Homework Answers
You mix 125 mL of 0.270 M CsOH with 50.0 mL of 0.675 M HF in...
You mix 125 mL of 0.270 M CsOH with 50.0 mL of 0.675 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 20.70 °C before mixing to 23.82 °C after the reaction. CsOH (aq) + HF (aq) ---> CsF (aq) + H2O (l) What is the enthalpy of reaction per mole of CsOH ? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g...
You mix 176 mL of 0.310 M CsOH with 76 mL of 0.6458 M HF in...
You mix 176 mL of 0.310 M CsOH with 76 mL of 0.6458 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 35.9 C degree before mixing, to 43.8 C degree after the reaction. CsOH (aq) + HF (aq) arrow CsF (aq) + H2O (l) What is the heat [q] for this reaction per mole of CsOH? Assue the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions...
You mix 142 mL of 0.254 M CSOH with 130.0 mL of 0.2774 M HF in...
You mix 142 mL of 0.254 M CSOH with 130.0 mL of 0.2774 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.10°C before mixing, to 22.90°C after the reaction. CsOH (aq) + HF (aq) --> CsF (aq) + H20 (1) What is the heat [g] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions are 4.18 J/(g.K). 90.5...
You mix 2.58 mL of 0.613 M CsOH with 510.0 mL of 0.3101 M HF in...
You mix 2.58 mL of 0.613 M CsOH with 510.0 mL of 0.3101 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.50 degree C before mixing, to 23.50 degree C after the reaction. CsOH (aq) + HF (aq) rightarrow CsF (aq) + H_2O (l) What is the heat [q] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions...
[References] INTERACTIVE EXAMPLE Using a Coffee-Cup Calorimeter Suppose you place 0.0500 g of magnesium chips in...
[References] INTERACTIVE EXAMPLE Using a Coffee-Cup Calorimeter Suppose you place 0.0500 g of magnesium chips in a coffee cup calorimeter and then add 100.0 ml. of 1,00 M HC. The reaction that occurs is Mg(s) + 2 HCl(aq)-H2(g) + MgCl(aq) The temperature of the solution increases from 23.41 °C (296.56 K) to 25.66 °C (298.81 K) What is the enthalpy change for the reaction per mole of MR? Assume a specific heat capacity of the solution is 4.20 J/gK and...
Assume that 100.0 mL of 0.200 M CsOH and 50.0 mL of 0.400 M HCl are...
Assume that 100.0 mL of 0.200 M CsOH and 50.0 mL of 0.400 M HCl are mixed in a calorimeter. The solutions start out at 22.50 ∘C, and the final temperature after reaction is 24.28 ∘C. The densities of the solutions are all 1.00 g/mL, and the specific heat of the mixture is 4.2J/(g⋅∘C). Calculate the energy which releases in the process. Express your answer using four significant figures.
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 22.8*C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.53/°C. Density Aqueous Solution - 1.00 g/mL Specific Heat of water = 4.184J/g•°C a. What is the total amount of heat evolved in this reaction? b. If 148 mmol of the...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 23.9°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.6J/°C. Density Aqueous Solution = 1.00 g/ml Specific Heat of water = 4.184 J/g °C Hide a. What is the total amount of heat evolved in this reaction? NG 3 b....
you mix 100.0ml of 0.200M CsOH and 50.0ml of 0.400M HCl in a calorimeter. write a...
you mix 100.0ml of 0.200M CsOH and 50.0ml of 0.400M HCl in a calorimeter. write a balanced equation. The initial temperature of both solutions was 22.50 degree Celsius, and the final temperature was 24.28 degree Celsius. calculate the change of heat for this reaction in kj/mol of CsOH. assume the densities of the solutions are both 1.00g/ml and the specific heats are both 4.184 j/gC please show work
In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M...
In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M HCl are mixed to yield the following reaction: Ag+(aq) + Cl-(aq) --> AgCl(s) The two solutions were initially at 22.6°C and the final temp is 23.4°C. Assume that the final solution has a mass of 10.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate delta for the reaction in kJ/mole of AgCl formed.
You mix 142 mL of 0.254 M CSOH with 130.0 mL of 0.2774 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.10°C before mixing, to 22.90°C after the reaction. CsOH (aq) + HF (aq) --> CsF (aq) + H20 (1) What is the heat [g] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions are 4.18 J/(g.K). 90.5...
You mix 2.58 mL of 0.613 M CsOH with 510.0 mL of 0.3101 M HF in a coffee cup calorimeter, and the temperature of both solutions rises from 20.50 degree C before mixing, to 23.50 degree C after the reaction. CsOH (aq) + HF (aq) rightarrow CsF (aq) + H_2O (l) What is the heat [q] for this reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL and the specific heats of the solutions...
[References] INTERACTIVE EXAMPLE Using a Coffee-Cup Calorimeter Suppose you place 0.0500 g of magnesium chips in a coffee cup calorimeter and then add 100.0 ml. of 1,00 M HC. The reaction that occurs is Mg(s) + 2 HCl(aq)-H2(g) + MgCl(aq) The temperature of the solution increases from 23.41 °C (296.56 K) to 25.66 °C (298.81 K) What is the enthalpy change for the reaction per mole of MR? Assume a specific heat capacity of the solution is 4.20 J/gK and...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 22.8*C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.53/°C. Density Aqueous Solution - 1.00 g/mL Specific Heat of water = 4.184J/g•°C a. What is the total amount of heat evolved in this reaction? b. If 148 mmol of the...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 23.9°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.6J/°C. Density Aqueous Solution = 1.00 g/ml Specific Heat of water = 4.184 J/g °C Hide a. What is the total amount of heat evolved in this reaction? NG 3 b....
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