Practice Test for 6.1-6.3 1. Complete the following molarity calculations: a. What is the molarity of a solution containing 25.3 grams of copper (II) chloride dissolved in 140 mL of water? b. How many grams of sodium hydroxide are needed to make 2 L of a 0.05 M solution?
4 Calculate the molar mass of these compounds: (relative atomic masses: H = 1; N = 14; O = 16; S = 32; Cu = 64; Br = 80; Pb = 207) (a) copper nitrate, Ca(NO3)2 (b) lead bromate, Pb(BrO3)2 (c) ammonium sulfate, (NH4)2SO4 5 The equation for the complete combustion of methane is shown below. CH4 + 2O2 → CO2 + 2H2O When 80 g of methane is completely combusted, 220 g of carbon dioxide and 180 g of water are formed. (a) Why is the mass of carbon dioxide formed greater than the mass of methane burnt? (b) Calculate the mass of oxygen that reacted. (c) Calculate the mass of water formed when 20 g of methane undergoes complete combustion.
What volume of concentrated (18.0 M) sulfuric acid would be required to make each of the following? a. 1.25 L of 6.00 M solution Mconc x Vconc = Mdil x Vdil (18.0 M) x (Vconc) = (6.00 M) x (1.25 L) Vconc=0.417 L b. 575 mL of 0.100 M solution Mconc x Vconc = Mdil x Vdil (18.0 M) x (Vconc) = (0.100 M) x (0.575 L) Vconc=0.00319 L Acid-Base Titrations 5. Calculate the molarity of an HCl solution if 20.0 mL of it requires 33.2 mL of 0.150 M NaOH for neutralization.
6.02 x 1023 atoms C. 6.02 x 1023 ions B. 6.02 x 1023 grams D. 6.02 x 1023 molecules 5. What ts the correct unit of a formula weight? A. gram B mol C. gram/mol D. mole/gram 6. How many individual atoms are there in 250 grams of O2?
If 63% of the mass of pyrolusite is due to manganese, what is the empirical formula of pyrolusite? • MnO • Mn2O • Mn2O2 • MnO2 4. A compound with an empirical formula of C2H4Br has a molar mass of 215.90 g/mol. What is the molecular formula? • C4H8Br2 • C2H4Br • CHBr • C6H12Br3 5.
1) Calculate the number of moles in each of the following solutions:- a) 2.0 dm3 of 0.050 mol.dm-3 hydrochloric acid b) 50 dm3 of 5 mol.dm-3 sulfuric acid c) 10 cm3 of 0.25 mol.dm-3 potassium hydroxide [3] 2) Calculate the volume in cm3 of each solution that contains the following numbers of moles:- a) 0.00500 moles of NaOH with concentration 0.100 mol.dm-3 b) 1.00×10-5 moles of HCl with concentration 0.0100 mol.dm-3 c) 9.25×10-3 moles of KCl with concentration 0.250 mol.dm-3 [3] 3) Find the concentrations of the following solutions in both mol.dm-3 and g.dm-3:- a) 0.400 moles of HCl in 2.00 dm3 of solution b) 12.5 moles of H2SO4 in 5.00 dm3 of solution c) 1.05g of NaOH in 500 cm3 of solution [6] 4) In a titration, 25.0 cm3 of a solution of sodium hydroxide required 18.80 cm3 of hydrochloric acid of concentration 0.0500 mol.dm-3 for neutralisation. Find the concentration of the sodium hydroxide in both mol.dm-3 and g.dm-3. [3] NaOH + HCl ( NaCl + H2O 5) Calculate the volume of 0.05 mol.dm-3 potassium hydroxide solution that is required to react exactly with 25.0 cm3 of 0.0150 mol.dm-3 nitric acid. [2] HNO3 + KOH ( KNO3 + H2O 6) In a titration, 20.0 cm3 of barium hydroxide solution required 28.60 cm3 of sulfuric acid of concentration 0.0250 mol.dm-3 for neutralisation. Find the concentration of the barium hydroxide in both mol.dm-3 and g.dm-3.
CHEM 10050 Problem Set #3 Name_________________ 1. Calculate the molarity of normal saline (0.90% w/w NaCl) given the density of this solution to be 1.05 g/ml. Assume 100 g solution. Then: [pic] [pic] [pic] [pic] 2. Calculate the molarity of an aqueous solution resulting when 275 ml of 3.15 M glucose is diluted with 150 ml of water.
The RQ or RER was 0.87. Based on Table 5.1(Kenney,Wilmore, &Costill, 2012; Physiology of Sport and Exercise(5th ed.) The ratio indicates that roughly 68% of the kcal that the subject was using came from carbohydrates and the remaining 32% of the kcal came from fat. During the 50W stage the volume of carbon dioxide was 2.2L/min and the volume of oxygen was 2.9L/min. The RQ was 0.79, which indicates that the 33% of the kcal that the subject was using came from carbohydrates and that 67% of the kcal came from fat.
Obtain between 0.1 to 0.2g of zinc metal. Making Predictions 2. Determine the amount of 6.0M HCl that will be needed to react completely with the zinc. 3. Determine the volume of hydrogen gas that will be generated by the reaction.
1. A solution containing 1.000M acetic acid (CH3COOH) and 1.000M ethyl alcohol (CH3CH2OH) at 150oC produced 0.171 mole/liter of the product ethyl acetate (CH3COOCH2CH3) when equilibrium was established. Determine Kc for the reaction. CH3COOH (aq) + CH3CH2OH (aq) CH3COOCH2CH3 (aq) + H2O (l) 2. Using the equilibrium constant from above, calculate the equilibrium concentrations of all the compounds in the reaction if 1.000M acetic acid is reacted with 2.000M ethyl alcohol.