Questions asked by April W.

• Back to user's profile
• How many moles of chlorine are present in 2.47 g of phosphorus pentachloride?
  
• How many moles of cobalt III bromide are present in 4.34 grams of this compound?
  
• Write the net ionic equation for the precipitation of zinc hydroxide from aqueous solution: ?
  
• Consider the reaction when aqueous solutions of cobalt(II) bromide and iron(III) nitrate are combined. The net ionic equation for this reaction is: ?
  
• Consider the reaction when aqueous solutions of silver(I) nitrate and barium bromide are combined. The net ionic equation for this reaction is:?
  
• When aqueous solutions of potassium carbonate and cobalt(II) bromide are combined, solid cobalt(II) carbonate and a solution of potassium bromide are formed. The net ionic equation for this reaction is:? are they gas, solid, liquid, or aq?
  
• Write the net ionic equation for the precipitation of silver iodide from aqueous solution:?
  
• Write the net ionic equation for the precipitation of silver iodide from aqueous solution:?
  
• When solid Pb metal is put into an aqueous solution of Cu(NO3)2, solid Cu metal and a solution of Pb(NO3)2 result. Write the net ionic equation for the reaction.?
  
• Consider the reaction when aqueous solutions of lead(II) acetate and chromium(III) bromide are combined. The net ionic equation for this reaction is:?
  
• Consider the reaction when aqueous solutions of barium nitrate and potassium sulfate are combined.?
  
• Consider the reaction when aqueous solutions of calcium nitrate and potassium hydroxide are combined.?
  
• Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as K How many grams of KHP are needed?
  
• A 0.211 mol sample of an unknown gas contained in a 5.00 L flask is found to have a density of 2.50 g/L. The molecular weight of the unknown gas is g/mol.?
  
• A 0.176 mol sample of Kr gas is contained in a 8.00 L flask at room temperature and pressure. What is the density of the gas, in grams/liter, under these conditions?
  
• According to the ideal gas law, a 0.9766 mol sample of carbon dioxide gas in a 1.295 L container at 270.0 K should exert a pressure of 16.71 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal ?
  
• A 9.380 mol sample of nitrogen gas is maintained in a 0.8198 L container at 301.8 K. What is the pressure in atm calculated using the van der Waals' equation for N2 gas under these conditions? For N2, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol. atm?
  
• He rate of effusion of Ne gas through a porous barrier is observed to be 8.45x10 to the negative 4th mol/h. Under the same conditions, the rate of effusion of NH3gas would be ? mol/h.
  
• The average molecular speed in a sample of CO2 gas at a certain temperature is 384 m/s. The average molecular speed in a sample of H2gas is m/s at the same temperature. ?
  
• Compute the root-mean-square speed of H2 molecules in a sample of hydrogen gas at a temperature of 94°C. m s-1 ?
  
• The average molecular speed in a sample of CO2 gas at a certain temperature is 384 m/s. The average molecular speed in a sample of H2 gas is m/s at the same temperature.?
  
• Compute the root-mean-square speed of H2 molecules in a sample of hydrogen gas at a temperature of 193°C. m s-1 ?
  
• Arrange the following molecules in order of increasing average molecular speed. All are at the same temperature. hydrogen, nitrogen dioxide, sulfur dioxide, nitrogen Enter formulas in the boxes below: 1 = slowest, 4 = fastest ? 1 2 3 4
  
• Arrange the following molecules in order of increasing average molecular speed. H2 at 371K, NO2 at 339K, Ne at 371K, H2 at 425K Enter formulas and temperatures in the boxes below: 1 = slowest, 4 = fastest 1 at K 2 at K 3 at K 4 at K ???
  
• Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NaOH(aq) + 6H2O(l)2NaAl(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 747 m ?
  
• A 13.1 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 22.8 mL of 0.456 M potassium hydroxide are required to neutralize the nitric acid, what is the percent by mass of nitric acid in the mixture? % by mass?
  
• In the laboratory a student combines 39.3 mL of a 0.165 M manganese(II) chloride solution with 25.3 mL of a 0.328 M manganese(II) sulfate solution. What is the final concentration of manganese(II) cation ? M ?
  
• A sample of gas contains 0.2000 mol of CH4(g) and 0.4000 mol of O2(g) and occupies a volume of 20.3 L. The following reaction takes place: CH4(g) + 2O2(g)CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place in liters?
  
• A 9.380 mol sample of nitrogen gas is maintained in a 0.8198 L container at 301.8 K. What is the pressure in atm calculated using the van der Waals' equation for N2 gas under these conditions? For N2, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol. __ atm
  
• Consider the reaction when aqueous solutions of sodium acetate and cobalt(II) bromide are combined. The net ionic equation for this reaction is?: label aq, s, l, or g
  
• Consider the reaction when aqueous solutions of iron(III) chloride and silver(I) nitrate are combined. The net ionic equation for this reaction is:? label aq, l,g,s
  
• When N2(g) reacts with H2(g) to form NH3(g) , 92.2 kJ of energy are evolved for each mole of N2(g) that reacts.?
  
• Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels. The heat of combustion of cyclopropane, C3H6, is 499.8 kcal/mol. ?