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Could you please answer these questions

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For a particular reaction, DeltaH = -111.4 kJ and DeltaS = -25.0 J/K. Calculate DeltaG for this reaction at 298 K Classify the following phase changes by the signs of the system's DeltaH and DeltaS. Consider these reactions, where M represents a generic metal. Use the information above to determine the enthalpy of the following reaction. Consider these reactions, where M represents a generic metal. 2M(s) + 6HCl(aq) rightarrow 2MCl3(aq) + 3H2(s) Delta H1, = -650.0 kJ HCl(g) rightarrow HCI(aq) Delta H2 = -74.8 kJ H2(g)+Cl2(g) rightarrow 2HC1(g) Delta H3 = -1845.0kJ MCI3(S) rightarrow MCI3(aq) Delta H4 = -416.0kJ Use the information above to determine the enthalpy of the following reaction 2M(S) + 3CI2(g) rightarrow 2MCI3(S) Delta H = A researcher studying the nutritional value of a new candy places a 4.20-gram sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.17 degree C. If the heat capacity of the calorimeter is 34.00 kJ K-1, how many nutritional Calories are there per gram of the candy? When 1.250 x 103 J of heat energy is added to 43.5 g of hexane, C6H14, the temperature increases by 12.7 degree C. Calculate the molar heat capacity of C6H14. If you have 420.0 mL of water at 25.00 degree C and add 130.0 mL of water at 95.00 degree C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water. A 54.21 g sample of a substance is initially at 24.2 degree C. After absorbing 2755 J of heat, the temperature of the substance is 108.6 degreeC. What is the specific heat (c) of the substance? If a system has 325 kcal of work done to it, and releases 5.00 times 102 kJ of heat into its surroundings, what is the change in internal energy of the system? Classify each of the following as a path function or a state function. A 1687 kg car is traveling down the road at 105.0 km/h. While traveling at this rate of speed, what is the kinetic energy of this vehicle in kilojoules? Convert the following energy units, 451 kJ to J 2060 kcal to kJ 9.77 x 106 J to kcal

Explanation / Answer

1) Given dH = -111.4 kJ and dS = -25 J/K

and temp =298 K

we know that dG =dH -TdS

dG = -111.4 kJ - 298 x -25

dG = -111.4 + 7.45

dG = -103.95 kJ

dG is -103.95 kJ

2) a ) ++ , liquid to gas , solid to liquid , solid to gas

b) +- , none

c) - + ,none

d) -- , gas to liquid , gas to solid ,liquid to solid

3) MgCl2 + H20 ---- > Mg0 + 2Hcl

dH rxn = dHf products - dHf reactants

dHrxn = dHf Mg0 + 2 dHf Hcl - dHf Mgcl2 - dHf H20

= -601.24 - 2 x 92.30 + 641.8 +285.8

= 141.76

dHrxn is 141.76 kJ

4) the final equation is obtained by

1 + (6 x2) + 3 - (2 x 4)

so dH = 1 dH1 + 6dH2 + 3dH3 - 2dH4

dH = -650 - 6 x 74.8 - 3 x 1845 + 2 x 416

dH = -5801.8 kJ

dH is -5801.8 kJ

5)

34 x 103 = heat / change in temp

heat = 34 x 103 x change in temp

heat = 34 x 103 x 2.17

heat = 73.78 x 103 J

heat = 73.78 x 103 /4.184 cal

heat = 17633.64 cal

given mass = 4.20

energy per gram = 17633.64 / 4.20

energy per gram = 4198.53

nutritional value per gram is 4198.53 cal

6)

we know that heat = mc dT

cahnge in temp = 12.7

c = Q/ mdT

= 1250 / 43.5 x 12.7

= 2.26

c is 2.26 J/g/C = 2.26 x 86 J/mol/K

molar heat capacity is 194.36 J /mol/K

7) Given 420 g of water at 25C and 130 g at 95 C

heat lost by hot water = heat gained by cold water

130 x Sw x ( 95-T) = 420 x Sw x ( T-25)

T = 41.54 C

final temp of the mixture is 41.54 C

8) we know that heat = mc dT

cahnge in temp = 108.6 -24.2 = 84.4

c = Q/ mdT

= 2755 / 54.21 x 84.4

= 0.60

c is 0.60 J/g/C

9) work done = 325 kCal =1359.8 kJ

Heat released = 500 kJ

change in internal energy = -500 + 1359.8

change in internal enegy =859.8 kJ

10) Path functions --work ,heat ,distance travelled

State functions - Enthalpy ,Energy

11)

kinetic enrgy = MV2/ 2

Given M = 1687

V = 105 km/h = 105 x 5/18 = 29.167

K.E = 1687 x (29.167) 2/ 2

K.E = 717.56 kJ

kinetic energy is 717.56 kJ

12) 451 kJ is 451000 J

2060 k Cal = 2060 x 4.184 kJ = 8619.04 k J

9.77 x 106 J = 2335.08 k Cal

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