What is the value of (delta)h(reaction (in kj/mol phosphoric acid) if 50.0ml of 0.60 m h3po4 was used in the reaction described?

the reaction described is: a neutralzation raction was carried out in a calormeter, the change in temp was 5.6c and the mas of the solution was 100.0g. caculate the amount of energy gained by the soulution, using 4.18j/(gxc) as the specific heat.

ΔH = 89.6 kJ/mol phosphoric acid.

Energy gained: 2688 J

Explanation:

The heat (Q) of the reaction can be calculated by:

Q = m*c*ΔT

Where m is the mass of the solution, c is the specific heat, and ΔT is the change in temperature. If the energy is gained, thus Q>0, and also ΔH >0, and the reaction is endothermic.

Q = 100*4.18*5.6

Q = 2688 J

The change in enthalpy is the heat divided by the number of moles. Because it's related to the phosphoric acid, it will be the number of moles of it, which is the volume (50.0 mL = 0.05 L) multiplied by the concentration (0.60 M).

n = 0.05 * 0.60 = 0.03 mol of H3PO4

ΔH = 2688/0.03

ΔH = 89600 J/mol

ΔH = 89.6 kJ/mol phosphoric acid.

possibly, yes.

explanation:

the amount of sugar you take in is dangerously high, risk of heart disease, high risk of diabetes, and etc.

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.