1. Suppose that you decompose 20.07 g of Ni2O3NiX2OX3, which has a molar mass of 165.39...
1. Suppose that you decompose 20.07 g of Ni2O3NiX2OX3, which has a molar mass of 165.39 g/mol, into nickel and oxygen.
2Ni2O3(s)⟶4Ni(s)+3O2(g)2NiX2OX3(s)⟶4Ni(s)+3OX2(g)
After completing the decomposition, you have 9.56 g of solid NiNi, which has a molar mass of 58.963 g/mol.
What is the percent yield of your decomposition?
2. Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table.
| Mass of weigh boat | 2.147 g |
|---|---|
| Mass of weigh boat and sample | 6.096 g |
What is the mass of the solid sample?
3.
Nitrogen and hydrogen react to form ammonia according to the reaction shown.
3H2(g)+N2−⇀↽−2NH33HX2(g)+NX2↽−−⇀2NHX3
What is the percent yield if 19.03 g nitrogen and 10.89 g hydrogen react to form 5.24 g of ammonia?
4.Suppose you separate a 2.55 g mixture of sand and salt and recover 1.60 g of salt. What is the percent by mass of salt in the mixture?
Homework Answers
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1. Suppose that you decompose 20.07 g of Ni2O3NiX2OX3, which has
a molar mass of 165.39...
Question 8 4 pts Nitrogen and hydrogen react to form ammonia according to the reaction shown:...
Question 8 4 pts Nitrogen and hydrogen react to form ammonia according to the reaction shown: 3 H2(g) + N2(g) + 2NH3(g) What is the percent yield if 19.20 g nitrogen and 10.81 g hydrogen react to form 5.24 g of ammonia? Question 9 2 pts Suppose you separate a 2.15 g mixture of sand and salt and recover 1.55 g of salt. What is the percent by mass of salt in the mixture?
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a...
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table. Mass of weigh boat 3.117 g Mass of weigh boat and sample 9.405 g What is the mass, in grams, of the solid sample? Question 7 2 pts Sulfuric acid, H2SO4, is an important industrial chemical (typically used for fertilizers and making of many other chemicals), typically synthesized in a multi-step process....
Question 5 Status: Not yet answered | Points possible: 1.00 Suppose that you decompose 24.45 g...
Question 5 Status: Not yet answered | Points possible: 1.00 Suppose that you decompose 24.45 g of Ni2O3, which has a molar mass of 165.39 g/mol, into nickel and oxygen. 2 Ni203 (s) + 4 Ni (s) + 3 02 (g) After completing the decomposition, you have 9.14 g of solid Ni, which has a molar mass of 58.963 g/mol. What is the percent yield of your decomposition? Answer:
A sample weighing 3.099 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3...
A sample weighing 3.099 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The A1203 does not react. If the sample residue (the solid species remaining after the reaction) weighs 2.498 g, what is the mass fraction of Fe2O3 in the original sample? Number g FeO g original sample
What would be for the mol reacted,, mol NH4X in sample, and yhr average molar mass?...
What would be for the mol reacted,, mol NH4X in sample, and yhr
average molar mass?
CALCULATIONS A. NaOH Preparation: Approximate molarity of NaOH 0.48 M B. NaOH Standardization: Trial # Mass of KHP E 1.7249 1.9569 1.8799 Volume of NaOH 18.58 L 20.58mLihat 19.71 mL Molarity of NaOH 0.4544 M 0.4654M 0. 3 M 0.4668M Average molarity of NaOH: 0.4668 M 0.4622 M C. Molar Mass of NH X Salt 1. Volume of NaOH 0.025 0.025 0.025L 2. Molarity...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 2.00 L. The salt decomposes when heated, the unbalanced equation for the decomposition reaction is shown below: Pb(NO3)2(s) → PbO(s) + NO2(g) + O2(g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 303 K? Assume the PbO(s) takes up negligible volume.
Question 4 Status: Not yet answered Points possible: 1.00 Consider the balanced equation of KI reacting...
Question 4 Status: Not yet answered Points possible: 1.00 Consider the balanced equation of KI reacting with Pb(NO3), to form a precipitate. 2 KI (aq) + Pb(NO3)2 (aq) + Pbl (8) + 2 KNO3(aq) What mass of Pbl, can be formed by adding 0.489 L of a 0.364 M solution of KI to a solution of excess Pb(NO3)2? Answer: Question 5 Status: Not yet answered Points possible: 1.00 Suppose that you decompose 24.45 g of Ni 03, which has a...
Question 7 (2 points) Nitrogen gas reacts with hydrogen gas to produce ammonia (NH3) (g). Suppose...
Question 7 (2 points) Nitrogen gas reacts with hydrogen gas to produce ammonia (NH3) (g). Suppose 2.900 g of nitrogen gas are reacted with 3.950 g of hydrogen gas. Calculate the maximum mass in grams of ammonia that can be produced. N2(g) + 3H2(g) → 2NH3(g) Report your answer to 2 decimal places. There are no marks for units. Your Answer: Answer units Question 8 (2 points) If 15.45 g of Al(s) is reacted with 10.44 g of solid iodine,...
1) Sample of nitrogen gas, N2 weighs 15.3 g. How many molecules N2 and how many...
1) Sample of nitrogen gas, N2 weighs 15.3 g. How many molecules N2 and how many atoms of N are present in this sample? 1a)A mixture of sand and salt is found to be 57 percent NaCl by mass. How many moles of NaCl are in 47 g of this mixture? 1b) What is the mass of 4.6*10^23 of ammonia? 1c) A water solution of sulfuric acid has a density of 1.67 g/mL and is 65 percent H2SO4 by mass....
please answer 1 & 2 thank you 1. limiting Reactant - Mass to Mass: Perform two...
please answer 1 & 2 thank you 1. limiting Reactant - Mass to Mass: Perform two calculations to determine the limiting reactant and amount of product produced. Hydrogen cyanide, a highly toxic compound, is made by the following reaction: 2 CH4(g) + 2 NH3(g) + 3 O2(g) → 2 HCN(g) + 6 H2O(g) What is the limiting reagent with respect to HCN production if 45.4 g of O2 are added to 23.8 g of NH3? (assume CH4 is in excess)...
Question 8 4 pts Nitrogen and hydrogen react to form ammonia according to the reaction shown: 3 H2(g) + N2(g) + 2NH3(g) What is the percent yield if 19.20 g nitrogen and 10.81 g hydrogen react to form 5.24 g of ammonia? Question 9 2 pts Suppose you separate a 2.15 g mixture of sand and salt and recover 1.55 g of salt. What is the percent by mass of salt in the mixture?
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table. Mass of weigh boat 3.117 g Mass of weigh boat and sample 9.405 g What is the mass, in grams, of the solid sample? Question 7 2 pts Sulfuric acid, H2SO4, is an important industrial chemical (typically used for fertilizers and making of many other chemicals), typically synthesized in a multi-step process....
Question 5 Status: Not yet answered | Points possible: 1.00 Suppose that you decompose 24.45 g of Ni2O3, which has a molar mass of 165.39 g/mol, into nickel and oxygen. 2 Ni203 (s) + 4 Ni (s) + 3 02 (g) After completing the decomposition, you have 9.14 g of solid Ni, which has a molar mass of 58.963 g/mol. What is the percent yield of your decomposition? Answer:
A sample weighing 3.099 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The A1203 does not react. If the sample residue (the solid species remaining after the reaction) weighs 2.498 g, what is the mass fraction of Fe2O3 in the original sample? Number g FeO g original sample
What would be for the mol reacted,, mol NH4X in sample, and yhr
average molar mass?
CALCULATIONS A. NaOH Preparation: Approximate molarity of NaOH 0.48 M B. NaOH Standardization: Trial # Mass of KHP E 1.7249 1.9569 1.8799 Volume of NaOH 18.58 L 20.58mLihat 19.71 mL Molarity of NaOH 0.4544 M 0.4654M 0. 3 M 0.4668M Average molarity of NaOH: 0.4668 M 0.4622 M C. Molar Mass of NH X Salt 1. Volume of NaOH 0.025 0.025 0.025L 2. Molarity...
Question 4 Status: Not yet answered Points possible: 1.00 Consider the balanced equation of KI reacting with Pb(NO3), to form a precipitate. 2 KI (aq) + Pb(NO3)2 (aq) + Pbl (8) + 2 KNO3(aq) What mass of Pbl, can be formed by adding 0.489 L of a 0.364 M solution of KI to a solution of excess Pb(NO3)2? Answer: Question 5 Status: Not yet answered Points possible: 1.00 Suppose that you decompose 24.45 g of Ni 03, which has a...
Question 7 (2 points) Nitrogen gas reacts with hydrogen gas to produce ammonia (NH3) (g). Suppose 2.900 g of nitrogen gas are reacted with 3.950 g of hydrogen gas. Calculate the maximum mass in grams of ammonia that can be produced. N2(g) + 3H2(g) → 2NH3(g) Report your answer to 2 decimal places. There are no marks for units. Your Answer: Answer units Question 8 (2 points) If 15.45 g of Al(s) is reacted with 10.44 g of solid iodine,...
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