If a student burns 0.59 grams of methane (CH_(4)) according to the equation below, what mass of carbon dioxide will be released?Round your answer to the nearest 0.01 and remember to include units and substance! CH_(4)+2O_(2)arrow CO_(2)+2H_(2)O Your Answer: square square Answer units

## Step1: Determine the Molar Mass of Methane<br />### Calculate the molar mass of methane ($CH_4$) by summing the atomic masses of carbon (12.01 g/mol) and hydrogen (1.008 g/mol each for 4 hydrogens). The molar mass of $CH_4$ is $12.01 + 4 \times 1.008 = 16.04$ g/mol.<br /><br />## Step2: Calculate Moles of Methane Burned<br />### Use the given mass of methane (0.59 g) to find the number of moles burned using the formula: $\text{moles} = \frac{\text{mass}}{\text{molar mass}}$. Thus, $\text{moles of } CH_4 = \frac{0.59}{16.04}$.<br /><br />## Step3: Use Stoichiometry to Find Moles of Carbon Dioxide Produced<br />### According to the balanced equation, 1 mole of $CH_4$ produces 1 mole of $CO_2$. Therefore, the moles of $CO_2$ produced are equal to the moles of $CH_4$ burned.<br /><br />## Step4: Calculate Mass of Carbon Dioxide Released<br />### Calculate the mass of $CO_2$ using its molar mass (44.01 g/mol): $\text{mass of } CO_2 = \text{moles of } CO_2 \times 44.01$ g/mol.<br /><br />## Step5: Round the Result<br />### Round the calculated mass of $CO_2$ to the nearest 0.01 grams as required.