(II)
Let's start by writing the neutralization reaction in case we need it later:
HCl + NaOH -> H2O + NaCl
Now, we will use the calorimeter/specific heat formula:
q = mcΔT
We have c = 4.18J/gK and we also have ΔT=6.5K, we need to calculate m (but we have volume and density) so m=100g.
Now we just substitute the values in the formula and we get a q = 2717J but that isn't the final answer because we didn't use 1 mole of HCl, so we need to calculate how many moles we used. In this case we used 0.05moles HCl. So to get ΔH we need to divide q/moles (be very careful to include the negative sign in q because this heat is released).
So, the final answer is ΔH = - 54.34 kJ/mol
MCQ A student mixes 30.0 mL of an NaOH solution originally at a temperature of 25.0 degrees Celsius with 30.0 mL of HCl at the same temperature in a coffee cup calorimeter with a heat capacity of 50.0 J/C. The final temperature of the mixture is 27.0 C. Which of the following equations calculates the heat of the calorimeter? a) 50.0 J/C x 2 C b) 30.0 g x 50.0J/C x 2 C c) 60.0 g x 4.18...
24 Question (1 point) @ See page 236 A 67.0 mL sample of 1.0 M NaOH is mixed with 41.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 27.5°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is...
A 71.0 mL sample of 1.0 M NaOH is mixed with 40.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.3°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0 g/mL, that the specific heat of the...
A 65.0 mL sample of 1.0 M NaOH is mixed with 48.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 24.4°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0 g/mL, that the specific heat of the...
A 68.0 mL sample of 1.0 M NaOH is mixed with 49.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.2°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0 g/mL, that the specific heat of the...
Page 36 When 50.0 mL of 1.00 M HCI(aq) and 50.0 mL of 1.00 M NaOH(aq), both at 22.0 °C, are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 28.9 C. What is the approximate amount of heat produced by this reaction? Specific heat of water is 4.184 J/g C HCl(aq) + NaOH(aq) → Nacl(aq) + H2O() The heat given off by the reaction is equal to that taken in by the solution....
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 coffee cup calorimeter. If both solutions were initially at 35.0°C and the temperature of the resulting solution was recorded as 37.0°C, determine the experimental AHxt (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCI. Assume that no heat is lost to the calorimeter or the surroundings, and that the density of the solution is...
5. 0.20 L of a 0.40 M HCI is totally reacted with 0.20 L of a NaOH solution in a Styrofoam coffee cup. The temperature of both solutions before mixing is 25.1 °C and 26.6 °C after. Assume that both the HCI and the NaOH solutions have a density of 1.00 g/mL, the heat absorbed by the cup is negligible, and the specific heat capacity of the solutions is 4.18 J/g C. Calculate the heat released per mol HCl in...
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
24 Question (1 point) See page 236 A 70.0 mL sample of 1.0 M NaOH is mixed with 43.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 29.8°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0...