Search & Filtering
How much heat (in joules) is used to heat a 39.79 gram sample of iron from 9.23 degrees Celcius to 100.00 degrees Celcius if the specific heat of Fe is 0.450 j/g*C? Record your answer to 2 decimal spaces.
Strontium chloride and sodium fluoride react to form strontium fluoride and sodium chloride, according to the reaction shown.
SrCl2(aq)+2NaF(aq)⟶SrF2(s)+2NaCl(aq)
What volume of a 0.190 M NaF solution is required to react completely with 417 mL of a 0.400 M SrCl2 solution?
How many moles of SrF2 are formed from this reaction?
A student needs to prepare 50.0 mL of a 1.30 M aqueous H2O2 solution. Calculate the volume of 5.1 M H2O2 stock solution that should be used to prepare the solution.
The pressure 80.0 m under water is 886 kPa.
What is this pressure in bar and Torr?
Consider the neutralization reaction
2HNO3(aq)+Ba(OH)2(aq)⟶2H2O(l)+Ba(NO3)2(aq)
A 0.110 L sample of an unknown HNO3 solution required 51.1 mL of 0.150 M Ba(OH)2 of
0.150 M Ba(OH)2 for complete neutralization. What is the concentration of the
HNO3 solution?
A student has 8.85 g of zinc powder, 1.95 L of a 2.00 M
calcium nitrate solution, and 1.35 L of a 3.10 M lead(II) nitrate solution.
Write the chemical reaction that occurs between the two reacting species. Include physical states.
What volume of the solution is needed to completely react all 8.85 g of zinc powder?
Calculate the molarity of the Zn2+ ions in solution after the reaction.
Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction.
SnBr4(aq)+2Na2S(aq)⟶4NaBr(aq)+SnS2(s)
Suppose a student adds 49.0 mL of a 0.452 M solution of SnBr4 to 44.8 mL of a 0.153 M solution of Na2S.
Identify the limiting reactant.
Calculate the theoretical yield of SnS2
The student recovers 0.347 g SnS2. Calculate the percent yield of
SnS2 that the student obtained.
.
Ammonia (NH3, MM 17.031 g/mol) and hypobromite (OBr−) react according to the following chemical reaction.
2NH3+3OBr−⟶N2+3Br−+3H2O
Suppose 0.809 g of ammonia reacts with 37.2 mL of a hypobromite solution. Calculate the concentration of the hypobromite solution.
An initial volume of 3.7 L of a gas are maintained at constant pressure while being cooled from 95 ºC to 22 ºC. What is the new volume of the gas?
Consider the following reaction.MgCl
MgCl2(aq)+2NaOH(aq)⟶Mg(OH)2(s)+2NaCl(aq)
A 127.0 mL solution of 0.132 M MgCl2 reacts with a 33.22 mL solution of 0.664 M NaOH to produce Mg(OH)2 and NaCl.
Caclulate the mass of Mg(OH)2 that can be produced.
The actual mass of Mg(OH)2 isolated was 0.501 g. Calculate the percent yield of Mg(OH)2
.
