You have four fixed-volume containers at STP.
Container A has 0.5 mol of gas in 11.2 L.
Container B has 2 mol of gas in 22.4 L.
Container C has 1 mol of gas in 22.4 L.
Container D has 2 mol of gas in 11.2 L.
Which containers have equal pressures?
Question 1 options:
B and C
A and C
A and B
C and D
To compare the pressures in the different containers, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (STP is 273 K)
Let's calculate the pressures for each container using this equation:
For Container A:
P_A = (n_A * R * T) / V_A
P_A = (0.5 mol * 0.0821 L·atm/(mol·K) * 273 K) / 11.2 L
P_A = 1.36 atm
For Container B:
P_B = (n_B * R * T) / V_B
P_B = (2 mol * 0.0821 L·atm/(mol·K) * 273 K) / 22.4 L
P_B = 2.05 atm
For Container C:
P_C = (n_C * R * T) / V_C
P_C = (1 mol * 0.0821 L·atm/(mol·K) * 273 K) / 22.4 L
P_C = 1.02 atm
For Container D:
P_D = (n_D * R * T) / V_D
P_D = (2 mol * 0.0821 L·atm/(mol·K) * 273 K) / 11.2 L
P_D = 3.63 atm
Therefore, the containers with equal pressures are B and C.