A gas was found to have a densitiy of .08747 mg/ml at 17.0 degree C and a pressure of 76o torr. What is its molecular mass? What type of gas most likely is this?
A certain laser uses a gas mixture made up of 9.00 g HCL, 2.00 g H2, and 165.0 g Ne. What pressure is exerted by the mixture in a 75.0 L tank at 22 degree C? Which gas has the smallest partial pressure?
A 100 ml sample of .10 molar NAOH solution was added to 100 ml of .10 molar H3C6H5O7. After equilibrium was established, which of the ions listed below was present in the greatest concentration? A) H2C6H5O7^- B) HC6H5O7^2- C) C6H5O7^3- D) OH E) H^+ Please provide thorough explanation for this question.
1. Step 1: Cl2 ------ 2Cl (fast) Step 2: CHCl3 + Cl -------- CCl3 + HCl (slow) Step 3: CCl3 + Cl ------------CCl4 (fast) Identify the rate determining step, reaction intermediates and the experimental rate law (intermediates can not be in the rate law) 2. For the half-reaction XeF2(aq) +
The numerical value of the rate constant for the gaseous reaction 2N2O5------- 4NO2+ O2 was found to be 5.8*10-4. The initial concetration of N205 was 1.00mol/L. Assuming all measurements are recorded in seconds, determine the tim required for the reation to be 60% complete if the reaction is second order
1. 5.30 moles of gas, initially at 25 degrees celcius and 5.00 atm pressure, was allowed to expand adiabatically( with no heat exchange between systen and surroundings) against a constant external pressure of 1.50 atm until the initial volume had trebled. The heat capacity of the gas was known to be 37.1 J/ degree celuius mol
Estimate the critical constants of a gas with van der Waals parameters a= 1.32 atm L^2/mol^2 b = 0.0436 L/mol
Derive expression and numerical value for compression factor of gas that obeys the equation of state.
Derive an expression for the compression factor of a gas that obeys the equation of state P(V - nb) = nRT where b and R are constants. If the pressure and temperature are such that Vm = 10b, what is the numerical value of the compression factor? Extra Info. As a measure of the deviation from ideality of the behavi
The two figures show Cp VS T for various transitions. I need to know what the graph would look like for: 1. u (internal energy) vs T 2. S (Entropy) vs T 3. and V vs T for a first order (discontinuous) transition. Extra Info: FOr the equilibrium phase transitions at constant T and P (temperature and pressure) t
An ammonium ion selective electrode responds to both NH4+ and H+, but not to NH3. (pKa=9.244 for NH4+) A) What pH conditions must be imposed to ensure the electode properly represents toe activity of NH4+ B) Why is the ionic strength an important factor when using this or any ISE? How can you compensate for this effect?
In the study of a first-order reaction, A--->B, it is found that A/Ao=0.125 after one hour. The system initially consisted of 0.20 mole of a gaseous A at 25 degrees C and 1 atm. Calculate the initial rate of reaction in moles of A reacting per minute.
For the following mechanism: N205------>k1<--------k2 N02 + N03 N0 + N03 ------>k3 2N02 Using the steady-state assumption, find the expression for dPN02/dt Note. The k1 is on top of the right pointing arow and k2 is below the left pointing arrow and the arrows are like they are in equilibriu
Determine the percent by mass of all the elements in the compound cobalt III acetate.
How would you prepare a liter of "carbonate buffer" at a pH of 10.10? Ka = 4.2 times ten to the negative 7(carbonic acid) Ka = 4.8 times ten to the negative 11(bicarbonate ion) It says the key to solving the problem is picking the correct Ka value. How do I know which one to work with?
Find delta Smix, delta Gmix, delta Hmix, and delta Vmix if 125 g of benzene and 25 g of naphthalene are mixed at 60 degrees C. Assume the solution to be ideal. The molecular weights of benzene and naphthalene are 78.12 g/mol and 128.19 g/mol respectively.
Calculate the freezing point of 250 ml of water containing 7.5 g of sucrose. For water, Kf=1.86 K kg/mol. The molecular weight of sucrose is 342.3 g/mol.
(See attached file for full problem description) --- 31. A sample of H2 gas occupies 615 mL at C and 575 mm Hg. When the gas is cooled, its volume is reduced to 455 mL and its pressure is reduced to 385 mm Hg. What is the new temperature of the gas? 54. Hydrogen can be made in the "water gas reaction." If you
I need some help with this question: Two wines are available for blending: One tank of 1000 L has a Titratable Acidity of 9.0 g/L and another tank containing 2000 L has a Titratable Acidity of 0.6 g/L. How much volume do you need to blend to make the 9.0 g/L Titatrable Acid wine equivalent to 7.2 g/L? What is the final volu
Relationship of mole to amu. Is mole same thing as amu?
I need to find a simple way to convert gases expressed as mol % to volume percent. Pressure and temperature are constant. For example, what volume percent would water vapour be if given as 1.52 mol %?
Consider the combustion reaction for propane below. CH3CH2CH3(g)+5O2(g)-------->3 C02(g)+4H20(g) a) Determine the delta G standard state at 298 K from the following standard state values at T= 298 S(CH3CH2CH3)=269.9 J/K mol S(C02)= 213.7 J/K mol S(H20)=188.8 J/K mol S(02)=205.1 J/ K mol delta H(CH3CH2CH3)=-103.9 kJ/mol
Show that the partial of H with respect to P at constant T =0 for an ideal gas. Hint: start with dH=VdP+TdS. Divide by dP and impose constant T. Use a maxwell relation from dG.
The heat capacity of a gas is given by Cp=a+bT where a and b are constants: a) Determine delta S for heating the gas from T1 to T2 at constant P b) Determine delta G for heating the gas from T1 to T2 at constant P HINT: the integral lnx dx= x ln x-x
Find the entropy change delta for argon gas undergoing the following temperature and pressure changes: good Ar(g),P=1 atm, T=300 K------> Ar(g), P=10 atm, T=500K
Consider the reacton: 2 H2(g) + O2(g) -------> 2 H2O(g). Determine delta G for this reaction at 1000 K.
*** Please see file for full description*** 1. Into each of three potatoes insert 1 copper and 1 zinc probe. The probes should be inserted to a medium depth inside the potatoes and should be spaced within about an inch of each other. The probes should NOT touch inside or outside of the potato. IMPORTANT: To illuminate an
Consider the reaction. Mn3N2 (s) +H2O (l) → Mg(OH)2 (s) + NH3 (g) a) Balance the equation and name each compound. b) How many moles of Mg(OH)2 are produced from .319 mol of magnesium nitride? c) How many grams of water are necessary to produce 4.39 mol of ammonia? d) If 12.48g of magnesium hydroxide are
Balance the following equations: a. S(2)O(3)^2- (aq)+I(3)^- (aq) ->S(4)O(6)^2- (aq) + I^- (aq) b. Mn^2+(aq) + HBiO(3) (s) ->MnO(4)^- (aq) + Bio^+ (aq) (acid) c. Cr(2)O(7)^2- (aq) + H(3)AsO(3) -> H(3)AsO(4) (aq) + Cr^3+ (aq) (acid) d. CIO^1(aq) + Cro(2)^- (aq) ->Cl^- (aq) + CrO(4)^2- (aq) (Basic) e. Obr^- (aq) +HPO(3)^2- (
Consider two solutions. One solution is 0.1115 M Ca(OH)(2). The other is 0.1050 M HClO(4). a) Write a balanced equation for the reaction between the two solutions. b) How many mL of Ca(OH)(2) will be required to neutralize 25.00 mL of the HClO(4)? c) If a student starts to titrate 31.39 mL of the Ca(OH)(2) solut
Question 3: The salt NaBrO(3) oxides Sn^2+ to SnCl(6)^2- in the presence of hydrochloric acid according to the equation 3 Sn^2+ (aq) + 18 Cl^- (aq)+ BrO(3)^- (aq) + 6 H^+ (aq) -> 3 SnCl(6)^2- (aq) + Br^- (aq) + 3 H(2)O A sample weighing 2.000g is