Answer to Question #59860 in Organic Chemistry for johnny

Question #59860
In experiment 1, you study a neutralization reaction involving an acid and a base.

Oxalosuccinic acid (H3C6H3O7) is a tricarboxylic acid.

It reacts with NaHCO3 (sodium bicarbonate or "baking soda") to yield carbon dioxide, water and sodium oxalosuccinate (Na3C6H3O7).

Balance the following reaction:

H3C6H3O7(aq) + 3NaHCO3(s) = 3CO2(g) + 3H2O(l) + Na3C6H3O7(aq)

A student measures 11.41 g of baking soda and adds this to 24. mL of 3.0 M oxalosuccinic acid (in an alcoholic solution).

Identify the limiting reagent and calculate the number of moles of CO2 produced.

The limiting reagent is: sodium bicarbonate.

1.358×10-1 mol of CO2 are produced.

Hypothetically, if the temperature of the solution goes from 25.0°C to 8.0°C the reaction is considered

Calculate the temperature change per mole of H+ which reacted.

ΔT/(mol H+ reacted) = K/mol
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