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In a constant‑pressure calorimeter, 60.0 mL of 0.920 M H 2 SO 4 was added to...

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Chemistry

In a constant‑pressure calorimeter, 60.0 mL of 0.920 M H 2 SO 4was added to 60.0 mL of 0.360 M NaOH . The reaction caused thetemperature of the solution to rise from 22.43 ∘ C to 24.88 ∘ C. Ifthe solution has the same density and specific heat as water ( 1.00g / mL and 4.184 J / ( g ⋅ °C), respectively), what is Δ H for thisreaction (per mole of H 2 O produced)? Assume that the total volumeis the sum of the individual volumes.

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3.9 Ratings (803 Votes)
First to say mL x M mL x mol L mL L x mol 103 molSince NaOH used is much lower than theH2SO4 so NaOH is the terminal reagent and itwill decide the amount of water produced Since one    See Answer
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