When 40.0 ml of 1.00 m h2so4 is added to 80.0 ml of 1.00 m naoh at 20.00°c in a coffee cup calorimeter, the temperature of the aqueous solution increases to 29.20°c. if the mass of the solution is 120.0 g and the specific heat of the calorimeter and solution is 4.184 j/g • °c, how much heat is given off in the reaction? (ignore the mass of the calorimeter in the calculation.) use q=mcp(tiangle)t 4.62 kj 10.0 kj 14.7 kj 38.5 kj

Explanation:

There are two heat transfers to consider:

Calculate q₂

 m = 120.0 g

 C = 4.184 J·°C⁻¹g⁻¹

 T₂ = 29.20 °C

 T₁ = 20.00 °C

ΔT = T₂ - T₁ =(29.20 – 20.00) °C =9.20 °C

 q₂ = 120.0 g × 4.184 J·°C⁻¹g⁻¹ × 9.20 °C = 4620 J = 4.62 kJ

Calculate q₁

q₁ + 4.62 kJ = 0

q₁ = -4.62 kJ

The negative sign shows that heat is given off.

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being