Question

ws: ideal gas and more
answer the following showing your work and proper units! box in your answer.

1. calculate the volume that a 0.323 mol sample of i₂ gas will occupy at 265 k and a pressure of 0.90 atm.
2. a 0.355 l balloon of co₂ is at a temperature of 18.0°c. it is heated to 30.0°c. what is the new volume?
3. a mixture of o₂, co₂ and n₂ has a total pressure of 0.97 atm. what is the partial pressure of o₂ if the partial pressure of co₂ is 0.70 atm and the partial pressure of n₂ is 0.12 atm?
4. what is the temperature in celsius required for 0.047 moles of kr to fill a balloon to 1.20 l at a pressure of 0.988 atm?
5. a flask is used to collect four gases at a total pressure of 6.870 atm. if p_h₂ = 0.234 atm, p_rn = 0.456 atm, p_ne = 1.330 atm, what is the partial pressure of the remaining gas xe?

Explanation:

Step1: Apply ideal gas law

$V = \frac{nRT}{P}$

Step2: Substitute values

$V = \frac{0.323\ \text{mol} \times 0.0821\ \text{L·atm/(mol·K)} \times 265\ \text{K}}{0.90\ \text{atm}} \approx 7.69\ \text{L}$

Step1: Convert temp to Kelvin

$T_1=18.0+273.15=291.15\ \text{K}, T_2=30.0+273.15=303.15\ \text{K}$

Step2: Apply Charles's law

$V_2 = V_1\frac{T_2}{T_1} = 0.355\ \text{L} \times \frac{303.15}{291.15} \approx 0.369\ \text{L}$

Step1: Use Dalton's law

$P_{O_2} = P_{\text{total}} - P_{CO_2} - P_{N_2}$

Step2: Calculate partial pressure

$P_{O_2} = 0.97\ \text{atm} - 0.70\ \text{atm} - 0.12\ \text{atm} = 0.15\ \text{atm}$

Step1: Solve for T (Kelvin)

$T = \frac{PV}{nR} = \frac{0.988\ \text{atm} \times 1.20\ \text{L}}{0.047\ \text{mol} \times 0.0821\ \text{L·atm/(mol·K)}} \approx 307.3\ \text{K}$

Step2: Convert to Celsius

$T(^\circ\text{C}) = 307.3 - 273.15 \approx 34.1^\circ\text{C}$

Answer:

7.69 L