(Solved): The stopcock connecting a 1.00L bulb containing carbon dioxide gas at a pressure of 570. mmHg, ...

The stopcock connecting a $1.00\mathrm{L}$ bulb containing carbon dioxide gas at a pressure of 570. $\mathrm{mm}\mathrm{Hg}$, and a $1.00\mathrm{L}$ bulb containing hydrogen gas at a pressure of $590.\mathrm{mm}\mathrm{Hg}$, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, what is the final pressure in the system? $\mathrm{mm}\mathrm{Hg}$ 9 more group attempts remaining Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: $\begin{array}{l}\mathrm{Zn}(\mathrm{s})+2\mathrm{HCl}(\mathrm{aq})?{\mathrm{ZnCl}}_2(\mathrm{aq})+\\ {\mathrm{H}}_2(\mathrm{g})\end{array}$ In an experiment, the ${\mathbf{H}}_2$ gas formed is collected over water in a flask where the total pressure is $749\mathrm{mm}\mathrm{Hg}$ and the temperature is $17.0^{?}\mathrm{C}$, at which temperature the vapor pressure of water is $15\mathrm{mm}\mathrm{Hg}$. (1) What is the partial pressure of ${\mathbf{H}}_2$ in the flask? $\mathrm{mm}\mathrm{Hg}$. (2) If the wet ${\mathbf{H}}_2$ gas occupies a volume of $9.77$ $\mathrm{L}$, how many moles of ${\mathbf{H}}_2$ are formed? $\mathrm{mol}$ 9 more group attempts remaining A mixture of methane and argon gases is maintained in a $6.67\mathrm{L}$ flask at a temperature of $79^{?}\mathrm{C}$. If the partial pressure of methane is $0.419\mathrm{atm}$ and the partial pressure of argon is $0.362\mathrm{atm}$, what is the total pressure in the flask? atm 9 more group attempts remaining