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.\n\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.\n\n4.62 kj\n10.0 kj\n14.7 kj\n38.5 kj

Answer

Explanation:

Step1: Identify given values

$m = 120.0\ g$, $C_p=4.184\ J/g\cdot^{\circ}C$, $\Delta T=T_{final}-T_{initial}=29.20^{\circ}C - 20.00^{\circ}C = 9.20^{\circ}C$

Step2: Apply heat - transfer formula

$q = mC_p\Delta T$ Substitute the values: $q=120.0\ g\times4.184\ J/g\cdot^{\circ}C\times9.20^{\circ}C$ $q = 120.0\times4.184\times9.20\ J$ $q = 4619.328\ J$

Step3: Convert to kJ

Since $1\ kJ = 1000\ J$, then $q=\frac{4619.328\ J}{1000}=4.619328\ kJ\approx4.62\ kJ$

Answer:

4.62 kJ