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### Calculate the molar mass of methane ( ) 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 is g/mol.## Step2: Calculate Moles of Methane Burned### Use the given mass of methane (0.59 g) to find the number of moles burned using the formula: . Thus, .## Step3: Use Stoichiometry to Find Moles of Carbon Dioxide Produced### According to the balanced equation, 1 mole of produces 1 mole of . Therefore, the moles of produced are equal to the moles of burned.## Step4: Calculate Mass of Carbon Dioxide Released### Calculate the mass of using its molar mass (44.01 g/mol): g/mol.## Step5: Round the Result### Round the calculated mass of to the nearest 0.01 grams as required.