Questions: A certain chemical reaction releases 16.7 kJ / g of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 1.1 kg 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. heat =

A certain chemical reaction releases 16.7 kJ / g of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 1.1 kg 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.

heat =

Transcript text: A certain chemical reaction releases $16.7 \mathrm{~kJ} / \mathrm{g}$ of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 1.1 kg 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. \[ \text { heat }= \] $\square$ $\square$ $\times 10$ $\mu$ $\square \cdot$ - $\square$ $\square$

Solution

Solution Steps

Step 1: Identify the given values

We are given the heat released per gram of reactant and the total mass of the reactant consumed. Specifically:

Heat released per gram of reactant: $ 16.7 \, \mathrm{kJ/g} $
Mass of reactant consumed: $ 1.1 \, \mathrm{kg} $

Step 2: Convert mass to grams

Since the heat released is given per gram, we need to convert the mass of the reactant from kilograms to grams: \[ 1.1 \, \mathrm{kg} = 1.1 \times 1000 \, \mathrm{g} = 1100 \, \mathrm{g} \]

Step 3: Set up the expression for total heat produced

The total heat produced can be calculated by multiplying the heat released per gram by the total mass in grams: \[ \text{heat} = 16.7 \, \mathrm{kJ/g} \times 1100 \, \mathrm{g} \]