The reaction between naoh(aq) and h2so4(aq) was studied in a constant-pressure calorimeter: 100.0 ml portions of 1.00 m aqueous naoh and h2so4, each at 24.0c, were mixed. the volume of the mixture was 200.0 ml. the maximum temperature achieved was 30.6c. neglect the heat capacity of the calorimeter and the thermometer, and assume that the solution of products has a density of 1.00 g/ml and a specific heat capacity of 4.18 j/(g·k). calculate h, the heat (enthalpy) of reaction, in kj per mole of acid. (hint: you may not have the equivalent amounts of naoh and h2so4 in this experiment.)

110,4 kJ / mole of acid

Explanation:

The reaction of NaOH with H₂SO₄ is:

2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

Moles of NaOH and H₂SO₄ are:

0,1000L×1,00M = 0,100 moles of NaOH and 0,100 moles of H₂SO₄. As 2 moles of NaOH reacts with 1 mole of  H₂SO₄, moles of acid that react are 0,100/2 = 0,0500moles of acid.

The produced heat is:

Q = C×m×ΔT

Where C is specific heat capacity (4,18J/gK)

m is mass: 200,0mL×(1,00g/mL) = 200g

ΔT is change in temperature: 30,6°C - 24,0°C = 6,6°C = 6,6K

Thus, Q is:

Q = 4,18J/gK×200g×6,6K

Q = 5518J = 5,52kJ

ΔH in kJ per mole of acid:

5,52kJ / 0,0500moles of acid = 110,4 kJ / mole of acid

I hope it helps!

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation: