A chemist measures the energy change ΔH during the following reaction:CH4(g)+2O2(g)→CO2(g)+2H2O(l) =ΔH−882.kJUse the information to answer the following question.Suppose 66.0g of CH4 react.Calculate how much heat will be released or absorbed.kJBe sure your answer has the correct number of significant digits.
Question
A chemist measures the energy change ΔH during the following reaction:CH4(g)+2O2(g)→CO2(g)+2H2O(l) =ΔH−882.kJUse the information to answer the following question.Suppose 66.0g of CH4 react.Calculate how much heat will be released or absorbed.kJBe sure your answer has the correct number of significant digits.
Solution
First, we need to determine the number of moles of CH4. We know that the molar mass of CH4 is approximately 16.04 g/mol.
So, the number of moles of CH4 is given by:
moles = mass / molar mass moles = 66.0 g / 16.04 g/mol = 4.11 mol
The balanced chemical equation tells us that 1 mol of CH4 releases 882 kJ of heat. Therefore, 4.11 mol of CH4 will release:
heat = ΔH * moles heat = -882 kJ/mol * 4.11 mol = -3622.2 kJ
The negative sign indicates that the heat is released. Therefore, 3622 kJ of heat will be released.
However, we need to consider the significant figures. The least number of significant figures given in the problem is three (from the 66.0 g of CH4). Therefore, we should round our answer to three significant figures:
heat = -3620 kJ
So, 3620 kJ of heat will be released.
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