How many moles of $MgC{l}_2$ are present in $150\mathrm{.}0mL$ of a $0\mathrm{.}250MMgCl$ solution?

a$.0\mathrm{.}250$mol

b$.0\mathrm{.}150$mol

c$.0\mathrm{.}0350$mol

d$.0\mathrm{.}0375$mol

What volume of $3\mathrm{.}50M{H}_{2}S{O}_4$ is needed to prepare $500\mathrm{.}0mL$ of a solution that is $0\mathrm{.}500M$ in $H_{2}S{O}_4?$

a$.50\mathrm{.}0mL$

b$.55\mathrm{.}9mL$

c$.71\mathrm{.}4mL$

d$.85\mathrm{.}4mL$

Calculate the change in total internal energy for a system that releases $3\mathrm{.}24{10}^{3}kJ$ of heat and does $1\mathrm{.}96{10}^{3}kJ$ of work on the surroundings. $U=q+w($U: internal energy; q: heat; w: work$)$

a$.1\mathrm{.}28{10}^{3}kJ$

b$.-1\mathrm{.}28{10}^{3}kJ$

c$.5\mathrm{.}20{10}^{3}kJ$

d$.-5\mathrm{.}20{10}^{3}kJ$

Given the thermochemical equation:

$H_2(g)+B{r}_2(l)=>2HBr(g),H=-72\mathrm{.}4k\frac{J}{m}ol,$ calculate the amount of heat released when a $320g$ of $B{r}_2(l)$ is consumed in this reaction.

a$.36\mathrm{.}2kJ$

b$.72\mathrm{.}4kJ$

c$.144\mathrm{.}8kJ$

d$.217\mathrm{.}2kJ$