What is the volume of 6M H2SO4 required by the balanced equation to react with the CuO to produce 0.025 moles of copper(ii) sulfate. Report the volume needed BEFORE allowing for excess in milliliters to two significant figures. Don not include units in the answer box.
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CuO + H2SO4 ==> CuSO4 + H2O
You want 0.025 mols CuSO4 so you must have start with 0.025 mols H2SO4 (from the coefficients in the balanced equation).
Then M H2SO4 = mols H2SO4/L H2SO4. You know M and mols, solve for L and convert to mL. I have no idea what "allowing for excess" means in this problem. I suspect you didn't type all of the problem.
To find the volume of 6M H2SO4 required, we need to use the balanced equation and the stoichiometry of the reaction.
The balanced equation is:
CuO + H2SO4 → CuSO4 + H2O
From the equation, we can see that the stoichiometric ratio between CuO and CuSO4 is 1:1. This means that for every mole of CuO reacted, we will produce one mole of CuSO4.
Given that we want to produce 0.025 moles of CuSO4, we need an equal amount of CuO. Therefore, we have:
0.025 moles CuO = 0.025 moles CuSO4
Now, let's calculate the volume of 6M H2SO4 required to react with 0.025 moles of CuO.
To do this, we need to use the following formula:
Volume (in liters) = moles / concentration (in moles per liter)
Let's plug in the values:
Volume = 0.025 moles / 6 moles per liter
Volume ≈ 0.00417 liters
Finally, we need to convert the volume from liters to milliliters:
Volume ≈ 0.00417 liters * 1000 milliliters per liter
Volume ≈ 4.17 milliliters
Therefore, the volume of 6M H2SO4 required, before allowing for excess, is approximately 4.17 milliliters.
To find the volume of 6M H2SO4 required, we need to use the balanced equation and stoichiometry.
The balanced equation for the reaction is:
CuO + H2SO4 -> CuSO4 + H2O
From the balanced equation, we can see that the stoichiometric ratio between CuO and CuSO4 is 1:1. This means that 1 mole of CuO will produce 1 mole of CuSO4.
Given that we have 0.025 moles of CuSO4, we can conclude that we need an equivalent amount of CuO. Therefore, we also have 0.025 moles of CuO.
Now, let's use the molar ratio between CuO and H2SO4 to find the volume of 6M H2SO4 required. The molar ratio is 1:1, which means that 1 mole of CuO requires 1 mole of H2SO4.
Since the concentration of H2SO4 is given as 6M (moles per liter), we can convert the number of moles of H2SO4 required to the volume by using the formula:
Volume (in liters) = Moles / Concentration
Volume = 0.025 moles / 6 M = 0.00417 liters
To convert the volume to milliliters, multiply by 1000:
Volume = 0.00417 liters * 1000 = 4.17 mL
Therefore, the volume of 6M H2SO4 required, before allowing for excess, is 4.17 mL (to two significant figures).