You carry out an exothermic reaction inside a Styrofoam cup calorimeter, using a temperature probe to monitor the temperature throughout the reaction. You find that the temperature increases 7.40 °C during the reaction. The specific heat of the reaction solution is known to be 5.59 J/g•°C, and the mass of the solution was measured as 36.0 g. Calculate q, the heat for this reaction, in kJ. Be sure to include the correct sign for your answer.

What I did was the following;

q=(5.59 J/g•°C)(36.0g)(7.40)(1 kJ/ 1000 J) =1.49 kJ

however the program I am working with says I'm wrong.

Your numbers are correct. So would he reaction be -1.49kJ or 1.49kj if it is exothermic.

Your numbers are correct. So would the reaction be -1.49kJ or 1.49kj if it is exothermic.

The program still states this is incorrect

Your numbers look correct, except you should have -1.49Kj

Your calculation is almost correct, but there is a small mistake in the units conversion.

First, you correctly identified the specific heat of the reaction solution as 5.59 J/g•°C.
Next, you correctly used the formula q = (specific heat) x (mass) x (change in temperature) to calculate the heat for the reaction.

However, when converting from Joules (J) to kilojoules (kJ), you need to divide by 1000 because there are 1000 J in 1 kJ.

So, the correct calculation would be:
q = (5.59 J/g•°C) x (36.0 g) x (7.40 °C) x (1 kJ/1000 J)

Evaluating this expression gives:
q = 1.46 kJ

Therefore, the correct answer for q, the heat for this reaction, is 1.46 kJ.