Question

How many moles of calcium hydroxide are needed to produce 73.7 milliliters of water, if the density of water is 0.987 g/mL?

HCl + Ca(OH) 2 ---> H2O + CaCl2
@Abhisar

Answer 1

2 HCl + Ca(OH)2 → 2 H2O + CaCl2
Mass of water: m=d*v
=.987 * 73.7 = 72.74
Molar mass of water is Hydrogen ((1.008) * 2) + Weight for 1 Oxygen (15.999) = 18.015
72.74g/18.015 = 4.04 mol
Mole of CaCl2 = 4.04 mol / 2 = 2.02 moles Ca(OH)2

Answer 2

The question marks are an arrow

Answer 3

Give me a sec..

Answer 4

Ok

Answer 5

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Answer 6

Could you check one other?

Answer 7

yes...go ahead

Answer 8

How many milliliters of magnesium metal, with a density of 1.74 g/mL, are needed to produce 102.3 grams of magnesium oxide in the single-replacement reaction below?

Mg + H2O ----> MgO + H2

Atomic Mass of Mg = 24.3050
Atomic Mass of Oxygen = 15.9994
Molar Mass of MgO = 24.3050 + 15.9994 = 40.3044 g/mol
102.3g/40.3044 g/mol = 2.54 moles Mg
2.54 moles Mg x 24.3050/mole = 61.7347 g Mg
V = mass / density
61.7347 g / 1.74 g/mL = 35.4797 mL

Answer 9

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Answer 10

Thank you!

Answer 11

ur most welcome :)