How many liters of 1.20 M calcium nitrate are required to produce .1 moles of calcium sulfate? Please balance the equation before solving the problem.

0.083L

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

Ca(NO3)2 + H2SO4 —> CaSO4 + 2HNO3

Next, we shall determine the number of mole of Ca(NO3)2 needed to produce 0.1 mole of CaSO4.

From the balanced equation above,

1 mole of Ca(NO3)2 reacted to produce 1 mole of CaSO4.

Therefore, 0.1 mole of Ca(NO3)2 will also react to produce 0.1 mole of CaSO4.

Finally, we can determine the volume of Ca(NO3)2 needed for the reaction as follow:

Mole of Ca(NO3)2 = 0.1 mole

Molarity of Ca(NO3)2 = 1.20M

Volume =?

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 0.1/1.2

Volume = 0.083L

Therefore, 0.083L of Ca(NO3)2 is needed for the reaction.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong