Question

A certain chemical reaction releases 13.8 Kj/g of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 2.1kg of reactant?

Set the math up. But don't do any of it. Just leave your answer as a math expression.

Also, be sure your answer includes all the correct unit symbols.

Answer 1

28,980 kJ is the heat produced by the consumption of 2.1 kg of reactant.

Explanation:

In a chemical reaction, 13.8 Kj/g of heat for 1 gram of reactant consumed.

Heat released when 1 gram of reactant is used = 13.8 kJ

Heat released when 1 gram of 2.1 kg of reactant is used:

Mass of the reactant 2.1 kg ,m= 2100 g (1 kg = 1000 g)

Heat released when 1 gram of 2100 g of reactant is used:Q

`Q=13.8 kJ* m`

`=13.8 kJ* m=13.8 kJ* 2100 g=28,980 kJ`

28,980 kJ is the heat produced by the consumption of 2.1 kg of reactant.

Answer 2

Here's what I get.

Step-by-step explanation:

Convert kilograms to grams and then to kilojoules.

Heat released}= 2.1 kg × (1000 g/1 kg) × (13.8 kJ/1 g)