Reference no: EM132669748
1. When an aqueous solution of Na2SO4 is mixed with an aqueous solution of CaCl2, a white precipitate form.
a. Write the balanced molecular equation (including all products and phases) for this reaction.
b. Write the complete ionic equation for this reaction.
c. Write the net ionic equation for this reaction.
2. Consider the following balanced chemical reaction:
3 BaCl2 (aq) + 2 (NH4)3PO4 (aq) -----> 6 NH4Cl (aq) + Ba3(PO4)2 (s)
How many mL of a 2.03 M (NH4)3PO4 solution are needed to completely react with 273.9 mL of a 1.79 M BaCl2 solution?
3. a) Determine the theoretical yield of HCI in grams if 59.8 g of BCI3 and 36.6 of H20 are reacted according to the following balanced reaction. Molar mass is BCI3 = 117.16 g/mol.
b) If the actual yield is 38.0 g what is the percent yield?
4. Consider the reaction:
2 HCI (aq) + MgCO3 (s) -----> CO2 (g) + H20 (I) + MgCl2 (aq)
What volume of CO2 gas (in L) at 0.750 atm and 26°C is produced by reacting of 10.0 g of MgCO3 (s)?
5. A 0.586 g sample of a compound occupies 266 mL at 298 K and 1.25 atm. What is the molar mass if the compound?
6. SO2 (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. Calculate the total pressure in the container in atm.
7. Determine the density of NH3 gas at 435°C and 1.00 atm.
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: 1. When an aqueous solution of Na2SO4 is mixed with an aqueous solution of CaCl2, a white precipitate form.
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