on being heated srtongly ,solid A decomposes completely togive oxygen  gas and solid potassiumchloride                                        IF 1.00g of solid A isdecomposed completely in this way ,calculate the volume of oxygen gas produced at room temperature andpressure  (one mole of gas at room temperature andpressure occupies 24 dm)

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18 Dec 2019

on being heated srtongly ,solid A decomposes completely togive oxygen  gas and solid potassiumchloride                                      
 
 
IF 1.00g of solid A isdecomposed completely in this way ,calculate the volume of oxygen gas produced at room temperature andpressure  (one mole of gas at room temperature andpressure occupies 24 dm)

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At elevated temperatures,SbCl5 gas decomposes into SbCl3 gas andCl2 gas, as shown by the following equation.
SbCl5 <===> SbCl3 + Cl2
An 89.7-gram sample of SbCl5 (molecular weight 299.0) isplaced inan evacuated 15.0-liter container at 182 Â°C.
(1) What is the concentration in moles per liter of SbCl5 in thecontainer before any decomposition occurs?
(2) What is the pressure in atmospheres of SbCl5 in the containerbefore any decomposition occurs?
b) If the SbCl5 is 29.2 percent decomposes when equilibrium isestablished at 182 Â°C, calculate the value for either equilibriumconstant, Kp or Kc, for this decomposition reaction.Indicatewhether you are calculating Kp or Kc.
c) In order to produce some SbCl5, a 1.00-mole sample of SbCl3 isfirst placed in an empty 2.00-liter container maintained at atemperature different from 182 Â°C. At this temperature Kc equals0.117. How many moles of Cl2 must be added to this container toreduce the number of moles of SbCl3 to 0.700 mole atequilibrium?

I understand 1 and 2 but I am stuck on (b) and (c)
i read somewhere that for (b) [SbCl3] = [Cl2] can you explain whyplease?? and i would love to have the work done in as much detailedEXPLANATION as possible (not just numbers and formulas)... thankyou!!

crimsonmammoth698

18. Hydrogen gas reacts with oxygen gas to form water vapor. If 34.5 g of hydrogen gas react with 26.6 g of oxygen gas, how many grams of water vapor will be produced? 2H2(g) + O2(g) --> 2H2O(g)

20. The reaction of 22.5 g of Fe with excess of oxygen gas produced 24.2 g of Fe2O3. Calculate the percent yield.

21. Milk of magnesia contains magnesium hydroxide. Mg(OH)2 reacted with HCl to form aqueous magnesium chloride and liquid water. Write the properly balanced equation for this reaction.

22. Lithium reacted with oxygen gas to form lithium chloride. The chemical formula for lithium chloride is___________.

(A). LiO (B). LiO2 (C). Li2O3 (D). Li2O (E). Li2O4

23. In the following reaction, how many grams of sodium sulfate are needed to react with 3.08 moles of strontium nitrate? (Hint: stoichiometry mol Na2SO4: mol Sr(NO3)2 = 1 mol: 1 mol) Sr(NO3)2 (aq) + Na2SO4 (aq) --> SrSO4 (s) + 2 NaNO3 (aq) (balanced?)

24. Which of the following represents a chemical property of oxygen gas?

(A). It is gaseous at room temperature. (B). It reacts explosively with propane. (C). It is less dense than air. (D). It is colorless

Practice problems for exam 2 ______________

Useful Information:

h=6.626Ã10-34JÂ·s.; c=3.0Ã108 m/sec; E=hï® ; E= hc , ï¬ = h/mv; 1J = 1 kg-m2/s2 ï¬

mass of electron = 9.11 Ã 10-28 g, ïE= q + w ; 1 cal = 4.184 Joules Please Show all Work

1. Which of the following substances have standard heats of formation that are equal to zero by definition (circle your answers): H2(g), H(g), O3(g), H2O(s), H2O(l), Hg(l), Hg(s), Hg(g).

2. Limestone stalactites are formed in the reaction: Ca2+(aq) + HCO3-(aq) ï CaCO3(s) + CO2(g) +

H2O(l)
If one mole of CaCO3 is produced at 298 K under one atmosphere of pressure, the reaction performs 590 calories of expansion work, pushing back the atmosphere as CO2 is formed. At the same time, 9310 calories of heat are absorbed from the environment. What is ïE in Kcal/mole for CaCO3.

3. What is the minimum wavelength of light in AÌ (1 AÌ = 10-8 cm) needed to provide enough energy per quantum to rupture the chemical bond in hydrogen iodide (HI). The bond dissociation energy of HI is 71.4 Kcal/mole.

4. Sketch the shape and orientation of the following types of orbitals: s, px, dxy, dz2, dx2-y2

5. Give the values of (n) , (l) and (ml) for each orbital in the 4p subshell.

6. Write the complete electron configuration for the following: Ti 2+_____________________________________ Cr_______________________________________

N______________________________________

7. Calculate the standard enthalpy of formation ( ï Ho) for diamond from graphite [i.e. C (graphite) ï C (diamond)] given that:

C (graphite) + O2 ï CO2 (g) ( ï Ho = -393.5 KJ/mole) C (diamond)] + O2 ï CO2 (g) ( ï Ho = -395.4 KJ/mole)

If 1.0g of graphite is converted to diamond, what is the energy change? Is this an endothermic or exothermic reaction?

8. An 160 pound astronaut on his way to Mars is buzzing along at 10,000 miles per hour. (a) Express his weight in grams (one pound = 454 grams) so that you can calculate the astronautâs wavelength (1mile/hour = 44.7 cm/sec)

(b) Suppose the astronaut detects outside his spacecraft a proton (m=1.7 x 10-24 g) from a âsolar windâ moving at exactly the spacecraft velocity. What is the proton wavelength is in AÌ (1 AÌ = 10-8 cm.

9. What is the maximum number of electrons that can occupy each of the following subshells? a) 3d_________________ b) 1s____________________ c) 2p ____________________

10. Identify the element represented by the following electronic configuration.

a) [Ne] 3s2____________________

b) What is the electron configuration for the first excited state of this atom.______________

11. Determine the number of valence electrons for each element.
(a) Br___________ (b) Na _________ (c) Sn __________

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The heat of formation for the following substances is given in kJ/mol:

CS2 CO2 SO2 117.4 -393.51 -296.83

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a. Ca(g) ï Ca(g)+2 + 2e-
b. I(g)+1e-ï I(g)-1
c. Ca(g)+2 + S(g)-2 ï CaS(s) d. I2(g)ï 2I(g)

( ) ( ) ( ) ( )

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a) O-2 or Na+ b) Ti+4 or Ti+2 c) B or C d) N or N-3

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ï H ï¯ f NaCl = -411KJ

Na(s) ï® Na(g) ï H =108KJ
1â2 Cl2 ï® Cl(g) ï H = 122KJ Ionization Energy of Na ï H = 496 KJ Electron affinity of Cl ï H = -349KJ

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