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dibrmoethane DE, P* = 22.9 kpa at 358 K and dibromopropene DP, P* = 17.1 kPa at 358 K form a nearly ideal solution if X(DE) = .6, what is

(i) Ptotal when the system is all liquid

(ii) the composition of the vapour when the system is all liquid

dibrmoethane DE, P* = 22.9 kpa at 358 K and dibromopropene DP, P* = 17.1 kPa at 358 K form a nearly ideal solution if X(DE) = .6, what is

(i) Ptotal when the system is all liquid

(ii) the composition of the vapour when the system is all liquid

10. CISPLATIN (Pt(NH3)2CL2) IS A COMMON CHEMOTHERAPEUTIC AGENT AND IS PREPARED BY REACTING AMMONIA WITH POTASSIUM TETRACHLOROPLATINATE: K2PtCL4 + NH3 ----------> KCL + Pt(NH3)2CL2. HOW MANY GRAMS OF AMMONIA ARE NEEDE TO REACT WITH 50.0 GRAMS OF POTASSIUM TETRACHLOROPLATINATE? THEN CALCULATE HOW MANY GRAMS OF CISPLATIN ARE FORM FROM 50.0 GRAM OF POTASSIUM TETRACHLOROPLATINATE, IF THE YEILD FOR REACTION IS 75 PRECENT.

10. CISPLATIN (Pt(NH3)2CL2) IS A COMMON CHEMOTHERAPEUTIC AGENT AND IS PREPARED BY REACTING AMMONIA WITH POTASSIUM TETRACHLOROPLATINATE: K2PtCL4 + NH3 ----------> KCL + Pt(NH3)2CL2. HOW MANY GRAMS OF AMMONIA ARE NEEDE TO REACT WITH 50.0 GRAMS OF POTASSIUM TETRACHLOROPLATINATE? THEN CALCULATE HOW MANY GRAMS OF CISPLATIN ARE FORM FROM 50.0 GRAM OF POTASSIUM TETRACHLOROPLATINATE, IF THE YEILD FOR REACTION IS 75 PRECENT.

Answer the following questions and explain briefly (in no more than three sentences):

a. Does the addition of an inert diluent to the reactants entering an exothermic process increase, decrease, or make no change in the heat transfer to or from the process?

b. If the reaction in a process is incomplete, what is the effect on the value of the standard heat of reaction? Does it go up, go down, or remain the same?

c. Consider the reaction H2 (g) + 1⁄2 O2 (g) → H2O (g). Is the heat of reaction with the reactants entering and the products leaving at 500 K higher, lower, or the same as the standard heat of reaction?

Answer the following questions and explain briefly (in no more than three sentences):

a. Does the addition of an inert diluent to the reactants entering an exothermic process increase, decrease, or make no change in the heat transfer to or from the process?

b. If the reaction in a process is incomplete, what is the effect on the value of the standard heat of reaction? Does it go up, go down, or remain the same?

c. Consider the reaction H2 (g) + 1⁄2 O2 (g) → H2O (g). Is the heat of reaction with the reactants entering and the products leaving at 500 K higher, lower, or the same as the standard heat of reaction?

How much magnesium sulfate and magnesium chloride will be needed to be dissolved in 1 gallon of water to contain 47,000 ppm magnesium, 70,000 ppm sulfate, and 86,000 chloride? in grams ? and in mL?

This is what I did, but it is not making sense. I need 332 g of MgSO4 and 438 g MgCl2 that does not equal 789 g. Where are the other 19 grams coming from?

1 gallon = 3.78541 L

1 ppm = 1 mg/L

70,000 ppm sulfate = 70,000 mg/L sulfate

So, sulfate concentration in 3.78541 L (1 gal) = 70,000 x 3.78541 = 264,978.7 mg is 70,000 ppm

1 MgSO4 has 1 Mg2+ and 1 sulfate

So, MgSO4 required to get 70,000 ppm SO4^2- in 1 gal water = 264,978.7 mg x 120.37 g/mol/96.06 g/mol = 332,037 mg = 332 g

For 86,000 ppm Cl = 86,000 mg/L x 3.78541 L = 325,545.26 mg to make 86,000 ppm in 1 gallon

So, MgCl2 required to get 86,000 ppm Cl- in 1 gal water = 325,545.26 mg x (95.2 g/mol/2)/35.4 g/mol = 437,739 mg = 438 g

Mg2+ concentration required = 47,000 ppm = 47,000 mg/L = 47,000 x 3.78541 = 177,914.27 mg in 1 gallon MgSO4 + MgCl2 = 1 Mg (from sulfate) + 1 Mg (from MgCl2) = 88957.15 mg each

So for 47,000 ppm total Mg, MgSO4 + MgCl2 required = 88957.15 mg x 120.37 g/mol/24.3 g/mol + 88957.15 mg x 95.2 g/mol/24.3 g/mol = 440,558.41 mg (MgSO4) + 348,435.33 mg (MgCl2) = 788,994 mg = 789 g

How much magnesium sulfate and magnesium chloride will be needed to be dissolved in 1 gallon of water to contain 47,000 ppm magnesium, 70,000 ppm sulfate, and 86,000 chloride? in grams ? and in mL?

This is what I did, but it is not making sense. I need 332 g of MgSO4 and 438 g MgCl2 that does not equal 789 g. Where are the other 19 grams coming from?

1 gallon = 3.78541 L

1 ppm = 1 mg/L

70,000 ppm sulfate = 70,000 mg/L sulfate

So, sulfate concentration in 3.78541 L (1 gal) = 70,000 x 3.78541 = 264,978.7 mg is 70,000 ppm

1 MgSO4 has 1 Mg2+ and 1 sulfate

So, MgSO4 required to get 70,000 ppm SO4^2- in 1 gal water = 264,978.7 mg x 120.37 g/mol/96.06 g/mol = 332,037 mg = 332 g

For 86,000 ppm Cl = 86,000 mg/L x 3.78541 L = 325,545.26 mg to make 86,000 ppm in 1 gallon

So, MgCl2 required to get 86,000 ppm Cl- in 1 gal water = 325,545.26 mg x (95.2 g/mol/2)/35.4 g/mol = 437,739 mg = 438 g

Mg2+ concentration required = 47,000 ppm = 47,000 mg/L = 47,000 x 3.78541 = 177,914.27 mg in 1 gallon MgSO4 + MgCl2 = 1 Mg (from sulfate) + 1 Mg (from MgCl2) = 88957.15 mg each

So for 47,000 ppm total Mg, MgSO4 + MgCl2 required = 88957.15 mg x 120.37 g/mol/24.3 g/mol + 88957.15 mg x 95.2 g/mol/24.3 g/mol = 440,558.41 mg (MgSO4) + 348,435.33 mg (MgCl2) = 788,994 mg = 789 g

Be sure to answer all parts.

When gaseous F2 and solid I2 are heated to high temperatures, the I2 sublimes and gaseous iodine heptafluoride forms. 3.50 × 102 torr of F2 and 4.00 g of solid I2 are put into a 2.50 L container at 2.50 × 102 K and the container is heated to 5.50 × 102 K.

(a) What is the final pressure? Ptotal = atm

(b) What is the partial pressure of I2 gas? PI2 = atm I2

Be sure to answer all parts.

When gaseous F2 and solid I2 are heated to high temperatures, the I2 sublimes and gaseous iodine heptafluoride forms. 3.50 × 102 torr of F2 and 4.00 g of solid I2 are put into a 2.50 L container at 2.50 × 102 K and the container is heated to 5.50 × 102 K.

(a) What is the final pressure? Ptotal = atm

(b) What is the partial pressure of I2 gas? PI2 = atm I2

A mixture is prepared that is 5.0% (w/w) of an unknown substance mixed with naphthalene (molar mass = 128.2 g mol-1). The freezing point of this mixture is found to be 77.3 °C. What is the molar mass of the unknown substance? (The melting point of naphthalene is 80.2 °C and Kf = 6.9 °C m-1.)

A mixture is prepared that is 5.0% (w/w) of an unknown substance mixed with naphthalene (molar mass = 128.2 g mol-1). The freezing point of this mixture is found to be 77.3 °C. What is the molar mass of the unknown substance? (The melting point of naphthalene is 80.2 °C and Kf = 6.9 °C m-1.)

2. IN AN AQUEOUS REACTION, BARIUM NITRATE PLUS POTASSSIUM SULFATE YIELDS POTASSIUM NITRATE AND BARIUM SULFATE. 100 GRAMS OF BARIUM NITRATE IS MIXED WITH SUFFICIENT WATER TO MAKE EXACTLY 2000 ML OF SOLUTION. CALCULATE THE MOLARITY OF THE POTASSIUM SULFATE SOLUTION. THEN, IF 200 GRAMS OF BARIUM NITRATE WERE DISSOLVED IN SUFFICIENT WATER TO MAKE 2 LITERS, HOW MANY ML OF THE POTASSIUM SULFATE SOLUTION WOULD BE REQUIRED TO REACT COMPLETELY WITH 35.00 ML OF THE BARIUM NITRATE SOLUTION.

2. IN AN AQUEOUS REACTION, BARIUM NITRATE PLUS POTASSSIUM SULFATE YIELDS POTASSIUM NITRATE AND BARIUM SULFATE. 100 GRAMS OF BARIUM NITRATE IS MIXED WITH SUFFICIENT WATER TO MAKE EXACTLY 2000 ML OF SOLUTION. CALCULATE THE MOLARITY OF THE POTASSIUM SULFATE SOLUTION. THEN, IF 200 GRAMS OF BARIUM NITRATE WERE DISSOLVED IN SUFFICIENT WATER TO MAKE 2 LITERS, HOW MANY ML OF THE POTASSIUM SULFATE SOLUTION WOULD BE REQUIRED TO REACT COMPLETELY WITH 35.00 ML OF THE BARIUM NITRATE SOLUTION.

Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25°C.

Write the equation for the cell reaction that occurs under standard-state conditions. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer.)

Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25°C.

Write the equation for the cell reaction that occurs under standard-state conditions. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer.)

If two isomers have been classified correctly as anomers, they may be also called

1) conformers

2) enantiomers

3) tautomers

4) diastereomers  

If the cube roots of unity are 1, w, w2, then the roots of the equation (x – 1)3 + 8 = 0 are

1) – 1, 1 + 2w, 1 + 2w2

2) – 1, 1 – 2w, 1 – 2w2

3) – 1, – 1, – 1

4) None of these  

Consider the compound Na2[Cr(NH3)2(NCS)4]. What is the coordination number with work shown?

Consider the compound Na2[Cr(NH3)2(NCS)4]. What is the coordination number with work shown?

Which of the following trends in lattice energy is due to differences in ionic radii?

the answer NaF > CsCl > CsBr explain ?

Which of the following trends in lattice energy is due to differences in ionic radii?

the answer NaF > CsCl > CsBr explain ?

Consider that 0.100 L of methane gas, CH4(g), at 25.0 C and 744 mmHG is burned at constant pressure in air. The heat produced is captured and used to melt 9.53 g of ice at 0 C. Write an equation for the complete combustion of methane and show through calculation that the combustion is incomplete in this case.

Consider that 0.100 L of methane gas, CH(g), at 25.0 C and 744 mmHG is burned at constant pressure in air. The heat produced is captured and used to melt 9.53 g of ice at 0 C. Write an equation for the complete combustion of methane and show through calculation that the combustion is incomplete in this case.

Consider that 0.100 L of methane gas, CH4(g), at 25.0 C and 744 mmHG is burned at constant pressure in air. The heat produced is captured and used to melt 9.53 g of ice at 0 C. Write an equation for the complete combustion of methane and show through calculation that the combustion is incomplete in this case.

Consider that 0.100 L of methane gas, CH(g), at 25.0 C and 744 mmHG is burned at constant pressure in air. The heat produced is captured and used to melt 9.53 g of ice at 0 C. Write an equation for the complete combustion of methane and show through calculation that the combustion is incomplete in this case.

what volume of 0.179M Na3PO4 solution is necessary to completely react with 92.3 mL of 0.122 M CuCl2

what volume of 0.179M Na3PO4 solution is necessary to completely react with 92.3 mL of 0.122 M CuCl2

The reaction of tert-butyl-bromide (CH3)3CBr with water is represented by the equation:

(CH3)3CBr + H2O → (CH3)3COH + HBr

The following data were obtained from three experiments using the method of initial rates:

a. What is the order with respect to (CH3)3CBr?

b. What is the order with respect to H2O?

c. What is the overall order of the reaction?

d. Write the rate equation.

e. Calculate the rate constant k for the reaction

The reaction of tert-butyl-bromide (CH3)3CBr with water is represented by the equation:

(CH3)3CBr + H2O → (CH3)3COH + HBr

The following data were obtained from three experiments using the method of initial rates:

a. What is the order with respect to (CH3)3CBr?

b. What is the order with respect to H2O?

c. What is the overall order of the reaction?

d. Write the rate equation.

e. Calculate the rate constant k for the reaction

6. At 150°C the decomposition of acetaldehyde CH3CHO to methane is a first order reaction. If the rate constant for the reaction at 150°C is 0.029 min-1 , how long does it take a concentration of 0.050 mol L-1 of acetaldehyde to reduce to a concentration of 0.040 mol L-1 ?

7. The decomposition of hydrogen iodide into hydrogen and iodine is a second order reaction. The rate constant k = 0.080 L mol-1 s-1 . How long does it take an initial concentration of 0.050 M to decrease to half this concentration?

8. The gold-198 isotope has a half-life of 2.7 days. If you start with 10 mg at the beginning of the week, how much remains at the end of the week, seven days later?

PLEASE SHOW FULL WORK. Thanks

6. At 150°C the decomposition of acetaldehyde CH3CHO to methane is a first order reaction. If the rate constant for the reaction at 150°C is 0.029 min-1 , how long does it take a concentration of 0.050 mol L-1 of acetaldehyde to reduce to a concentration of 0.040 mol L-1 ?

7. The decomposition of hydrogen iodide into hydrogen and iodine is a second order reaction. The rate constant k = 0.080 L mol-1 s-1 . How long does it take an initial concentration of 0.050 M to decrease to half this concentration?

8. The gold-198 isotope has a half-life of 2.7 days. If you start with 10 mg at the beginning of the week, how much remains at the end of the week, seven days later?

PLEASE SHOW FULL WORK. Thanks

10. The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism.

The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and an ozone molecule:

Step 1: O3(g) O2(g) + O(g) Fast, reversible, reaction

Step 2: O3(g) + O(g) → 2O2(g) Slow

a. Which is the rate determining step?

b. Write the rate equation for the rate-determining step.

Please show full work

c. Write the rate equation for the overall reaction.

10. The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism.

The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and an ozone molecule:

Step 1: O3(g) O2(g) + O(g) Fast, reversible, reaction

Step 2: O3(g) + O(g) → 2O2(g) Slow

a. Which is the rate determining step?

b. Write the rate equation for the rate-determining step.

Please show full work

c. Write the rate equation for the overall reaction.

1. Carbon tetrachloride has a vapor pressure of 213 torr at 40.°C and 888 torr at 82°C. What is the normal boiling point of CCl4? Boiling point = ___ C 2. Diethyl ether was one of the first chemicals used as an anesthetic. At 34.6°C, diethyl ether has a vapor pressure of 760. torr, and at 18.1°C, it has a vapor pressure of 407 torr. What is the ΔH of vaporization for diethyl ether? ΔH of vaporization = ___ kJ/mol

1. Common commercial hydrochloric acid is an aqueous solution that is 38% HCl by mass, with a density of 1.19 g/cm^3. Calculate the molarity of this reagent. Molarity = ___mol/L Calculate the molality of this reagent. Molality = ___mol/kg Calculate the mole fraction of this reagent. Mole fraction = 2. Common commercial nitric acid is an aqueous solution that is 70.% HNO3 by mass, with a density of 1.42 g/cm^3. Calculate the molarity of this reagent. Molarity = ___mol/L Calculate the molality of this reagent. Molality = ___mol/kg Calculate the mole fraction of this reagent. Mole fraction = 3. Common commercial sulfuric acid is an aqueous solution that is 95% H2SO4 by mass, with a density of 1.84 g/cm^3. Calculate the molarity of this reagent. Molarity = ___mol/L Calculate the molality of this reagent. Molality = ___mol/kg Calculate the mole fraction of this reagent. Mole fraction = 4.Common commercial acetic acid is an aqueous solution that is 99% by mass CH3CO2H, with a density of 1.05 g/cm^3. Calculate the molarity of this reagent. Molarity = ___mol/L Calculate the molality of this reagent. Molality = ___mol/kg Calculate the mole fraction of this reagent. Mole fraction = 5. Common commercial ammonia is an aqueous solution that is 28% NH3 by mass, with a density of 0.90 g/cm^3. Calculate the molarity of this reagent. Molarity = ___mol/L Calculate the molality of this reagent. Molality = ___mol/kg Calculate the mole fraction of this reagent. Mole fraction =

1. Pentane (C5H12) and hexane (C6H14) form an ideal solution. At 25oC the vapor pressures of pentane and hexane are 511 and 150 torr, respectively. A solution is prepared by mixing 25 mL pentane (density, 0.63 g/mL) with 36 mL hexane (density, 0.66 g/mL). What is the vapor pressure of the resulting solution? Ptotal = ___ torr 2. Pentane (C5H12) and hexane (C6H14) form an ideal solution. At 25oC the vapor pressures of pentane and hexane are 511 and 150 torr, respectively. A solution is prepared by mixing 25 mL pentane (density, 0.63 g/mL) with 36 mL hexane (density, 0.66 g/mL). What is the composition by mole fraction of pentane in the vapor that is in equilibrium with this solution? X V pen = ___