How many milliliters of 4.00M H2SO4 are required to react with 1.60g of CuO acco

Question

How many milliliters of 4.00M H2SO4 are required to react with 1.60g of CuO according to the equation

CuO(s) + H2SO4(aq) --> CuSO4(aq) + H2O(l)

Explanation / Answer

CuO + H2SO4 --> CuSO4 + H2O Convert the mass of CuO into moles: 1.60 g CuO / 79.5 g/mol = 0.0201 moles CuO From the balanced equation, you can see that you will need 0.0201 moles of H2SO4 to react. Since your H2SO4 solution is 4.00 moles/L, you will need: 0.0201 moles H2SO4 / 4.00 mol/L = 0.00503 L of H2SO4. Converting that to mL: 0.00503 L X 1000 mL/L = 5.03 mL H2SO4

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