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What mass of NaCl is needed to produce 500 mL of a 2.0 mol/L solution?
as2s3+nano3+na2co3 -> na3aso4 + na2so4 + nano2 +co2 determine the theoretical mass of reactants needed to form 50 g of sodium arsenate
1. How many moles of Na2SO4 are produced by reaction of 124 g of NaOH with sufficient H2SO4?
2. How many moles of PbI2 can be prepared by the reaction of 0.128 mol of Pb(NO3)2 and 0.206 mol NaI?
3. A sample of a hydrocarbon (a compound of carbon and hydrogen only) is burned, and 1.10 g CO2 and 0.450 g H2O are produced. What is the empirical formula of the hydrocarbon?
4. What is the molarity of a solution prepared by dissolving 63.0 g NaF in enough water to make 250.0 mL of solution?
5. Calculate the number of milliliters of 1.25 M solution required to contain 0.622 mol of solute.
6. What is the concentration of a solution containing 1.23 mmol in 1.00 mL?
7. What is the final concentration of 2.00 L of 3.00 M solution if enough water is added to dilute the solution to 10.0 L?
8. What is the concentration of a solution prepared by diluting 25.0 mL of 3.00 M solution to 60.0 mL?
9. Calculate the number of moles of AgCl that can be prepared by mixing 0.740 L of 1.25 M AgNO3 with excess NaCl.
2. How many moles of PbI2 can be prepared by the reaction of 0.128 mol of Pb(NO3)2 and 0.206 mol NaI?
3. A sample of a hydrocarbon (a compound of carbon and hydrogen only) is burned, and 1.10 g CO2 and 0.450 g H2O are produced. What is the empirical formula of the hydrocarbon?
4. What is the molarity of a solution prepared by dissolving 63.0 g NaF in enough water to make 250.0 mL of solution?
5. Calculate the number of milliliters of 1.25 M solution required to contain 0.622 mol of solute.
6. What is the concentration of a solution containing 1.23 mmol in 1.00 mL?
7. What is the final concentration of 2.00 L of 3.00 M solution if enough water is added to dilute the solution to 10.0 L?
8. What is the concentration of a solution prepared by diluting 25.0 mL of 3.00 M solution to 60.0 mL?
9. Calculate the number of moles of AgCl that can be prepared by mixing 0.740 L of 1.25 M AgNO3 with excess NaCl.
1. A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction
was: 2 H2 0 + 2 e - → H2 + 2 OH-. If a current of 3.0 amp was used for 30 min, what weight of H2 gas would be produced?
2. What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in
the electrolysis of H2 O?
3. Give the notation for a cell that utilizes the reaction: a) Cl2 (g) + 2 I – (aq) → 2 Cl – (aq) + I2 (s) b) What is the E° for the cell? c) Which electrode is the cathode?
4. The standard electrode potential for the Fe2+ ↔ Fe3+ + e – half reaction is -0.770 V. a)
Using the Nernst equation [ E = E°− ( 0.059/n) log [Oxid]/[Red]] calculate the voltage of this half-cell when the [Fe3+] is 1.0 x 10 -3 and [Fe2+] is 1.0 x 10 -1. b) Calculate the approximate equilibrium constant (K) for the half reaction.
was: 2 H2 0 + 2 e - → H2 + 2 OH-. If a current of 3.0 amp was used for 30 min, what weight of H2 gas would be produced?
2. What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in
the electrolysis of H2 O?
3. Give the notation for a cell that utilizes the reaction: a) Cl2 (g) + 2 I – (aq) → 2 Cl – (aq) + I2 (s) b) What is the E° for the cell? c) Which electrode is the cathode?
4. The standard electrode potential for the Fe2+ ↔ Fe3+ + e – half reaction is -0.770 V. a)
Using the Nernst equation [ E = E°− ( 0.059/n) log [Oxid]/[Red]] calculate the voltage of this half-cell when the [Fe3+] is 1.0 x 10 -3 and [Fe2+] is 1.0 x 10 -1. b) Calculate the approximate equilibrium constant (K) for the half reaction.
It takes 585 J of energy to raise the temperature of 125.6 g mercury from 20.08C to 53.58C. Calculate the specific heat capacity and the molar heat capacity of mercury.
Calculate the standard entropy of formation of liquid ethanol at 25°C. [S0(Cgraphite) = 160.70J/K•mol, S0(O2) = 205.14 J/K•mol, S0(H2) = 130.68 J/K•mol, S0(C2H5OH) = 130.68 J/K•mol]
H2C2O4.2H2O(s) is a primary standard substance. 2.3688 g of oxalic acid dihydrate were completely neutralized by 42.56 ml of NaOH solution. Calculate the molar concentration of the NaOH solution.
What mass of Na2S2O3 is needed to react with 0.12 g of Cl2?
A student uses a pH meter to measure the pH of a 2.0 M solution of ammonium hydroxide. The pH meter reads 12.94. What is the pOH of the solution?
The three major isotopes of lead are Pb-206, Pb-207 and Pb-208. If they exist in the abundances 19.4%, 40.3% and 40.3% respectively, what is the AVERAGE ATOMIC MASS of lead? *SHOW YOUR WORK!
