How many grams of water will be produced, if you used 60mL H2SO4 and 1.886 g CuO?
60mL H2SO4(aq) + Zn(s)----> ? H2(g) + ZnSO4(aq)
Just follow the steps in this example stoichiometry problem. Remember that moles = M x L.
To find out how many grams of water will be produced in the reaction between 60 mL of H2SO4 and 1.886 g of CuO, we first need to know the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between H2SO4 (sulfuric acid) and CuO (copper(II) oxide) is as follows:
H2SO4 + CuO -> CuSO4 + H2O
According to the chemical equation, 1 mole of H2SO4 reacts with 1 mole of CuO to produce 1 mole of CuSO4 and 1 mole of H2O.
To determine the number of moles of H2SO4 used in the reaction, we need to convert the given volume of H2SO4 from milliliters (mL) to moles using the molar volume of H2SO4.
The molar volume of H2SO4 is 98.09 g/mol, which means that one mole of H2SO4 has a mass of 98.09 grams.
Using this information, we can calculate the number of moles of H2SO4:
Number of moles of H2SO4 = Volume of H2SO4 (in liters) x molarity of H2SO4
Since the molarity of H2SO4 is not given, we cannot calculate the number of moles of H2SO4 accurately and thus cannot determine the amount of water produced in the reaction.
However, if you have the molarity of H2SO4, you can use the equation above to calculate the number of moles of H2SO4 and CuO, and then determine the amount of water produced based on the balanced chemical equation.