Given:

Atmospheric Pressure $358\mathrm{.}1mmHg$

$TH2=$ Room temperature. $10\mathrm{.}05C$

$PH2=349\mathrm{.}35mmHg$

$VH2=4\mathrm{.}25ml$

Use the units that match Formulas for solving a and $b$

Formula for a and $b$ and can explain which $Ru$ use and why

Calculate moles of $H_2$ gas:

$n_{H_2}=\frac{P_{H_2}*V_{H_2}}{R*T_{H_2}}$

$R=62\mathrm{.}4\frac{L*mm{H}_g}{\text{m}\text{o}\text{l}*K},orR=0\mathrm{.}0821\frac{L*atm}{\text{m}\text{o}\text{l}*K}$

Calculate moles of the metal

$n_M=n_{H_2}\frac{1\text{m}\text{o}\text{l}\text{e}M}{1\text{m}\text{o}\text{l}\text{e}{H}_2}$

Molar Mass of the metal:

$MMof$ Metal $=\frac{\text{m}\text{a}\text{s}\text{s}of\text{m}\text{e}\text{t}\text{a}\text{l}}{\text{m}\text{o}\text{l}\text{e}\text{s}of\text{m}\text{e}\text{t}\text{a}\text{l}}$

a$.$ Find the mo$.$le$.$s of $H2$ gas and mo$.$les. of metal mg$.$

b$.$ Find The molar mass of $mg.$

Please also answer c because i$\text{'}$m not sure how to do it and let me know if any

information is missing

c$.$ If $Fe$ is use instead of mg me$.$tal. calculate vo$.$lum.e $H2$ gas. pro.duced from $0\mathrm{.}02755$

$g$ of $Fe$ metal. Given

$2F{e}_{(s)}+6HC{l}_{(aq)}2F{e}_{(aq)}^{3+}+3H_{2(g)}$