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…

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 = mcₚδt.\n4.62 kj\n10.0 kj\n14.7 kj\n38.5 kj

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 = mcₚδt.\n4.62 kj\n10.0 kj\n14.7 kj\n38.5 kj

Answer

Answer:

4.62 kJ

Explanation:

Step1: Identify given values

$m = 120.0$ g, $C_p=4.184$ J/g·°C, $\Delta T=29.20 - 20.00=9.20$ °C

Step2: Apply heat - transfer formula

$q = mC_p\Delta T$ $q=120.0\times4.184\times9.20$ $q = 120.0\times38.4928$ $q = 4619.136$ J

Step3: Convert to kJ

$q=\frac{4619.136}{1000}=4.619136\approx4.62$ kJ