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.) 4.62 kJ 10.0 kJ 14.7 kJ 38.5 kJ

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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.) 4.62 kJ 10.0 kJ 14.7 kJ 38.5 kJ

Chemistry
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\[q = mc \Delta T\] q is the heat, in joules, given off by the reaction m is the mass of solution C is the specific heat of the solution in J/g*C T is the temperature change in degrees Celcius make sure to convert q to kJ after you're done

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