Chemistry 20 Midterm review. Unit 1,2 and 3 PDF

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Review on chem 20 solutions, bonding and gas law practise. dosent have answers but youll figure it out....

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Chemistry*20*Midterm*Review* Unit*1:*Bonding* Fill$in$the$following$chart$ Formula$ Ionic$or$ Electron$Dot$ If$molecular$ If$ Molecular$ Diagram$and$ VSEPR$Shape$$ molecular,$ Dipoles$(if$ polar$or$ molecular)$ non@polar$ molecule$ CH3F$

molecular$

K3P$

ionic$

CH2O$

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CH3OH$

CaF2$

PF3$

NH3$

NF2@$

SO3$

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If$ molecular,$ what$IMF$ are$present$ in$the$ molecule?$ $

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$ $ 2.$$Which$has$a$higher$boiling$point?$ a)$NaCl$$or$H@Cl?$ $ b)$CH4$or$CH3OH$ $ c)$CF4$or$CH3F$ $ $ Unit*2:*Gas*Laws* $ 1. Temperature$is$a$measure$of$the$______________$______________$energy$of$the$molecules$in$a$sample.$ 2.

A$gas$exerts$pressure$on$its$container$because$the$molecules$___________$with$the$walls.$

3.

According$to$the$assumptions$of$KMT…$ •

The$molecules$of$an$ideal$gas$are$in$_____________$$motion.$

•

Most$of$the$volume$of$a$gas$is$_____________$space.$

•

Collisions$in$an$ideal$gas$are$completely$_____________.$

•

There$are$no$attractive$or$repulsive$__________$in$an$ideal$gas.$

The$assumptions$of$KMT$fail$under$high$_____________$or$low$____________.$ 5.$_______________$law$relates$pressure$and$volume$in$an$equation.$ 6.$_______________$law$relates$volume$and$temperature$in$an$equation.$ 7.$_______________$law$relates$volume$and$moles$in$an$equation.$ 8.$PV$=$nRT$is$referred$to$as$the$____________$gas$law.$ 9.$Standard$pressure$is$equal$to$_________$atm,$_________$kPa,$____________$mm$Hg,$or$____________$torr.$ 10.$Standard$temperature$is$equal$to$___________$0C$or$_________$K.$ 11.$A$gas$occupies$a$volume$of$28.4$mL$at$725$torr.$What$will$be$the$volume$of$this$gas$at$800$torr?$$$ $ $ $ $$12.$A$gas$occupies$a$volume$of$34.2$mL$at$a$temperature$of$15$˚C$and$a$pressure$of$800$mm$Hg.$ What$will$be$the$volume$of$this$gas$at$STP?$$ $ $ 13.$How$many$moles$of$chloroform,$CHCl3,$are$required$to$fill$a$100.$mL$flask$at$373K$and$a$pressure$ of$47.0$kPa?$$ $ $

14.$$A$sample$of$hydrogen$at$47$˚C$exerts$a$pressure$of$0.329atm.$The$gas$is$heated$to$77$˚C$at$ constant$volume.$What$will$its$new$pressure$be?$$ $ $ 15.$At$a$temperature$of$76.00$˚C,$a$gas$occupies$a$volume$of$4.588mL.$What$Kelvin$temperature$will$ the$gas$occupy$at$a$volume$of$21.24$mL?$$ 16.$$Ethane$gas$(C2H6)$burns$according$to$the$following$equation:$$$ 2$C2H6(g)$$+$5$O2(g)$@@>$4$CO2(g)$$+6$H2O$(g)$ What$volume$of$oxygen$is$required$to$react$with$250$mL$of$ethane$gas?$$ $ Unit*3:*Solutions* 1. Determine$the$concentration$of$a$solution$made$by$dissolving$4.25$g$of$barium$sulfide,$BaS(s),$in$ enough$water$to$make$225$mL$of$solution.$$(0.112%mol/L)$ $ 2. How$many$litres$of$a$0.200$mol/L$solution$of$copper$(II)$nitrate$solution,$Cu(NO3)2(aq),$may$be$ prepared$from$2.2$g$of$solute?$(0.059L)$ $ $ 3. Calculate$the$concentration$in$ppm$of$a$solution$made$by$dissolving$4.75$µg$of$sodium$fluoride$in$ 3.75$L$of$solution$(the$density$of$water$is$1$g/mL).$(1$µg$=$1$x$10@6$g)$(1.27%x1003%ppm)$ $ $ 4.

Determine$the$molar$concentration$of$iron(III)$ions$in$a$solution$prepared$by$dissolving$3.1$mg$ of$iron(III)$sulfate,$Fe2(SO4)3(s),$in$enough$water$to$make$750$mL$of$solution.$([Fe3+]%=%2.0%x1005%mol/L)$

% $ 5.

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What$mass$of$potassium$permanganate,$KMnO4(s),$would$have$to$be$dissolved$to$make$375$mL$ of$a$0.50$mol/L$solution?$(30%g)$

6. Determine$the$concentration$of$copper$in$percent$by$mass$if$1.25$g$of$copper$is$mixed$with$$$ 27.35$g$of$iron$to$make$an$alloy.$(4.37%)$ $ $ 7. What$is$the$concentration$in$ppm$if$2.5$x$10–5$g$of$chlorine$is$dissolved$in$a$bathtub$containing$ 135$L$of$water?$(1.9%x1004%ppm)$ $ $ 8. Determine$the$molar$concentration$of$a$solution$made$by$dissolving$0.0235$g$of$magnesium$ sulfate,$MgSO4(s),$in$enough$water$to$make$225$mL$of$solution.$(8.68%x1004%mol/L)$ $ $ $ 9. What$mass$of$aluminum$chloride,$AlCl3(s),$would$have$to$be$dissolved$to$make$225$mL$of$a$0.100$ mol/L$solution?$(3.00g)$ $ $ 10. What$mass$of$sodium$carbonate,$Na2CO3(s),$would$be$required$to$produce$100$mL$of$a$$0.250$ mol/L$solution?(2.65$g)$ $ $ 11. Determine$the$volume$of$a$0.47$mol/L$solution$that$could$be$made$using$1.35$kg$of$ammonium$ fluoride,$NH 4F(s).$(78%L)$ $ $ 12. What$is$the$concentration$of$the$sodium$ion$in$a$solution$of$sodium$sulfate$if$the$sulfate$ion$ concentration$is$0.450$mol/L?$$(0.900%mol/L)$ $ $

13. Determine$the$concentration$of$a$solution$made$by$diluting$25.0$mL$of$a$3.00$mol/L$solution$of$ sodium$hydroxide,$NaOH(aq),$to$a$volume$of$500.0$mL.$(0.15%mol/L)$ $ $ 14. What$volume$of$concentrated$18$mol/L$sulfuric$acid,$H2SO4(aq),$is$needed$to$prepare$250$mL$of$ a$6.0$mol/L$solution?$(83%mL)$ $ $ 15. To$what$volume$should$15.0$mL$of$a$5.0$mol/L$of$aqueous$potassium$chloride,$KCl(aq),$be$ diluted$in$order$to$prepare$a$0.25$mol/L$solution?$(300%mL)$ % % % 16.$$Write$an$equation$to$show$what$happens$to$the$following$solutes$when$they$are$placed$in$water.$ a)$NH4Cl$ b)$NH3$ c)$CaF2$ d)$AgCH3COO$ e)$CH3OH$ f)$O2$ g)$Na2SO4$ $ 17.$$What$two$processes$are$occurring$at$the$same$rate$in$a$saturated$solution$in$dynamic$ equilibrium.$ $ $ *...