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.
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Assume that 100.0 mL of 0.200 M CsOH and 50.0 mL of 0.400 M HCl
are...
You mix 125 mL of 0.180 M CsOH with 50.0 mL of 0.450 M HF in...
You mix 125 mL of 0.180 M CsOH with 50.0 mL of 0.450 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.38 °C after the reaction. CsOH(a) +HF(a)-CaF a)+H20() 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 Jg K. Enthalpy of reaction- siol
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 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
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
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...
Suppose you mix 200.0 mL of 0.200 M RbOH(aq) with 100.0 mL of 0.400 M HBr...
Suppose you mix 200.0 mL of 0.200 M RbOH(aq) with 100.0 mL of 0.400 M HBr (aq) in a coffee cup calorimeter. The initial temperature of each of the two solutions was 24.40°C and after mixing the temperature of the solution was 26.18°C. Assume the specific heat capacity of the solution is the same as water, 4.18J/(g- C) and the density of the solution is 1.0 g/mL. What is AH° (in kJ) for the reaction shown below? (Enter your answer...
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...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HCl in a calorimeter. Both solutions were initially at 35.00°C and the final temperature of the resulting solution was recorded as 37.00°C. Write a balanced chemical reaction for the neutralization reaction between aqueous NaOH and HCl, determine the number of moles of water formed in this reaction, and calculate the overall heat change of the solution. Assume 1) that no heat is...
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each...
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each at 24.00°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 26.65 °C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1.00 g/mL and specific heat capacity of 4.18 J/(g•C) How much heat did the reaction release?
You mix 125 mL of 0.180 M CsOH with 50.0 mL of 0.450 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.38 °C after the reaction. CsOH(a) +HF(a)-CaF a)+H20() 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 Jg K. Enthalpy of reaction- siol
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
Suppose you mix 200.0 mL of 0.200 M RbOH(aq) with 100.0 mL of 0.400 M HBr (aq) in a coffee cup calorimeter. The initial temperature of each of the two solutions was 24.40°C and after mixing the temperature of the solution was 26.18°C. Assume the specific heat capacity of the solution is the same as water, 4.18J/(g- C) and the density of the solution is 1.0 g/mL. What is AH° (in kJ) for the reaction shown below? (Enter your answer...
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...
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