1/V2
P2= 1 atm x 5,00L/3, 00L=1, 67 atm