Is my answer correct?
Calculate the mass of frost (water ice) on a piece of dry ice that would completely
react with 2 mmol of phenylmagnesium bromide.
(1/44 CO2)*(0.002mol of phenylmagnesium bromide)= 0.0000455
To calculate the mass of frost on a piece of dry ice that would completely react with 2 mmol of phenylmagnesium bromide, you need to set up a balanced chemical equation for the reaction and then use stoichiometry to convert between moles of reactant and product.
The balanced chemical equation for the reaction between phenylmagnesium bromide and dry ice (CO2) is:
C6H5MgBr + CO2 → C6H6 + MgBr2
From the equation, we can see that for every 1 mole of phenylmagnesium bromide (C6H5MgBr), 1 mole of CO2 reacts to form 1 mole of benzene (C6H6) and 1 mole of magnesium bromide (MgBr2).
Given that you have 2 mmol of phenylmagnesium bromide, you need to convert this amount into moles:
2 mmol x 0.001 mol/mm = 0.002 mol
Now, using the stoichiometry from the balanced equation, we know that 1 mole of phenylmagnesium bromide reacts with 1 mole of CO2. Therefore, the number of moles of CO2 required to completely react with 0.002 mol of phenylmagnesium bromide is also 0.002 mol.
Now, to calculate the mass of CO2 (frost) needed, we can use the molar mass of CO2, which is 44 g/mol:
Mass = Number of moles x Molar mass
Mass = 0.002 mol x 44 g/mol
Mass = 0.088 g
So, the mass of frost (water ice) on the piece of dry ice that would completely react with 2 mmol of phenylmagnesium bromide is 0.088 grams.
Therefore, your answer of 0.0000455 g is incorrect.