Question

7) a 1.50L glass vessel contains 0.112 mole of Cl2(g) and 0.117 mile of HI(g) at 210°C.

A) starting with the ideal gas law, PV=nRT, solve for P/RT. What are the units for P/RT when simplified?

B) calculate the molarities of the gases and convert those values into pressure using the ideal gas law.

C) assume moles, temperature, and pressure stated above, if the following reaction goes to completion, what is the total pressure in the container? Assume constant temperature and volume.

A 1.50 L glass vessel contains 0.112 mol of Cl2 (g) and 0.117 mol of HI (g) at 110 °c. a Starting with the ideal gas law, PV nRT (pg 208), solve for P/RT. What are the units for P/RT (when simplified)? Calculate the molarities of the gases and convert those values into pressure using the ideal gas law. E(wait for lab lecture before trying this) Assuming moles, temperature, and pressure stated above, if the following reaction goes to completion, what is the total pressure in the container? Assume constant temperature and volume (pg 221-223). Cl2 (g) 2 HI (g)- I2 (s) 2 HCI (g)

Answer 1

$(hiven: Volume Glass vessel - . s utre CI, - o.li2 mole H -o-117 mole מ 0.229- mole RT\V útre Unit <^ P - mole/ itse RT 0.078 mole/ PV ank) V RT$