I tried everything can't find out how to do these two problems. Thanks to everyone that attempts to help me its a problem that's going to be in my final exam.
1.) 250 mL of a 0.5 M cesium sulfate is used in a single replacement reaction with calcium. What mass of the element product will be formed?
2.) Copper (III) nitrate undergoes a single replacement reaction with magnesium. If the reaction starts with 125 mL of 1.2 M solution of copper (III) nitrate, what mass of solid product will be formed?
1.) 250 mL of a 0.5 M cesium sulfate is used in a single replacement reaction with calcium. What mass of the element product will be formed?
2.) Copper (III) nitrate undergoes a single replacement reaction with magnesium. If the reaction starts with 125 mL of 1.2 M solution of copper (III) nitrate, what mass of solid product will be formed?
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Cs2SO4 + Ca --> CaSO4 + 2Cs.....as an aside, Ca will not replace Cs in Cs2SO4 because Ca is NOT more reactive than Cs. therefore, a reaction will not occur.
anyway
0.25L x 0.5M = 0.125moles Cs2SO4, 1:1 ratio with Cs so 0.125moles Cs produced
0.125moles Cs x 132.9g/mole = 16.6g produced
2. there is no copper III nitrate, it is either copper I or copper II
Cu(NO3)2 + Mg --> Mg(NO3)2 + Cu.....Mg is more reactive than Cu so it will replace Cu in the compound.
0.125L x 1.2M Cu(NO3)2 = 0.15moles Cu(NO3)2 present, 1:1 ratio with Cu so 0.15moles Cu produced.
0.15moles Cu x 63.5g/mole = 9.5g produced
anyway
0.25L x 0.5M = 0.125moles Cs2SO4, 1:1 ratio with Cs so 0.125moles Cs produced
0.125moles Cs x 132.9g/mole = 16.6g produced
2. there is no copper III nitrate, it is either copper I or copper II
Cu(NO3)2 + Mg --> Mg(NO3)2 + Cu.....Mg is more reactive than Cu so it will replace Cu in the compound.
0.125L x 1.2M Cu(NO3)2 = 0.15moles Cu(NO3)2 present, 1:1 ratio with Cu so 0.15moles Cu produced.
0.15moles Cu x 63.5g/mole = 9.5g produced