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Moles of Reactant to Moles of Product: Use mole ratio from balanced chemical equation. 1.Ammonia burns...

Moles of Reactant to Moles of Product: Use mole ratio from balanced chemical equation.

1.Ammonia burns in oxygen according to the following equation:


4 NH3 + 3 O2  → 2 N2 + 6 H2O


How many moles of nitrogen gas are generated by the complete reaction of 8.23 moles of ammonia? Express your answer to two decimal places.

mol N2

2.

Moles of Product to Moles of Reactant: Use mole ratio from balanced chemical equation.

The commercial process used to make nitric acid is as follows:


3 NO2(g) + H2O(l)  → 2 HNO3(aq) + NO(g)


How many moles of nitrogen dioxide are required to produce 7.19 moles of nitric acid? Express your answer to two decimal places.

mol NO2

3.

Moles of Reactant to Mass of another Reactant: Balance equation. Use mole ratio, then convert to grams.

Balance the chemical equation showing the reaction of sulfuric acid with calcium phosphate to produce phosphoric acid and calcium sulfate:


Ca3(PO4)2(s) +   H2SO4(aq)  →   CaSO4(s) +   H3PO4(aq)


What mass of calcium phosphate is needed to completely reacted with 6.665 moles of sulfuric acid? Express your answer to two decimal places.

g Ca3(PO4)2

4.

Moles of Product to Mass of Each Reactant: Perform a separate calculation for each reactant. Use mole ratio, then convert to grams.

If 0.63 moles of carbon monoxide gas are produced by the following reaction, how many grams of silicon dioxide and of carbon were reacted (assume just enough of each)? Express your answer to two decimal places.


SiO2(s) + 2 C(s)  → Si(l) + 2 CO(g)


Mass of SiO2 needed:  g

Mass of C needed:  g

5.

Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams.

A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction:


O3(g) + 2 I-(aq) + H2O(l)  → O2(g) + I2(aq) + 2 OH-(aq)


How many grams of ozone can be removed from the air sample if 5.11 moles of iodide ions are present in the bubbler? Express your answer to two decimal places.

g

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Expert Solution

queen_honey_blossom answered 10 months ago
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