Answer:
Step-by-step explanation:
(The basics: / means fraction)
To solve this problem, you can use the ideal gas law:
PV = nRT
Where:
- P is the pressure (in atmospheres, atm)
- V is the volume (in liters, L)
- n is the number of moles of the gas (in moles, mol)
- R is the ideal gas constant (0.0821 L atm / mol K)
- T is the temperature (in kelvin, K)
1) First, calculate the initial conditions with 10.3 moles and 4.01 L:
P1 x V1 = n1 x R x T
2) Now, you can calculate the final volume (V2) for 77.0 moles at the same temperature and pressure:
P1 x V2 = n2 x R x T
3) Both equations share the same pressure (P) and temperature (T. Thus, you can write:
V1/n1 = v2/n2
4) Now plug in the values:
4.01 L/10.3 mol = V2/77.0 mol
5) Solve for V2:
V2 = 30.02L
So, 77.0 moles of CO will occupy 33.02 Liters at the same temperature and pressure.