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2. What is the molar concentration of a AgNO3 solution if 16.35-mL react with:
a) 0.3017-g KIO3 ANSWER: 0.08623 M AgNO3
b) 12.33 mL of 0.02149 M K4Fe(CN)6 ANSWER: 0.06482 M AgNO3
Molar masses: KIO3 = 214.0 K4Fe(CN)6 = 368.4
a) 0.3017-g KIO3 ANSWER: 0.08623 M AgNO3
b) 12.33 mL of 0.02149 M K4Fe(CN)6 ANSWER: 0.06482 M AgNO3
Molar masses: KIO3 = 214.0 K4Fe(CN)6 = 368.4
A student was assigned to recrystallize an impure sample of benzoic acid. he obtained 3.2g of pure benzoic acid from 5g of the sample. calculate the % yield of recrystallized (pure) benzoic acid.
A balloon is filled with 10 L of air at a pressure of 1400 torr. What is the pressure of the balloon if the volume is changed to 5 L?
How much energy (in joules) will be given off from the following reaction, if 3.0g of sodium reacts with 1.2g of nitrogen in the following reaction? 2Na+ N2 ——> 2NaN3 delta H= -42.7kJ
Iodine dissolves in an aqueous solution of iodine ion's to form triiodide .this ion's consist of one one iodine atom bonded to two others. Describe the bonding of triiodide in terms of valance bond theory ?
Explain wind powered electrolysis
CH4+2H2O+heat <--> CO2+4H2
A test reaction is done starting with only methane and excess water in the autoclave. If the initial concentration of methane is 0.112 mol/L, and the methane concentration at equilibrium is 0.017 mol / L, then the equilibrium concentration of hydrogen is?
(two digit answer)
A test reaction is done starting with only methane and excess water in the autoclave. If the initial concentration of methane is 0.112 mol/L, and the methane concentration at equilibrium is 0.017 mol / L, then the equilibrium concentration of hydrogen is?
(two digit answer)
From the following dissociation question:
Al2(SO4)3 ----> 2Al^3 + 3SO4^2-
What will be the concentration of the CATION present if 25.5g aluminum sulfate is dissolved in 1.00L of water?
Al2(SO4)3 ----> 2Al^3 + 3SO4^2-
What will be the concentration of the CATION present if 25.5g aluminum sulfate is dissolved in 1.00L of water?
In a calorimeter made from Iron 38.2 grams of (iodine) I2 (s) was produced by the decomposition of (hydrogen iodide) HI (g) from the data below, calculate the molar enthalpy change of I2 (s) in this reaction.
Mass of (iodine) I2(s)-----38.2 g
Mass of iron calorimeter------70.0 g
the volume of H2O(L)--------100 mL
Initial temperature--------6.0 celsius
Final temperature-------23.8 celsius
Mass of (iodine) I2(s)-----38.2 g
Mass of iron calorimeter------70.0 g
the volume of H2O(L)--------100 mL
Initial temperature--------6.0 celsius
Final temperature-------23.8 celsius
calculate the molar enthalpy of the combustion of butane if 1.22 g of the fuel increased the temperature of a tin can calorimeter (22.5 g of tin and 200 mL of water) by 8.30 celsius
