When 26.1 mL of 0.500 M H2SO4 is added to 26.1 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)

ΔH = -55816 J / mol = -55.8 kJ/mol

Explanation:

Step 1: data given

Volume of a 0.500 M H2SO4 solution = 26.1 mL = 0.0261 L

Volume of a 1.00 M KOH = 26.1 mL = 0.0261 L

Temperature of the coffee cup = 23.50° C

The temperature rises to 30.17°C

Step 2: The balanced equation

H2SO4 + 2KOH → K2SO4 + 2H2O

Step 3: Calculate moles

Moles = molarity * volume

Moles H2SO4 = 0.500 M * 0.0261 L

Moles H2SO4 = 0.01305 moles

Moles KOH =1.00 M * 0.0261 L

Moles KOH = 0.0261 moles

Step 4: Calculate the limiting reactant

The mol ration is 1:2

So H2SO4 and KOH is both completely used.

Step 5: Calculate total volume

Total volume = 26.1 mL + 26.1 mL = 52.2 mL

Step 5: Calculate mass

Mass = density * volume

Mass = 52.2 mL * 1.00 g/mL

Mass = 52.2 grams

Step 6: Calculate Q

Q = c*ΔT*m

⇒c = the specific heat of water = 4.184 J/g°C

⇒ΔT = the change of temperature = 30.17 - 23.50 = 6.67 °C

⇒m = the mass = 52.2 grams

Q = 4.184 * 6.67 * 52.2

Q = 1456.8 J

As, heat change of reaction = -(Heat change of solution)

Therefore, heat change of reaction = -1456.8 J

Step 7: Calculate ΔH

There will be produced 0.0261 moles H2O

ΔH = Q / n

ΔH = -1456.8 J / 0.0261 moles

ΔH = -55816 J / mol = -55.8 kJ/mol

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

so since they all have the same shape? i mean maybe because m& m and reeses are both chocolates

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.