Step-by-step explanation:
We have to determine the pressure inside a balloon that has a volume of 950 mL and contains 1.6 moles of He at 34 °C. To find the pressure we can use the ideal gas law formula.
P * V = n * R * T
P = n * R * T/V
Where P is the pressure, n is the number of moles, R is the ideal gas constant (R = 0.082 atm*L/mol*K), T is the temperature and V is the volume.
We already know the temperature in °C, the number of moles and the volume in mL. Before we find the answer to our problem we will have to convert the mL into L and the °C into K.
R = 0.082 atm*L/(mol*K)
n = 1.6 moles
T = (34 + 273.15) K
T = 307.15 K
V = 950 mL * 1 L/(1000 mL)
V = 0.950 L
Finally we can replace those values in the formula and get the answer to the problem.
P = n * R * T/V
P = 1.6 moles * 0.082 atm*L/(mol*K) * 307.15 K/(0.950 L)
P = 42.4 atm
Answer: the pressure is 42.4 atm.