Get college assignment help at uniessay writers A system expands in volume from 2.0 L to 24.5 L at constant temperature. Calculate the work (w) if the expansion occurs against a constant pressure of 5.00 atm.
Would you just do number 6 and number 9 please?
11. A student found that her mixture was 13% NH4, 18% NaCl, and 75% SiO2. Assuming that her calculations are correct, what did she most likely do incorrectly in her experiment?
Calculate the new temperature in degress Celsius when pressure is changed with na nd V constant. A tank of helium gas with a pressure of 250 torr at 0 degrees celsius is heated to give a pressure of 1500 torr
True or False: When the reaction 2SO2(g) O2(g) 2SO3(g) takes place in the presence of NO(g), the rate is increased. This system involves a homogeneous catalyst.
Predict the direction that equilibrium will shift for each change in the components of the following reaction C(s) H2O heat CO(g) H2(g) ( Reversible arrow) a. Adding heat b. Adding CO(g) c. removing H2 (g) d. Adding H2O(g)
How many moles of HNO3 are present in 35.0 mL of a 2.20 M solution of nitric acid?
1. How many moles of Ni2(SO4)3 are in 102.3 g of the compound? 2.How many grams of NaCl are in 750.0 mL of a solution which is 0.150 M? 3.Determine the empirical formula of a compound which percent composition is 39.10% C, 8.700% H, and 52.20% O. 4.How many grams of Bi(s) are produced from 352.0 g Bi2O3(s) according to the balanced chemical equation shown: Bi2O3(s) 3C(s) → 2Bi(s) 3CO(g) 5. 12.0 grams of aluminum react with 54.0 grams of iron (III) oxide. If 19.5 grams of iron were obtained, what was the percent yield of the reaction? 2Al(s) Fe2O3(s) → 2Fe(s) Al2O3(s) 6. How many mL of 0.500 M acetic acid are required to react with 250.0 mL of barium hydroxide solution which is 0.250 M according to the following reaction: 2CH3COOH(aq) Ba(OH)2(aq) → Ba(CH3COO)2(aq) 2H2O(l)
A stock solution is prepared by adding 26 mL of 0.4 M Na3PO4 to enough water to make 76 mL. What is the PO43- concentration of 50 mL of the stock solution
Assuming the density of a 5% acetic acid solution is 1.0 g/ml, determine the volume of the acetic acid solution necessary to neutralize 25.0 ml of .10M NaOH. Also record this calculation on your report sheet.
Get college assignment help at uniessay writers The solubility of Ce(IO3)3 in a 0.20 M KIO3 is 4.4 multiplied by 10-8 mol/L. Calculate Ksp for Ce(IO3)3.
You have a solution that is buffered at pH = 2.0 using H3PO4 and H2PO4 (pKa1 = 2.12; pKa2 = 7.21; pKa3 = 12.68). You decide to titrated this buffer with a strong base. 15.0 mL are needed to reach the first equivalence point. What is the total volume of base that will have been added when the second equivalence point is reached? 1. 30 mL 2. A second equivalence point in the titration will never be observed. 3. > 30 mL 4. < 30 mL
how many grams of solute are in 448 mL of 0.800 M Na2SO4 solution
freezing point 0.00°C boiling point 100.00°C Kf 1.86°C/m Kb 0.512°C/m What is the boiling point of the solution in which you are going to cook spaghetti if it contains 53.0 g of NaCl dissolved in 1.00 L of water? Assume the density of water is 1.00 g/mL
What volumes of 0.50M HNO2 and 0.50M NaNO2 must be mixed to prepare 1.00L of a solution buffered at pH 3.55? (Ka of HNO2 = 4.0 x 10^-4).
A 31.43 ml volume of .108M NaOH is require to reach the phenolphthalein endpoint in the titration of a 4.441g sample of vinegar. Calcute the percent acetic acid in the vinegar.
“A 31.43 ml volume of .108M NaOH is require to reach the phenolphthalein endpoint in the titration of a 4.441g sample of vinegar. Calcute the percent acetic acid in the vinegar.”
lemon juice has a pH of about 2.5 assuming that the acidity of lemon juice is due solely to citric acid, that citirc acid is a monoprotic acid,and that the density of lemon juice is 1.0 g/ml, then the citric acid concentraion calculates to .5% by mass. estimate the volume of .0100M NaOH required to neutralize a 3.71 g sample of lemon juice. the molar mass of citric acid is 190.12 g/mol
Indicators can be used to estimate the pH value of soultions. To determine the pH of a 0.01M weak acid (HX), a few drops of three different indicators are added to separate portions of HX. The resulting colors of the HX solution are below. What is the approximate pH and Ka value of 0.01M HX? Indicator#1 (HIn): Bromphenol blue Color of HIn : Yellow Color of In- : Blue pKa of HIn: 4.0 Color of 0.01M HX: Blue Indicator#2 (HIn): Bromcresol pruple Color of HIn : Yellow Color of In- : Purple pKa of HIn: 6.0 Color of 0.01M HX: Yellow Indicator#3 (HIn): Bromcresol green Color of HIn : Yellow Color of In- : Blue pKa of HIn: 4.8 Color of 0.01M HX: Green
Solid MX dissolves in water but only limited amount. MX(s) M (aq) X- (aq) The solubility of MX in a solution buffered to pH=2.00 is only 3.17 x 10^-8M. It turns out that HX is a weak acid. (Ka= 1.00 x 10^-15M) (a) Given that, would you expect the solubility of MX in pure water to be bigger or smaller than that is in 2.00 pH buffer? Why? (b) Calculate the Ksp for MX.
When 0.052 mol of aluminum sulfate are dis- solved in enough water to make 179 milliliters of solution, what is the molar concentration of aluminum ions?
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