More chemistry help please :\

[whc235]

---

Members don't see this ad.

Thanks guys for answering my previous post. Very helpful and I can't thank you enough. Ok more chemistry struggle .. this is what happens .. when u're relearning everything from year 1...

.10. Hydrogen sulfide reacts with sulfur dioxide to give H2O and S. If 6.00 L of H2S gas at 750. torr produced 3.20 g of sulfur, what is the temperature in C?: * .
.a. –165 °C.
.b. 10500 °C.
.c. 208 °C.
.d. 803 °C.

..
.
Please respond to the question above... 14. A 135 g sample of nickel at 95.0 °C is placed in 100. g of water at 25.0 °C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g•K) : * .
.a.13.3 °C.
.b.33.8 °C.
.c.45.1 °C.
.d.54.4 °C.



..
.
Please respond to the question above... 16. 90.0 g of iron(III) chloride reacts with 52.0 g of hydrogen sulfide. What is the mass of HCl is produced and what mass of excess reactant remains after the reaction?: * .
.a. 111 g HCl and 74.7 g FeCl3.
.b. 60.8 g HCl and28.4 g H2S.
.c. 111 g HCl and 164 g FeCl3.
.d. 60.8 g HCl and 23.6 g H2S
.





..
.
Please respond to the question above... 19. The heat of reaction for the following reaction is -850. kJ:.
.2Al(s) + Fe2O3 (s) →2Fe(s) + Al2O3 (s).
.
What is the enthalpy change when 1.5 mol of iron reacts with excess aluminum oxide?: * .
.a.638 kJ.
.b.-638 kJ.
.c. 1.3 x 103 kJ.
.d. -1.3 x 103 kJ.

Can't thank you enuff!

 

[prsndwg]

.10. Hydrogen sulfide reacts with sulfur dioxide to give H2O and S. If 6.00 L of H2S gas at 750. torr produced 3.20 g of sulfur, what is the temperature in C?: * .
.a. –165 °C.
.b. 10500 °C.
.c. 208 °C.
.d. 803 °C

write and balance the formula 1st:
2H2S + SO2 => 2H2O + 3S

Use stoichiomerty to find the moles of H2S.
3.2 g S (1mole S/ 32g S) (2 mole H2S/ 3 mole S) = 0.06 moles of H2S

Then use PV=nRT 750torr/760torr (6L) = .06 moles of H2S (0.08) T T= Kelvin -273 is ~ 800ish
.

 

[rowill]

14. A 135 g sample of nickel at 95.0 °C is placed in 100. g of water at 25.0 °C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g•K) : *
a.13.3 °C
b.33.8 °C
c.45.1 °C
d.54.4 °C

you need to look up the specific heat capacity of water (4.185 J/g*k)

This is an enthalpy question where the heat (q) from the nickel is being transferred to the water.

so... q (nickel) = - q (water)
recall q= (mass)(speecific heat)(change in temp)

q(nickel) = (135g)(.444)(Tf-95)
= 59.94 Tf - 5694.3

q(water) = - (100g)(4.185)(Tf - 25)
= - (418.5 Tf - 1046.25)
= -418.5Tf + 1046.25

59.94 Tf - 5694.3 = -418.5Tf + 10462.5
Tf = 33.77

 

[ads]

16. 90.0 g of iron(III) chloride reacts with 52.0 g of hydrogen sulfide. What is the mass of HCl is produced and what mass of excess reactant remains after the reaction?: *
.a. 111 g HCl and 74.7 g FeCl3.
.b. 60.8 g HCl and28.4 g H2S.
.c. 111 g HCl and 164 g FeCl3.
.d. 60.8 g HCl and 23.6 g H2S
.
.The answer to this question is b..

.First you have to balance the equation which gives you: 2 FeCl3 + 3H2S => 6 HCl + Fe2S3.
..
.Second you need to figure out what the limiting reagent is. FeCl3 is the limiting reagent because there are less moles of this than H2S..
..
.Third just complete the stoichiometry. .
.90g FeCl3(1mol FeCl3/163g FeCl3) * (6mol HCl/2mol FeCl3) * (36g HCl/1mol HCl) = Approximately 60g HCl.
..
.90g FeCle(1mol FeCl3/163g FeCl3) * (3mol H2S/2mol FeCl3) * (36g H2S/1mol H2S) = Approximately 30g H2S.
..
.Hope this helps 🙂
.