# A small crystal has a mass of 7.03 mg

1. A small crystal has a mass of 7.03 mg and is shaped like a cylinder with a height of 5.17 in and a radius of 34.8 mm. What is the density of the solid in g/cm3?

1. If the price of gasoline is \$2.03 dollars/gal, what is its price in Euros per liter, given the exchange rate is \$1.20 per Euro.

1. Convert 316.25 K into o Convert 14.7 oC into oF.

1. Provide the names for the following compounds

1. NaF
2. N2O4
3. KNO3
4. MgSO4
5. NH3
6. Cr(NO2)

1. Provide formulas for the following compounds

1. Calcium iodide
2. Aluminum sulfide
3. Lithium carbonate
5. Manganese (II) dichromate

1. Name These Acids:
2. H2S b. HF c. H2CO3                                                       d. HNO2

1. Write formulas for the following acids:
2. Hydroiodic acid b. Hydrophosphoric acid c. Nitric acid                                    d. Chromic acid
3. How many neon atoms are there in 2.585 mol of neon?
4. What is the mass in grams of 0.2338 mol of Titanium?
5. How many moles of barium are there in 42.9g of barium?
6. Molar mass of Copper (II) Nitrate = ___________________g/mole
7. Balancing Equations
8. a) ____ Na3PO4 + ____ Ba(OH)2 à ____ NaOH + ____ Ba3(PO4)2

b) ____ CaF2 + ____ Li2CO3 à ____ CaCO3 + ____ LiF

c)         ____ Ba3N2 + ____ PtF2 à ____ BaF2 + ____ Pt3N2

9. Write chemical equations for the following reactions.
a) Rubidium reacts with bromine to form Rubidium bromide.
10. b) Iron (II) sulfide and water vapor are formed when hydrogen sulfide and iron (II) hydroxide react.

c) Calcium reacts violently with water to produce calcium hydroxide and hydrogen.

1. Stoichiometry

2. If 2.98 moles of C are reacted with an excess of Cu2O, what mass of CO would be produced?
3. If 43.6 g of Co(NO3)3 are reacted with an excess of (NH4)2S, how many moles of NH4NO3 would be produced?
4. If 19.6g of FeS is added to 44.8g of HCl and allowed to react, what is the theoretical yield of H2S? If 6.20 g of H2S were obtained in the lab, what is the percent yield?

1. 947 g of chromium (III) chloride combined with 1.13 g of copper (II) sulfate to produce 0.154 g of copper (II) chloride. What is the percent yield of this reaction?

2. Solutions and Solubility

Label the following compounds as soluble or insoluble in water:

1. NaCl
2. CaSO4
3. AgNO3
4. PbCl2
5. Li2S
6. MgCO3

1. Calculate the molar concentration, M, of a solution of a sample with 0.271 moles in 55.0 L or solution.

1. Calculate the pH of a 0.543M HCl solution.

1. Write the net ionic equations for the following reactions. Be sure to show all physical states for reactants and products for each equation type:
2. ___KBr +    ___Pb(NO3)2             à     ___PbBr2            +    ___KNO3

1. ___Fe(C2H3O2)2 +    ___Li2SO4                 à     ___FeSO4            +    ___LiC2H3O2
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